Oxford International AQA Examinations IGCSE Science 9204 Specification
AQA INTERNATIONAL
GCSE
COMBINED SCIENCE -
DOUBLE AWARD
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BIOLOGY
(Oxford AQA International GCSE Combined Science Double award)
ORGANISATION
(Oxford AQA International GCSE Combined Science Double award)
All organisms are constituted of one or more cells. Multi–cellular organisms
have cells that are differentiated
according to their function.
All the basic functions of life are the result of what happens inside the cells
which
make up an organism. Growth is the result of multiple cell divisions.
Cell structure
(Oxford AQA International GCSE Combined Science Double award)
a.
Most animal cells (eukaryotic cells) have the following parts:
•
a nucleus, which controls the activities of the cell
•
cytoplasm, in which most of the chemical reactions take place
•
a cell membrane, which controls the passage of substances into and out of the
cell
•
mitochondria, which is where most energy is released in respiration
•
ribosomes, which is where protein synthesis occurs.
b.
In addition to the above, plant cells (eukaryotic cells) often have:
•
chloroplasts, which absorb light energy to make food
•
a permanent vacuole filled with cell sap.
Plant and algal cells also have a cell wall made of cellulose, which strengthens
the cell.
c.
A bacterial cell (prokaryotic cell) consists of cytoplasm and a membrane
surrounded by a cell wall; the
genes are not in a distinct nucleus; some of the genes are located in circular
structures called plasmids.
d.
Cells may be specialised to carry out a particular function.
Students should be able, when provided with appropriate information, to relate
the structure of different
types of cell to their function in a tissue, an organ, or the whole organism.
Introduction to plant and animal cell structure and
function - comparison of subcellular structures
Principles of organisation
(Oxford AQA International GCSE Combined Science Double award)
a.
Large multicellular organisms develop systems for exchanging materials. During
the development of a
multicellular organism, cells differentiate so that they can perform different
functions.
b.
A tissue is a group of cells with similar structure and function.
c.
Organs are made of tissues. One organ may contain several tissues.
d.
Organ systems are groups of organs that perform a particular function.
Students should develop an understanding of size and scale in relation to cells,
tissues, organs and systems
Introduction to the organisation of cells =>
tissues => organs => organ systems (e.g. in humans)
Animal tissues, organs and organ systems
(Oxford AQA International GCSE Combined Science Double award)
a.
Examples of animal tissues include:
•
muscular tissue, which can contract to bring about movement
•
glandular tissue, which can produce substances such as enzymes and hormones
•
epithelial tissue, which covers some parts of the body.
b.
An example of an animal organ is the stomach, which contains:
•
muscular tissue, to allow contents to move through the digestive system
•
glandular tissue, to produce digestive juices
•
epithelial tissue, to cover the outside and the inside of the stomach.
c.
An example of an animal organ system is the digestive system, a system in which
humans and other
mammals exchange substances with the environment. The digestive system includes:
•
glands, such as the pancreas and salivary glands, which produce digestive juices
•
the stomach and small intestine, where digestion occurs
•
the liver, which produces bile
•
the small intestine, where the absorption of soluble food occurs
•
the large intestine, where water is absorbed from the undigested food, producing
faeces.
Enzymes - structure, functions, optimum conditions,
investigation experiments, human digestion system
Plant tissues, organs and systems
(Oxford AQA International GCSE Combined Science Double award)
a.
Examples of plant tissues include:
•
epidermal tissues, which cover the plant
•
palisade mesophyll, which carries out photosynthesis
•
spongy mesophyll, which has air spaces to facilitate diffusion of gases
•
xylem and phloem, which transport substances around the plant.
b.
Plant organs include stems, roots and leaves.
Details of the internal structure of these organs are limited to the leaf and to
the position of the xylem and
phloem in a dicotyledonous primary root and primary stem
Plant cells - transport, gas exchange,
transpiration & experiments, absorption of nutrients, leaf & root structure
Transport in cells
(Oxford AQA International GCSE Combined Science Double award)
The movement of substances into and out of cells.
a.
Diffusion is the spreading of the particles of any substance in solution, or
particles of a gas, resulting in
a net movement from an area of higher concentration to an area of lower
concentration. The greater the
difference in concentration, the faster the rate of diffusion.
b.
Dissolved substances can move into and out of cells by diffusion.
c.
Oxygen required for respiration passes through cell membranes by diffusion.
d.
Osmosis is the diffusion of water from a dilute to a more concentrated solution
through a selectively
permeable membrane that allows the passage of water molecules.
e.
Differences in the concentrations of the solutions inside and outside a cell
cause water to diffuse into or
out of the cell by osmosis.
Students should be familiar with experiments related to diffusion and osmosis as
well as the terms isotonic,
hypertonic, turgor and plasmolysis.
f.
Substances are sometimes absorbed against a concentration gradient. This
requires the use of energy from
respiration. The process is called active transport.
g.
Active transport enables plants to absorb ions from very dilute solutions, eg by
root hair cells. Similarly,
sugar may be absorbed from low concentrations in the intestine and from low
concentrations in the kidney
tubules.
h.
A single-celled organism has a relatively large surface area to volume ratio.
All the necessary exchanges
occur across its surface membrane.
The increased size and complexity of an organism increases the difficulty of
exchanging materials.
i.
In multicellular organisms many organ systems are specialised for exchanging
materials. The effectiveness
of an exchange surface is increased by:
•
having a large surface area that is thin, to provide a short diffusion path
•
(in animals) having an efficient blood supply
•
(in animals, for gaseous exchange) being ventilated.
Students should be able to explain how the small intestine and lungs in mammals,
and the roots and leaves
in plants, are adapted for exchanging materials.
j.
Gas and solute exchange surfaces in humans and other organisms are adapted to
maximise effectiveness.
Students should be able to explain how gas and solute exchange surfaces are
adapted to maximise
effectiveness
Diffusion, osmosis, active transport, exchange of
substances - examples fully explained
BIOENERGETICS AND ECOLOGY
(Oxford AQA International GCSE Combined Science Double award)
Food provides materials and energy for organisms to carry out the basic
functions of life and to grow. Some
plants
and bacteria are able to use energy from the Sun to generate complex food
molecules. Animals obtain
energy by breaking down complex food molecules and are ultimately dependent on
green plants for energy.
In any ecosystem there is competition among species for the energy and materials
they need to live and
reproduce.
BIOENERGETICS
(Oxford AQA International GCSE Combined Science Double award)
Photosynthesis
(Oxford AQA International GCSE Combined Science Double award)
a.
Photosynthesis is summarised by the equations:
carbon dioxide + water == light ==>
glucose + oxygen
6CO2
+ 6H2O
== light ==>
C6H12O6
+ 6O2
b.
During photosynthesis:
•
light is absorbed by a green substance called chlorophyll, which is found in
chloroplasts in some plant
cells and in algae
•
light is used to convert carbon dioxide (from the air) and water (from the soil)
into sugar (glucose)
•
oxygen is released as a by-product.
c.
The rate of photosynthesis may be limited by:
•
low temperature
•
shortage of carbon dioxide
•
shortage of light.
These factors interact and any one of them may be the factor that limits
photosynthesis.
Students should be able to relate the principle of limiting factors to the
economics of enhancing the
following conditions in greenhouses
including
temperature,
carbon dioxide concentration and
light intensity.
Required practical:
Investigate how variables affect the rate of photosynthesis.
d.
The glucose produced in photosynthesis may be used as a source of chemical
energy or converted to larger
molecules for storage and use later. The glucose can be:
•
used for respiration
•
converted into insoluble starch for storage
•
used to produce fat or oil for storage
•
used to produce cellulose, which strengthens the cell wall
•
used to produce proteins.
e.
To produce proteins, plants also use nitrate ions that are absorbed from the
soil
Photosynthesis,
importance
explained, limiting factors affecting rate, leaf adaptations
Circulation in humans
(Oxford AQA International GCSE Combined Science Double award)
a.
Substances are transported from where they enter the body to the cells, or from
the cells to where they are
removed from the body, by the circulatory system (the heart, the blood vessels
and the blood).
b.
The heart is an organ that pumps blood around the body in a double circulatory
system. Much of the wall of
the heart is made from muscle tissue.
c.
The heart has four main chambers (right and left atria and right and left
ventricles).
d.
Blood enters the atria of the heart. The atria contract and force blood into the
ventricles. The ventricles
contract and force blood out of the heart. Valves in the heart ensure that blood
flows in the correct
direction.
Knowledge of the names of the heart valves is not required.
e.
Blood flows from the heart to the organs through arteries and returns through
veins. There are two
separate circulation systems, one for the lungs and one for all other organs of
the body.
Knowledge of the blood vessels associated with the heart is limited to aorta,
vena cava, pulmonary artery,
pulmonary vein and coronary arteries.
f.
Arteries have thick walls containing muscle and elastic fibres. Veins have
thinner walls and often have
valves to prevent back-flow of blood.
g.
In the organs, blood flows through very narrow, thin-walled blood vessels called
capillaries. Substances
needed by the cells in body tissues pass out of the blood and substances
produced by the cells pass into
the blood, through the walls of the capillaries.
h.
Blood is a tissue consisting of a fluid called plasma, in which the white blood
cells, platelets and red blood
cells are suspended.
i.
Blood plasma transports:
•
carbon dioxide from the organs to the lungs
•
soluble products of digestion from the small intestine to other organs
•
urea from the liver to the kidneys.
j.
Red blood cells have no nucleus. They are packed with a red pigment called
haemoglobin. Red blood cells
transport oxygen from the lungs to the organs. In the lungs haemoglobin combines
with oxygen to form
oxyhaemoglobin. In other organs oxyhaemoglobin splits up into haemoglobin and
oxygen.
k.
White blood cells have a nucleus. They form part of the body’s defence system
against microorganisms.
l.
Platelets are small fragments of cells. They have no nucleus. Platelets help
blood to clot at the site of a
wound.
m.
Blood clotting is a series of enzyme-controlled reactions, resulting in the
change of fibrinogen to fibrin,
which forms a network of fibers (fibres) trapping blood cells and forming a
clot.
n.
Antigens are proteins on the surface of cells
The human circulatory system - heart, lungs, blood,
blood cells/vessels, causes/treatment of cardiovascular disease
Digestion
(Oxford AQA International GCSE Combined Science Double award)
a.
Starch (a carbohydrate), proteins and fats are insoluble. They are broken down
into soluble substances
so that they can be absorbed into the bloodstream in the wall of the small
intestine. In the large intestine
much of the water mixed with the food is absorbed into the bloodstream. The
indigestible food which
remains makes up the bulk of the faeces. Faeces leave the body via the anus.
Students should be able to recognise the following on a diagram of the digestive
system: salivary glands,
oesophagus, stomach, liver, gall bladder, pancreas, duodenum, small intestine,
large intestine, anus.
b.
Enzymes help the breakdown of food in the digestive system.
•
Enzymes are large proteins that act as biological catalysts. Catalysts increase
the rate of chemical
reactions and are utilized in the digestive process to speed up the breakdown of
large molecules to
small molecules for absorption into the bloodstream.
•
The shape of an enzyme is vital for the enzyme’s function. High temperatures
denature the enzyme,
changing the shape of the active site.
•
Different enzymes work best at different pH values.
•
Some enzymes work outside the body cells. The digestive enzymes are produced by
specialised cells
in glands and in the lining of the gut. The enzymes then pass out of the cells
into the gut, where they
come into contact with food molecules. They catalyse the breakdown of large
molecules into smaller
molecules
c.
Digestive enzymes.
•
The enzyme amylase is produced in the salivary glands, the pancreas and the
small intestine. Amylase
catalyses the breakdown of starch into sugars in the mouth and small intestine.
•
Protease enzymes are produced by the stomach, the pancreas and the small
intestine. These enzymes
catalyse the breakdown of proteins into amino acids in the stomach and the small
intestine.
•
Lipase enzymes are produced by the pancreas and small intestine. These enzymes
catalyse the
breakdown of lipids into fatty acids and glycerol in the small intestine.
•
The stomach also produces hydrochloric acid. The enzymes in the stomach work
most effectively in acid
conditions.
•
The liver produces bile, which is stored in the gall bladder before being
released into the small intestine.
Bile neutralises the acid that was added to food in the stomach. This provides
alkaline conditions in
which enzymes in the small intestine work most effectively.
•
Bile also emulsifies fats (breaks large drops of fats into smaller droplets).
This increases the surface area
of fats for lipase enzymes to act upon.
Enzymes - section on
human digestion, metabolism and synthesis
Breathing
(Oxford AQA International GCSE Combined Science Double award)
a.
The respiratory (breathing) system takes air into and out of the body so that
oxygen from the air can
diffuse into the bloodstream and carbon dioxide can diffuse out of the
bloodstream into the air. The lungs
are in the upper part of the body (thorax), protected by the ribcage and
separated from the lower part of
the body (abdomen) by the diaphragm.
Students should be able to recognise the following on a diagram of the
respiratory system: ribs, intercostal
muscles, diaphragm, lungs, trachea, bronchi, bronchioles, alveoli.
b.
To inhale:
•
the intercostal muscles contract, pulling the ribcage upwards
•
at the same time the diaphragm muscles contract, causing the diaphragm to
flatten
•
these two movements cause an increase in the volume of the thorax
•
the consequent decrease in pressure to below that of the air surrounding the
body results in
atmospheric air entering the lungs.
To exhale:
•
the intercostal muscles relax, allowing the rib cage to move downwards
•
at the same time the diaphragm muscles relax, allowing the diaphragm to resume
its domed shape
•
these two movements cause a reduction in the volume of the thorax
•
the consequent increase in pressure results in air leaving the lungs.
c.
The alveoli provide a very large surface area, richly supplied with blood
capillaries, so that gases can readily
diffuse into and out of the blood.
Examples of surfaces for the exchange of substances in
animal organisms
Respiration
(Oxford AQA International GCSE Combined Science Double award)
a.
Respiration in cells can take place aerobically (using oxygen) or anaerobically
(without oxygen), to transfer
energy.
b.
During aerobic respiration chemical reactions occur that use glucose (a sugar)
and oxygen and transfer
energy.
c.
Aerobic respiration is summarised by the equations:
glucose
+
oxygen ==>
carbon dioxide
+
water
(+ energy)
C6H12O6
+
6O2==>
6CO2
+
6H2O
(+ energy)
d.
Aerobic respiration takes place continuously in both plants and animals.
e.
Most of the reactions in aerobic respiration take place inside mitochondria.
f.
The energy that is transferred during respiration may be used by the organism in
a variety of ways:
•
to build larger molecules from smaller ones
•
in animals, to enable muscles to contract
•
in mammals and birds, to maintain a steady body temperature in colder
surroundings
•
in plants, to build up sugars, nitrates and other nutrients into amino acids,
which are then built up into
proteins.
g.
During exercise the human body needs to react to the increased demand for
energy. A number of changes
take place:
•
the heart rate increases, increasing blood flow to the muscles
•
the rate and depth of breathing increase
•
glycogen stored in the muscles is converted back to glucose.
h.
These changes increase the supply of glucose and oxygen to, and increase the
rate of removal of carbon
dioxide from, the muscles.
i.
If insufficient oxygen is reaching the muscles, energy is transferred by
anaerobic respiration.
glucose ==>
lactic acid
C6H12O6
==>
2C3H6O3
j.
Anaerobic respiration in muscles is the incomplete breakdown of glucose, which
causes a build-up of lactic
acid.
An oxygen debt needs to be repaid to oxidise the lactic acid to carbon dioxide
and water.
k.
As the breakdown of glucose is incomplete, much less energy is transferred in
anaerobic respiration than
during aerobic respiration.
l.
During long periods of vigorous activity muscles become fatigued and stop
contracting efficiently. One
cause of muscle fatigue is the build-up of lactic acid in the muscles. Blood
flowing through the muscles
eventually removes the lactic acid.
Required practical:
Investigate the effects of exercise on the human body.
m.
Anaerobic respiration in plant cells and in some microorganisms results in the
production of ethanol and
carbon dioxide.
Respiration - aerobic and anaerobic in plants and animals,
investigations
ECOLOGY
(Oxford AQA International GCSE Combined Science Double award)
Materials including carbon and water are continually recycled by the living
world, being released through
respiration of animals, plants and decomposing microorganisms and taken up by
plants in photosynthesis. All
species live in ecosystems composed of complex communities of animals and plants
dependent on each other
and that are adapted to particular conditions, both abiotic and biotic.
Energy transferred in ecosystems
(Oxford AQA International GCSE Combined Science Double award)
a.
Radiation from the Sun is the source of energy for most communities of living
organisms. Plants and
algae transfer about 1
% of the incident energy from light for photosynthesis. This energy is stored in
the
substances that make up the cells of the plants.
b.
Only approximately 10
% of the biomass from each trophic level is transferred to the level above it
because:
•
some materials and energy are always lost in the organisms’ waste materials
•
respiration supplies all the energy needs for living processes, including
movement. Much of this energy
is eventually transferred to the surroundings.
Construction of food webs and chains, and of pyramids of numbers, is not
required. An understanding of
pyramids of numbers is not required.
c.
The biomass at each stage can be drawn to scale and shown as a pyramid of
biomass.
Students should be able to interpret pyramids of biomass and construct them from
appropriate
information.
Ecosystems - biotic & abiotic factors - interactions between organisms
- interdependency
Food chains, food webs, trophic
levels, pyramids of numbers or biomass, transfer efficiency
Adaptations, interdependence and competition
(Oxford AQA International GCSE Combined Science Double award)
a.
To survive and reproduce, organisms require a supply of materials from their
surroundings and from the
other living organisms there.
b.
Plants often compete with each other for light and space, and for water and
nutrients from the soil.
c.
Animals often compete with each other for food, mates and territory.
d.
Organisms, including microorganisms, have features (adaptations) that enable
them to survive in the
conditions in which they normally live.
e.
Some organisms live in environments that are very extreme, containing high
levels of salt, high
temperatures or high pressures. These organisms are called extremophiles.
f.
Adaptations include:
•
structural adaptations, eg the ways in which organisms are shaped, or coloured
•
behavioural adaptations, eg migration, huddling together
•
functional adaptations, related to processes
such as reproduction and metabolism.
Students given appropriate information should be able to suggest how animals and
plants are adapted to
their environment.
Adaptations, lots of examples explained including extremophiles
Decay and the carbon cycle
(Oxford AQA International GCSE Combined Science Double award)
a.
Living organisms remove materials from the environment for growth and other
processes. These materials
are returned to the environment either in waste materials or when living things
die and decay.
b.
Materials decay because they are broken down (digested) by microorganisms.
Microorganisms are more
active and digest materials faster in warm, moist, aerobic conditions.
c.
The decay process releases substances that plants need to grow.
d.
In a stable community, the processes that remove materials are balanced by
processes that return
materials. The materials are part of a constant cycle.
e.
The constant cycling of carbon is called the carbon cycle.
In the carbon cycle:
•
carbon dioxide is removed from the environment by green plants and algae during
photosynthesis
•
the carbon from the carbon dioxide is used to make carbohydrates, fats and
proteins, which make up
the body of plants and algae
•
when green plants and algae respire, some of this carbon becomes carbon dioxide
and is released into
the atmosphere
•
when green plants and algae are eaten by animals and these animals are eaten by
other animals, some
of the carbon becomes part of the fats and proteins that make up the bodies of
the consumers
•
when animals respire, some of this carbon becomes carbon dioxide and is released
into the atmosphere
•
when plants, algae and animals die, some animals and microorganisms feed on
their bodies
•
carbon is released into the atmosphere as carbon dioxide when microorganisms
respire
•
by the time the microorganisms and detritus feeders have broken down the waste
products and dead
bodies of organisms in ecosystems and cycled the materials as plant nutrients,
all the energy originally
absorbed by green plants and algae has been transferred
•
combustion of wood and fossil fuels releases carbon dioxide into the atmosphere.
Students should be able to apply the principles of the carbon cycle.
Carbon cycle,
nitrogen cycle, water cycle, decomposition - decay investigation, biogas
ORGANISMS’ INTERACTION WITH THE ENVIRONMENT
(Oxford AQA International GCSE Combined Science Double award)
Changes in environmental conditions may be biotic or abiotic and can result in
responses from an organism
which protect the organism from harm and support maintenance of the species.
Such responses may impact
on the internal stability of the organism or promote certain behaviours to
protect it.
The human nervous system
(Oxford AQA International GCSE Combined Science Double award)
a.
The nervous system enables humans to react to their surroundings and to
coordinate their behaviour.
b.
Information from receptors passes along cells (neurones) as impulses to the
central nervous system (CNS).
The CNS is the brain and spinal cord. The brain coordinates the response.
c.
Reflex actions are automatic and rapid. They often involve sensory, relay and
motor neurones.
d.
In a simple reflex action such as a pain-withdrawal reflex:
•
impulses from a receptor pass along a sensory neurone to the CNS
•
at a junction (synapse) between a sensory neurone and a relay neurone in the
CNS, a chemical is
released that causes an impulse to be sent along a relay neurone
•
a chemical is then released at the synapse between a relay neurone and motor
neurone in the CNS,
causing impulses to be sent along a motor neurone to the effector
•
the effector is either a muscle or a gland: a muscle responds by contracting and
a gland responds by
releasing (secreting) chemical substances.
e.
Effectors include muscles and glands.
Students should be able, when provided with appropriate information, to analyse
a particular given
example of behaviour in terms of:
stimulus
→
receptor
→
coordinator
→
effector
→
response
An introduction
to the nervous system including the reflex arc
Homeostasis
(Oxford AQA International GCSE Combined Science Double award)
a.
Automatic control systems in the body keep conditions inside the body relatively
constant.
b.
Control systems include:
•
cells called receptors, which detect stimuli (changes in the environment)
•
coordination centres that receive and process information from receptors
•
effectors, which bring about responses.
c.
Receptors are found in many organs, including:
•
the eyes – sensitive to light
•
the ears – sensitive to sound, and to changes in position (which enables us to
keep our balance)
•
the tongue and in the nose – sensitive to chemicals (enable us to taste and to
smell)
•
the skin – sensitive to touch, pressure, pain and to temperature changes
•
the brain – sensitive to blood temperature and the concentration of water in the
blood
•
the pancreas – sensitive to the concentration of glucose in the blood.
Knowledge and understanding of the structure and functions of sense organs such
as the eye and the ear is
not
required.
d.
Coordination centres include the brain and spinal cord and the pancreas.
e.
Internal conditions that are controlled include
•
temperature
•
the water content of the body
•
the ion content of the body
•
blood glucose levels.
Homeostasis - introduction to how it functions (negative
feedback systems explained)
Temperature control
(Oxford AQA International GCSE Combined Science Double award)
a.
Body temperature is monitored and controlled by the thermoregulatory centre in
the brain. The
thermoregulatory centre has receptors sensitive to the temperature of the blood
flowing through the brain.
The name of the centre in the brain (hypothalamus) is
not
required.
b.
Temperature receptors in the skin send impulses to the thermoregulatory centre,
giving information about
skin temperature.
c.
If the core body temperature is too high:
•
blood vessels supplying the skin capillaries dilate so that more blood flows
through the capillaries and
more energy is transferred from the skin to the environment
•
sweat glands release more sweat, which cools the body as it evaporates.
Core Tier students are
not
expected to describe details of changes in the blood vessels when the core body
temperature is too high, but should understand that the skin looks red when we
are hot due to increased
blood flow.
d.
Sweating helps to cool the body. More water is lost when it is hot, and more
fluid has to be taken through
drink or food to balance this loss.
If the core body temperature is too low:
•
blood vessels supplying the skin capillaries constrict to reduce the flow of
blood through the
capillaries
•
muscles may ‘shiver’ – their contraction needs respiration, which transfers
energy to warm the body.
Core Tier students are
not
expected to describe details of changes in the blood vessels when the core body
temperature is too low.
Homeostasis - thermoregulation, control of temperature
Control of blood glucose
(Oxford AQA International GCSE Combined Science Double award)
a.
The blood glucose concentration is monitored and controlled by the pancreas.
Much of the glucose is
stored as glycogen in the liver and muscles. When these stores are full, excess
glucose is stored as lipid.
b.
If blood glucose levels are too high, the pancreas produces the hormone insulin,
which allows the glucose
to move from the blood into the cells.
c.
When blood glucose levels fall, the pancreas produces a second hormone,
glucagon. This causes
glycogen to be converted into glucose and released into the blood.
d.
In Type 1 diabetes a person’s blood glucose level may be too high because the
pancreas does not produce
enough of the hormone insulin. Type 1 diabetes may be controlled by careful
diet, exercise, and by injecting
insulin.
e.
Type 2 diabetes develops when the body does not respond to its own insulin.
Obesity is a significant factor
in the development of Type 2 diabetes. Type 2 diabetes can be controlled by
careful diet, exercise and by
drugs that help the cells to respond to insulin
Homeostasis - control of blood sugar level
- insulin and diabetes
Behaviour
(Oxford AQA International GCSE Combined Science Double award)
a.
Sexual reproduction requires the finding and selection of a suitable mate, and
can involve courtship
behaviours that advertise an individual’s quality. Animals have different mating
strategies, including:
•
a mate for life
•
several mates over a life time
•
a mate for a breeding season
•
several mates over one breeding season.
b.
Some animals have developed special behaviours for rearing their young. Parental
care can be a successful
evolutionary strategy, including:
•
increased chance of survival of offspring
•
increased chance of parental genes being passed on by the offspring.
Students should be able to explain how, within the animal kingdom, parental care
may involve risks to the
parents
c.
The different behaviours displayed by animals include:
•
innate behaviour
•
imprinting
•
habituation
•
classic conditioning
•
operant conditioning.
d.
Humans can make use of conditioning when training captive animals for specific
purposes, including:
•
sniffer dogs
•
police horses.
e.
Methods of communication within the animal kingdom. Animals use a variety of
types of signals to
communicate.
Students should be able to describe the types of signals animals use to
communicate eg sound, chemical,
visual.
Infection and response
(Oxford AQA International GCSE Combined Science Double award)
a.
Microorganisms that cause infectious disease are called pathogens.
b.
Bacteria and viruses may reproduce rapidly inside the body. Bacteria may produce
poisons (toxins) that
make us feel ill. Viruses live and reproduce inside cells, causing damage.
Knowledge of the structure of viruses is
not
required
c.
White blood cells help to defend against pathogens by:
•
ingesting pathogens (phagocytosis)
•
producing antibodies, which destroy particular bacteria or viruses
•
producing antitoxins, which counteract the toxins released by the pathogens.
d.
The immune system of the body produces specific antibodies to kill a particular
pathogen. This leads
to immunity from that pathogen. In some cases, dead or inactivated pathogens
stimulate antibody
production. If a large proportion of the population is immune to a pathogen, the
spread of the pathogen is
very much reduced.
e.
People can be immunised against a disease by introducing small quantities of
dead or inactive forms of
the pathogen into the body (vaccination). Vaccines stimulate the white blood
cells to produce antibodies
that destroy the pathogen. This makes the person immune to future infections by
the microorganism,
because the body can respond by rapidly making the correct antibody, in the same
way as if the person
had previously had the disease. The MMR vaccine is used to protect children
against measles, mumps and
rubella.
Details of vaccination schedules and side effects associated with specific
vaccines are not required.
Students should be able to evaluate the advantages and disadvantages of being
vaccinated against a
particular disease.
f.
Antibiotics, such as penicillin, are medicines that help to cure bacterial
disease by killing infective bacteria
inside the body. It is important that specific bacteria should be treated by
specific antibiotics. The use of
antibiotics has greatly reduced deaths from infectious bacterial diseases.
g.
Antibiotics cannot kill viral pathogens.
Students should be aware that it is difficult to develop drugs that kill viruses
without also damaging the
body’s tissues.
h.
Mutations of pathogens produce new strains.
Antibiotics kill individual pathogens of the non-resistant
strain but individual resistant pathogens survive and reproduce, so the
population of the resistant
strain rises.
Antibiotics and vaccinations may no longer be effective against a new resistant
strain of the
pathogen. The new strain will then spread rapidly because people are not immune
to it and there is no
effective treatment.
Knowledge of development of resistance in bacteria is limited to the fact that
pathogens mutate,
producing resistant strains.
i.
Many strains of bacteria, including MRSA, have developed resistance to
antibiotics. Overuse and
inappropriate use of antibiotics has increased the rate of development of
antibiotic-resistant strains of
bacteria.
Antibiotics are not currently used to treat non-serious infections such as mild
throat infections,
in order to slow down the rate of development of resistant strains.
j.
The development of antibiotic-resistant strains of bacteria necessitates the
development of new
antibiotics.
Required practical:
Investigate the effect of disinfectants and antibiotics on uncontaminated
cultures of microorganisms.
Keeping healthy - communicable diseases -
pathogen infections including viruses and vaccination
Keeping healthy - non-communicable diseases
- risk factors for e.g. CVD, cancers, obesity, diabetes, body/mass/hip
indexes
Keeping healthy - defence against
pathogens, infections, treating diseases, vaccination, new drugs and testing, monoclonal antibodies,
detecting diseases and development of new drugs and medicines
INHERITANCE
(Oxford AQA International GCSE Combined Science Double award)
Genetic information in a cell is held in the chemical DNA in the form of a four
letter code. Genes determine the
development and structure of organisms. In asexual reproduction all the genes in
the offspring come from one
parent. In sexual reproduction half of the genes come from each parent.
Reproduction
(Oxford AQA International GCSE Combined Science Double award)
There are two forms of reproduction:
•
sexual reproduction – the joining (fusion) of male and female gametes. The
mixture of the genetic
information from two parents leads to variety in the offspring
•
asexual reproduction – no fusion of gametes and only one individual is needed as
the parent. There is
no mixing of genetic information and so no genetic variation in the offspring.
These genetically identical
individuals are known as clones
Cell division
(Oxford AQA International GCSE Combined Science Double award)
a.
The nucleus of a cell contains chromosomes. Chromosomes carry genes that control
the characteristics of
the body. Each chromosome carries a large number of genes.
b.
Many genes have different forms called alleles, which may produce different
characteristics.
c.
In body cells the chromosomes are normally found in pairs.
d.
Body cells divide by mitosis to produce additional cells during growth or to
produce replacement cells.
e.
When a body cell divides by mitosis:
•
copies of the genetic material are made
•
the cell then divides once to form two genetically identical body cells.
f.
Cells in reproductive organs divide to form gametes.
g.
A cell divides to form gametes by meiosis.
h.
When a cell divides to form gametes:
•
copies of the genetic information are made
•
the cell then divides twice to form four gametes, each with a single set of
chromosomes.
i.
Gametes join at fertilisation to form a single body cell with new pairs of
chromosomes. This cell repeatedly
divides by mitosis to form many cells. As an organism develops, these cells
differentiate to form different
kinds of cells.
j.
Most types of animal cell differentiate at an early stage whereas many plant
cells retain the ability to
differentiate throughout life. In mature animals, cell division is mainly
restricted to repair and replacement.
k.
Cells from human embryos and adult bone marrow, called stem cells, can be made
to differentiate into
many different types of human cell.
l.
In therapeutic cloning an embryo is produced with the same genes as the patient.
Stem cells from the
embryo will not be rejected by the patient’s body so they may be used for
medical treatment.
m.
Treatment with stem cells may be able to help conditions such as paralysis.
Knowledge and understanding of stem cell techniques is
not
required.
Students should be able, when provided with appropriate information, to make
informed judgements about
the social and ethical issues concerning the use of stem cells from adult bone
marrow and embryos in
medical research and treatments.
Cell division - cell cycle - mitosis, meiosis, sexual/asexual reproduction,
binary fission, cancer cells
Stem cells and medical uses, and
an introduction to cell
differentiation and specialisation
Genetic variation
(Oxford AQA International GCSE Combined Science Double award)
a.
Differences in the characteristics of individuals of the same kind may be due to
differences in:
•
the genes they have inherited (genetic causes)
•
the conditions in which they have developed (environmental causes)
•
a combination of genetic and environmental causes.
b.
The information that results in plants and animals having similar
characteristics to their parents is carried
by genes, which are passed on in the sex cells (gametes) from which the
offspring develop.
c.
The nucleus of a cell contains chromosomes. Chromosomes carry genes that control
the characteristics of
the body. Chromosomes are normally found in pairs.
d.
In human body cells, one of the 23 pairs of chromosomes carries the genes that
determine sex. In females
the sex chromosomes are the same (XX); in males the sex chromosomes are
different (XY).
e.
Different genes control the development of different characteristics of an
organism. Some characteristics
are controlled by a single gene. Each gene may have different forms called
alleles.
Students should understand that genes operate at a molecular level to develop
characteristics that can be
seen.
f.
If both chromosomes in a pair contain the same allele of a gene, the individual
is homozygous for that
gene. If the chromosomes in a pair contain different alleles of a gene, the
individual is heterozygous for
that gene.
g.
An allele that controls the development of a characteristic when it is present
on only one of the
chromosomes is called a dominant allele. An allele that controls the development
of a characteristic only if
the dominant allele is not present is called a recessive allele.
Students should be familiar with principles used by Mendel in investigating
monohybrid inheritance in peas.
They should understand that Mendel’s work preceded the work by other scientists
which linked Mendel’s
‘inherited factors’ with chromosomes.
Extension Tier students should be able to construct genetic diagrams of
monohybrid crosses and
to predict the outcomes of monohybrid crosses. They should be able to use the
terms homozygous,
heterozygous, phenotype and genotype.
Core Tier students should be able to interpret genetic diagrams of monohybrid
inheritance and sex
inheritance, but will
not
be expected to construct genetic diagrams or use the terms homozygous,
heterozygous, phenotype of genotype.
Students should understand that genetic diagrams are biological models which can
be used to predict the
outcomes of crosses.
Students should be able to interpret genetic diagrams, including family trees.
h.
Chromosomes are made up of large molecules of DNA. DNA contains the coded
information that
determines inherited characteristics.
i.
A gene is a small section of DNA.
Each gene codes for a particular combination of amino acids, to make a
specific protein.
j.
DNA is made of very long strands, twisted to form a double helix, which contain
four different compounds,
called bases.
Students are
not
expected to know the names of the four bases or how complementary pairs of bases
enable DNA replication to take place.
k.
A sequence of three bases is the code for a particular amino acid. The order of
bases controls the order in
which amino acids are assembled to produce a particular protein.
Cell division - cell cycle - mitosis, meiosis, sexual/asexual reproduction,
binary fission and cancer
DNA and RNA structure and Protein Synthesis and an
experiment to extract DNA
An introduction to genetic
variation and the formation and consequence of mutations
Introduction to the inheritance of characteristics,
genetic diagrams (including Punnett squares) including technical terms, Mendel's work
Genetic disorders
(Oxford AQA International GCSE Combined Science Double award)
Attention is drawn to the potential sensitivity needed in teaching about
inherited disorders.
a.
Some disorders are inherited.
Students should be able to interpret data relating to genetic disorders such as
polydactyly, cystic fibrosis
and sickle cell anaemia.
b.
Some inherited conditions are caused by inheritance of abnormal numbers of
chromosomes, eg Down’s
Syndrome is caused by the presence of an extra chromosome
Inherited genetic disorders, genetic
testing
Genetic manipulation
(Oxford AQA International GCSE Combined Science Double award)
a. Modern cloning techniques include:
• tissue culture – using small groups of cells from part of a plant
• embryo transplants – splitting cells from a developing animal embryo before
they become specialised,
then transplanting the identical embryos into host mothers
• adult cell cloning – the nucleus is removed from an unfertilised egg cell and
the nucleus from an adult
body cell, eg a skin cell, is inserted into the egg cell. An electric shock then
acts as the catalyst for
the egg cell to begin to divide to form embryo cells. These embryo cells contain
the same genetic
information as the adult skin cell. When the embryo has developed into a ball of
cells, it is inserted into
the womb of an adult female to continue its development.
b. In genetic engineering, genes from the chromosomes of humans and other
organisms can be ‘cut out’
and transferred to cells of other organisms:
• enzymes are used to isolate the required gene
• this gene is inserted into a vector, usually a bacterial plasmid or a virus
• the vector is used to insert the gene into the required cells.
c. Genes can also be transferred to the cells of animals, plants or
microorganisms at an early stage in their
development so that they develop with desired characteristics.
d. Crops that have had their genes modified in this way are called genetically
modified (GM) crops. GM crops
include ones that are resistant to insect attack or to herbicides.
e. GM crops generally show increased yields.
f.
Concerns about GM crops include the effect on populations of wild flowers and
insects, and uncertainty
about the effects of eating GM crops on human health.
Students should be able, when provided with appropriate information, to
interpret information about
cloning techniques and genetic engineering techniques and to make informed
judgements about issues
concerning cloning and genetic engineering, including GM crops.
Genetic
engineering: uses - making insulin, medical applications, GM crops & food
security
Genetic
engineering: Uses including GM crops & food
security
VARIATION AND EVOLUTION
(Oxford AQA International GCSE Combined Science Double award)
All life today is directly descended from a universal common ancestor that was a
simple one-celled organism.
Over countless generations changes resulted from natural diversity within a
species which makes possible the
selection of those individuals best suited to survive under certain conditions.
Organisms not able to respond
sufficiently to changes in their environment are at risk of becoming extinct.
Continuous and
Discontinuous Variation
(Oxford AQA International GCSE Combined Science Double award)
The causes of variation include:
•
genetic variation – different characteristics as a result of mutation or
reproduction
•
environmental variation – different characteristics caused by an organism’s
environmental (acquired
characteristics).
Natural selection
(Oxford AQA International GCSE Combined Science Double award)
a.
Theories of how organisms have evolved include:
•
the theory of evolution by natural selection
•
other theories, including that of Lamarck, are based mainly on the idea that
changes that occur in an
organism during its lifetime can be inherited. We now know that in the vast
majority of cases this type
of inheritance cannot occur.
b.
Evolution occurs via natural selection.
•
Individual organisms within a particular species may show a wide range of
variation because of
differences in their genes.
•
Individuals with characteristics most suited to the environment are more likely
to survive to breed
successfully.
•
The genes that have enabled these individuals to survive are then passed on to
the next generation.
Students should develop an understanding of the time scales involved in
evolution.
c.
New species arise as a result of:
•
isolation: two populations of a species become separated, eg geographically
•
genetic variation: each population has a wide range of alleles that control
their characteristics
•
natural selection: in each population, the alleles that control the
characteristics which help the organism
to survive are selected
•
speciation: the populations become so different that successful interbreeding
leading to fertile
offspring, is no longer possible.
Evolution - theories and evidence, variation, speciation -
new/old species & extinctions, selective breeding
An introduction to genetic
variation and the formation and consequence of mutations
CHEMISTRY
(Oxford AQA International GCSE Combined Science Double award)
ATOMIC STRUCTURE AND THE PERIODIC TABLE
Atoms are the building blocks of all materials and knowledge of atomic structure
and the periodic table are
fundamental to the learning associated with all the following sections.
Solids liquids and gases
(Oxford AQA International GCSE Combined Science Double award)
a.
Matter can be classified in terms of the three states of matter.
Students should be familiar with states of matter and be able to name each
inter-conversion process. They
should be able to describe and explain their inter-conversion in terms of how
the particles are arranged and
their movement. They should understand the energy changes that accompany changes
of state.
b.
Evidence for the existence of particles can be obtained from simple experiments.
Students should be familiar with simple diffusion experiments such as Br2/air,
NH3/HCl,
KMnO4/water.
States of Matter: particle theory - gas, liquid & solid GCSE study revision notes
Quizzes-Worksheets section 16.
(opens in new window for convenience)
A simple model of the atom
(Oxford AQA International GCSE Combined Science Double award)
a.
All substances are made of atoms. A substance that is made of only one sort of
atom is called an element.
There are about 100 different elements. Elements are shown in the periodic
table.
b.
Atoms of each element are represented by a chemical symbol, eg O represents an
atom of oxygen.
Knowledge of the chemical symbols for elements other than those named in the
specification is
not
required.
c.
Atoms have a small central nucleus, made up of protons and neutrons, and around
which there are
electrons.
Students should be aware that the atomic model has changed over time.
d.
The relative electrical charges
and name of particle:
Proton
+1.
Neutron
0,
Electron
–1
e.
In an atom, the number of electrons is equal to the number of protons in the
nucleus. Atoms have no
overall electrical charge.
f.
The number of protons in an atom of an element is its atomic number. The sum of
the protons and
neutrons in an atom is its mass number.
Students will be expected to calculate the numbers of each sub-atomic particle
in an atom from its atomic
number and mass number.
g.
Atoms of the same element can have different numbers of neutrons; these atoms
are called isotopes of
that element.
h.
Atoms can be represented as shown in this example:
mass number
of
23,
atomic number
11
for sodium
i.
Electrons occupy particular energy levels. Each electron in an atom is at a
particular energy level (in a
particular shell). The electrons in an atom occupy the lowest available energy
levels (innermost available
shells).
Students may answer questions in terms of either energy levels or shells e.g.
diagram on the right.
Students should be able to represent the electronic structure of the first
twenty elements of the periodic
table in the following forms
j. The relative masses of protons, neutrons and electrons are:
Sub–atomic particle |
Relative mass |
Electric charge |
Comments |
Proton |
1 |
+1
(+ positive) |
In
the nucleus, a nucleon |
Neutron |
1 |
0
(zero) |
In the nucleus, a nucleon |
Electron |
1/1850 or 0.00055 very small |
–1
(– negative) |
NOT a nucleon. Electrons are arranged in energy levels or shells
in orbit around the nucleus |
k.
The relative atomic mass of an element (Ar) compares the mass of atoms of the element with the
12C
isotope (carbon-12). It is an average value for the isotopes of the element.
Students will not be expected to calculate relative atomic masses from isotopic
abundances.
Atomic Structure
including isotopes
and
Quizzes-Worksheets
THE PERIODIC
TABLE
(Oxford AQA International GCSE Combined Science Double award)
a.
The periodic table is arranged in order of atomic (proton) number. Elements with
similar properties are in
columns, known as groups. The table is called a periodic table because similar
properties occur at regular
intervals.
Students should know that the current periodic table is based on the work of
Mendeleev.
b.
Elements in the same group in the periodic table have the same number of
electrons in their highest energy
level (outer electrons) and this gives them similar chemical properties.
Students should know that basing the periodic table on groups of elements with
similar properties has
allowed for the prediction of elements which were still to be discovered.
c.
The elements in Group 0 of the periodic table are called the noble gases. They
are unreactive because their
atoms have stable arrangements of electrons.
Students should know that the noble gases have eight electrons in their outer
energy level, except for
helium, which has only two electrons.
The Periodic Table - overview and summary
and
Quizzes-Worksheets section
(opens in new window for convenience)
Group 1
The Alkali Metals,
physical & chemical properties, uses
and
Quizzes-Worksheets section
(opens in new window for convenience)
Group 7
The Halogens,
physical & chemical properties
and
Quizzes-Worksheets section
(opens in new window for convenience)
Group 0/8
Noble Gases
and
Quizzes-Worksheets section
STRUCTURE, BONDING AND THE PROPERTIES OF MATTER
This section examines how atoms interact to form chemical bonds and how these
bonds determine the
properties and uses of materials.
Chemical bonds: ionic, covalent and metallic
(Oxford AQA International GCSE Combined Science Double award)
a.
Compounds are substances in which atoms of two or more elements are chemically
combined.
b.
Chemical bonding involves either transferring or sharing electrons in the
highest occupied energy levels
(outer shells) of atoms in order to achieve the electron arrangement of a noble
gas.
c.
When atoms form chemical bonds by transferring electrons, they form ions. Atoms
that lose electrons
become positively charged ions. Atoms that gain electrons become negatively
charged ions. Ions have the
electron arrangement of a noble gas (Group 0). Compounds formed from metals and
non-metals consist of
ions.
Students should know that metals form positive ions, whereas non-metals form
negative ions.
Students should be able to represent the electron arrangement of ions in the
following form:
e.g. for the ionic compound sodium chloride, made up of the sodium ion (Na+)
and chloride ion (Cl-)
combination.

Students should be able to relate the charge on simple ions to the group number
of the element in the
periodic table
d.
The elements in Group 1 of the periodic table, the alkali metals, all react with
non-metal elements to form
ionic compounds in which the metal ion has a single positive charge.
Knowledge of the chemical properties of alkali metals is limited to their
reactions with non-metal elements
and water.
e.
The elements in Group 7 of the periodic table, the halogens, all react with
metals to form ionic compounds
in which the halide ions have a single negative charge.
Knowledge of the chemical properties of the halogens is limited to reactions
with metals and displacement
of less reactive halogens.
f.
An ionic compound is a giant structure of ions. Ionic compounds are held
together by strong electrostatic
forces of attraction between oppositely charged ions. These forces act in all
directions in the lattice and
this is called ionic bonding.
Students should be familiar with the structure of sodium chloride but do
not
need to know the structures of
other ionic compounds.
Students given appropriate information, should be able to draw or complete
diagrams to show how
elements form ions and ionic compounds.
g.
When atoms share pairs of electrons, they form covalent bonds. These bonds
between atoms are strong.
Some covalently bonded substances, such as H2,
Cl2
, O2, N2, HCl, H2O, NH3
and CH4, consist of simple
molecules. Others, such as diamond and silicon dioxide, have giant covalent
structures (macromolecules).
Students should be able to represent the covalent bonds in molecules such as
water, ammonia, hydrogen,
hydrogen chloride, methane and oxygen in the following forms:
e.g. for ammonia (NH3)
be familiar with these different styles
Students, given appropriate information, should be able to draw or complete
diagrams to show how
elements form covalent compounds by sharing electrons.
Students should be able to recognise other simple molecules and giant structures
from diagrams that
show their bonding
h.
Compounds formed from non-metals consist of molecules. In molecules, the atoms
are held together by
covalent bonds.
i.
Metals consist of giant structures of atoms arranged in a regular pattern.
j.
The electrons in the highest occupied energy levels (outer shell) of metal atoms
are delocalised and so
free to move through the whole structure. This corresponds to a structure of
positive ions with electrons
between the ions holding them together by strong electrostatic attractions. The
bonding in metals is
represented in the following form:
Showing the original neutral atoms and the actual ions and delocalised electrons
in the real metallic lattice of a metal crystal.
How bonding and structure are related to the properties of substances
a.
Ionic compounds have regular structures (giant ionic lattices) in which there
are strong electrostatic forces
of attraction in all directions between oppositely charged ions.
These compounds have high melting points and high boiling points because of the
large amounts of
energy needed to break the many strong bonds.
b.
When melted or dissolved in water, ionic compounds conduct electricity because
the ions are free to move
and carry the current.
Knowledge of the structures of specific ionic compounds other than sodium
chloride is
not
required.
c.
Substances that consist of simple molecules are gases, liquids or solids that
have relatively low melting
points and boiling points.
d.
Substances that consist of simple molecules have only weak forces between the
molecules
(intermolecular forces). It is these intermolecular forces that are overcome,
not the covalent bonds,
when the substance melts or boils.
Students need to understand that intermolecular forces are weak compared with
covalent bonds.
e.
Substances that consist of simple molecules do not conduct electricity because
the molecules do not have
an overall electric charge.
f.
Atoms that share electrons can also form giant structures or macromolecules.
Diamond and graphite
(forms of carbon) and silicon dioxide (silica) are examples of giant covalent
structures (lattices) of atoms.
All the atoms in these structures are linked to other atoms by strong covalent
bonds and so they have very
high melting points.
Students should be able to recognise other giant structures or macromolecules
from diagrams showing
their bonding.
g.
Metals conduct heat and electricity because of the delocalised electrons in
their structures.
Students should know that conduction depends on the ability of electrons to move
through the metal.
Structure and bonding in carbon
(Oxford AQA International GCSE Combined Science Double award)
a.
The element carbon can form four covalent bonds.
b.
In diamond, each carbon atom forms four covalent bonds with other carbon atoms
in a giant covalent
structure, so diamond is very hard.
c.
In graphite, each carbon atom bonds to three others, forming layers. The layers
are free to slide over each
other because there are no covalent bonds between the layers and so graphite is
soft and slippery.
Extension Tier students should be able to explain the properties of graphite in
terms of weak forces
between the layers.
d.
In graphite, one electron from each carbon atom is delocalised. These
delocalised electrons allow
graphite to conduct heat and electricity.
Students should realise that graphite is similar to metals in that it has
delocalised electrons.
e.
Carbon can also form fullerenes with different numbers of carbon atoms.
Fullerenes can be used for drug
delivery into the body, in lubricants, as catalysts, and in nanotubes for
reinforcing materials, eg in tennis
racquets.
Students are only required to know that the structure of fullerenes is based on
hexagonal rings of carbon
atoms
INDEX of all
Types of Chemical Bonding and Materials Science Notes
Introduction to
Chemical Bonding
Ionic Bonding - compounds and properties
Covalent Bonding -small simple molecules and properties
Covalent Bonding - macromolecules and giant covalent structures
Metallic Bonding - structure and properties of metals
Quizzes-Worksheets section
(opens in new window for convenience)
CHEMICAL CHANGES
(Oxford AQA International GCSE Combined Science Double award)
The group of materials known as metals are explored in more detail including how
atoms are rearranged to
form new substances in chemical reactions.
Metals
(Oxford AQA International GCSE Combined Science Double award)
a.
Metals are useful materials because they are good conductors of heat and
electricity. They can be bent or
hammered into shape because the layers of atoms in metals are able to slide over
each other.
b.
An alloy is a mixture of at least two elements, at least one of which is a
metal. Alloys often have properties
that are different to the metals they contain. This makes them more useful than
the pure metals alone.
Steels are a mixture of iron with carbon and sometimes other metals.
Students may be given information on the composition of specific alloys so that
they can evaluate their
uses.
c.
Copper is useful for electrical wiring and plumbing because it has the following
properties:
•
it is a good conductor of heat and electricity
•
it can be bent but is hard enough to be used to make pipes or tanks
•
it does not react with water.
Metallic Bonding - structure and properties of metals
The reactivity series of metals
(Oxford AQA International GCSE Combined Science Double award)
a.
Metals can be arranged in an order of their reactivity from their reactions with
water and dilute acids.
Students should be able to recall and describe the reactions, if any, of
potassium, sodium, lithium, calcium,
magnesium, zinc, iron and copper with water or dilute acids. Students should be
able, where appropriate,
to place them in order of reactivity.
b.
Displacement reactions involving metals and their compounds in aqueous solution
establish positions
within the reactivity series.
Students should be able to describe displacement reactions in terms of oxidation
and reduction, and to
write the ionic equations.
c.
Unreactive metals such as gold are found in the Earth as the metal itself but
most metals are found as
compounds that require chemical reactions to extract the metal.
d.
Metals that are less reactive than carbon can be extracted from their oxides by
reduction with carbon: for
example, iron oxide is reduced in the blast furnace to make iron.
Knowledge and understanding are limited to the reduction of oxides using carbon.
Knowledge of reduction is limited to the removal of oxygen.
Students should understand that oxidation can be described as the gain of oxygen
by a substance.
Details of the blast furnace are
not
required, but students should know the raw materials used and explain
the simple chemistry involved, including the use of equations.
Knowledge of the details of the extraction of other metals is
not
required. Examination questions may
provide further information about specific processes for students to interpret
or evaluate.
e.
Metals that are more reactive than carbon, such as aluminium, are extracted by
electrolysis of molten
compounds. The use of large amounts of energy in the extraction of these metals
makes them expensive.
Knowledge of the details of industrial methods of electrolysis is
not
required, other than the detail required
for aluminium.
f.
New ways of extracting copper from low-grade ores are being researched to limit
the environmental impact
of traditional mining.
Copper can be extracted by phytomining, or by bioleaching.
Students should know and understand that:
•
phytomining uses plants to absorb metal compounds and that the plants are burned
to produce ash that
contains the metal compounds
•
bioleaching uses bacteria to produce leachate solutions that contain metal
compounds.
Further specific details of these processes are
not
required.
g.
Copper can be obtained from solutions of copper salts by electrolysis.
Students should know the electrode material and be able to write the ionic half
equations for the reactions
occurring at both electrodes.
h.
Copper can be obtained from solutions of copper salts by displacement using
scrap iron.
Students should be able to describe this in terms of oxidation and reduction,
and to write the ionic equation.
i.
We should recycle metals because extracting them uses limited resources, and is
expensive in terms of
energy and in terms of effects on the environment.
Students are
not
required to know details of specific examples of recycling, but should
understand the
benefits of recycling in the general terms specified here
The Reactivity Series of Metals
Metal Reactivity Series
Experiments-Observations and explanations
INDEX
and introduction to the extraction of metals
Extraction and Purification of Copper
Economic & environmental Issues -
emphasis on metal extraction and recycling
Metal carbonates
(Oxford AQA International GCSE Combined Science Double award)
a.
The carbonates of magnesium, copper, zinc, calcium and lithium decompose on
heating (thermal
decomposition) in a similar way.
Students should be aware that not all carbonates of metals in Group 1 of the
periodic table decompose at
the temperatures reached by a Bunsen burner.
b.
Metal carbonates react with acids to produce carbon dioxide, a salt and water.
Limestone, lime
- uses, includes thermal decomposition of carbonates
Acid reactions with
metals, oxides, hydroxides, carbonates and neutralisation reactions
Electrolysis
(Oxford AQA International GCSE Combined Science Double award)
a.
When an ionic substance is melted or dissolved in water, the ions are free to
move about within the liquid
or solution.
b.
Passing an electric current through ionic substances that are molten, eg lead
bromide, or in solution breaks
them down into elements. This process is called electrolysis and the substance
broken down is called the
electrolyte.
c.
During electrolysis, positively charged ions move to the negative electrode (the
cathode), and negatively
charged ions move to the positive electrode (the anode).
d.
Oxidation and reduction can be defined as the loss and gain of electrons
respectively.
e.
At the cathode, positively charged ions gain electrons; at the anode, negatively
charged ions lose
electrons.
f.
Reactions at electrodes can be represented by half equations, for example:
2Cl
–
→
Cl2
+ 2e–
or
2Cl–
– 2e–
→
Cl2
Students should be able to write half equations for the reactions occurring at
the electrodes during
electrolysis, and may be required to complete and balance supplied half
equations.
g.
If there is a mixture of ions:
•
at the cathode, the products formed depend on the reactivity of the elements
involved
•
at the anode, the products formed also depend on the relative concentrations of
the ions present.
h.
Electrolysis is used to electroplate objects. This may be for reasons such as
appearance, durability and
prevention of corrosion. It includes copper plating and silver plating.
i.
Aluminium is manufactured by the electrolysis of a molten mixture of aluminium
oxide and cryolite.
Aluminium forms at the negative electrode and oxygen at the positive electrode.
The positive electrode is
made of carbon, which reacts with the oxygen to produce carbon dioxide.
Students should understand why cryolite is used in this process.
Students should be aware that large amounts of energy are needed in the
extraction process.
j.
The electrolysis of sodium chloride solution produces hydrogen and chlorine.
Sodium hydroxide solution
is also produced. These are important reagents for the chemical industry, eg
sodium hydroxide for the
production of soap and chlorine for the production of bleach and plastics.
Students should be able to explain, using ideas related to reactivity, why each
of these products is
produced
INDEX
Electrochemistry, electrolysis
and applications
Introduction to electrolysis – electrolytes,
non–electrolytes, electrode equations
Electrolysis of copper(II) sulfate solution
Electrolysis of sodium chloride solution (brine)
Extraction of Aluminium
CHEMICAL ANALYSIS
(Oxford AQA International GCSE Combined Science Double award)
This section focuses on developing practical skills in chemistry which identify
substances and reinforces the
idea of a pure substance as consisting of one substance only.
Purity and chromatography
(Oxford AQA International GCSE Combined Science Double award)
a.
A pure element or compound contains only one substance, with no other substances
mixed in.
Students should be able to identify substances and assess their purity from
melting point and boiling point
information.
b.
Measures of purity are important in everyday substances such as foodstuffs and
drugs.
c.
A mixture consists of two or more elements or compounds not chemically combined
together. The
chemical properties of each substance in the mixture are unchanged. It is
possible to separate the
substances in a mixture by physical methods, including distillation, filtration
and crystallisation.
d.
Paper chromatography can be used to analyse substances present in a solution, eg
food colourings and
inks/dyes.
Students should be able to describe how to carry out paper chromatography
separations and
Extension
Tier students should be able to describe how the components of a mixture can be
identified using Rf
values.
They have to be aware that solvents other than water can be used.
e.
Chromatography involves a stationary and a mobile phase and separation depends
on the relative
solubilities of the components.
Students should be able to suggest chromatographic methods for distinguishing
pure from impure
substances.
Paper
& thin layer chromatography (tlc) and gas chromatography (gc, glc)
Some important
ideas and definitions in Chemistry
Identification of ions
(Oxford AQA International GCSE Combined Science Double award)
a.
Flame tests can be used to identify metal ions. Lithium, sodium, potassium,
calcium and barium
compounds produce distinctive colours in flame tests:
•
lithium compounds result in a crimson flame
•
sodium compounds result in a yellow flame
•
potassium compounds result in a lilac flame
•
calcium compounds result in a red flame
•
barium compounds result in a green flame.
Required practical:
Identify the metal ion in an unknown compound using flame testing techniques.
b.
Aluminium, calcium and magnesium ions form white precipitates with sodium
hydroxide solution but only
the aluminium hydroxide precipitate dissolves in excess sodium hydroxide
solution.
c.
Copper(II), iron(II) and iron(III) ions form coloured precipitates with sodium
hydroxide solution. Copper(II)
forms a blue precipitate, iron(II) a green precipitate and iron(III) a brown
precipitate.
d.
Carbonates react with dilute acids to form carbon dioxide. Carbon dioxide
produces a white precipitate
with limewater, which turns limewater cloudy white.
e.
Halide ions in solution produce precipitates with silver nitrate solution in the
presence of dilute nitric acid.
Silver chloride is white, silver bromide is cream and silver iodide is yellow.
f.
Sulfate ions in solution produce a white precipitate with barium chloride
solution in the presence of dilute
hydrochloric acid.
Summary of tests for common ions
ACIDS, BASES AND SALTS
(Oxford AQA International GCSE Combined Science Double award)
This section looks in greater detail at the properties and applications of acids
and bases.
INDEX of pH scale, acids,
alkalis, salts
The properties of acids and bases
(Oxford AQA International GCSE Combined Science Double award)
a.
Metal oxides and hydroxides are bases. Soluble hydroxides are called alkalis.
b.
Acids react with bases to form salts. These reactions are called neutralisation
reactions.
c.
The particular salt produced in any reaction between an acid and a base or
alkali depends on:
•
the acid used (hydrochloric acid produces chlorides, nitric acid produces
nitrates, sulfuric acid
produces sulfates)
•
the metal in the base or alkali.
d.
Ammonia dissolves in water to produce an alkaline solution. It is used to
produce ammonium salts.
e.
A solution of calcium hydroxide in water (limewater) reacts with carbon dioxide
to produce calcium
carbonate.
f.
Hydrogen ions, H
+
(aq), make solutions acidic and hydroxide ions, OH–
(aq), make solutions alkaline. The pH
scale is a measure of the acidity or alkalinity of a solution.
Students should be familiar with the pH scale from 0 to 14, and know that pH 7
is a neutral solution.
Students should be able to describe the use of universal indicator to measure
the approximate pH of a
solution.
g.
In neutralisation reactions, hydrogen ions react with hydroxide ions to produce
water. This reaction can be
represented by the equation:
H+(aq) + OH–(aq)
→
H2O(l)
Acid reactions with
metals, oxides, hydroxides, carbonates and neutralisation reactions
Reactions of bases-alkalis
like ammonia and sodium hydroxide
Preparation of salts
(Oxford AQA International GCSE Combined Science Double award)
a.
Soluble salts can be made from acids by reacting them with:
•
metals – not all metals are suitable; some are too reactive and others are not
reactive enough
•
insoluble bases – the base is added to the acid until no more will react and the
excess solid is filtered off
•
alkalis – an indicator can be used to show when the acid and alkali have
completely reacted to produce a
salt solution.
Students should be able to suggest methods to make a named soluble salt.
b.
Salt solutions can be crystallised to produce solid salts.
c.
Insoluble salts can be made by mixing appropriate solutions of ions so that a
precipitate is formed.
Precipitation can be used to remove unwanted ions from solutions: for example,
in treating water for
drinking or in treating effluent.
Students should be able to name the substances needed to make a named insoluble
salt.
Methods
of making salts and a summary of tests for common ions
Making a salt by neutralising a soluble acid with a soluble base (alkali) -
neutralisation reaction
Preparing a salt by reacting an acid with a metal or with an
insoluble base - oxide, hydroxide or carbonate
Preparing an
insoluble salt by mixing solutions of two soluble compounds
QUANTITATIVE CHEMISTRY
(Oxford AQA International GCSE Combined Science Double award)
Conservation of mass is a key concept in chemistry and this is developed during
this section. This is then
used to develop a quantitative approach to chemical reactions, leading to many
opportunities to develop
experimental skills through practical work and mathematical skills
INDEX
of Chemical Calculations for GCSE
Conservation of mass including the quantitative interpretation of chemical
equations
a.
Chemical reactions can be represented by word equations or by symbol equations.
Students should be able to write word and balanced symbol equations for
reactions in the specification.
b.
Information about the states of reactants and products can be included in
chemical equations.
Students should be able to use the state symbols (g), (l), (s) and (aq) in
equations where appropriate.
c.
No atoms are lost or made during a chemical reaction so the mass of the products
equals the mass of the
reactants.
d.
The masses of reactants and products can be calculated from balanced symbol
equations.
Students should be able to calculate the mass of a reactant or product from
information about the masses
of the other reactants and products in the reaction and the balanced symbol
equation.
e.
Even though no atoms are gained or lost in a chemical reaction, it is not always
possible to obtain the
calculated amount of a product because:
•
the reaction may not go to completion because it is reversible
•
some of the product may be lost when it is separated from the reaction mixture
•
some of the reactants may react in ways different from the expected reaction.
Explaining and calculating % reaction yield,
reasons why never 100%
Calculating relative formula/molecular mass (Mr) of a compound or element molecule
Law of Conservation of Mass and simple reacting mass calculations
Use of amount of substance in relation to masses of pure substances
a.
The relative formula mass (Mr) of a compound is the sum of the relative atomic masses of the atoms in the
numbers shown in the formula.
Students are expected to use relative atomic masses in the calculations
specified in the subject content.
Students should be able to calculate the relative formula mass (Mr)
of a compound from its formula.
b.
The percentage by mass of an element in a compound can be calculated from the
relative atomic mass of
the element in the formula and the relative formula mass of the compound.
c.
The empirical formula of a compound can be calculated from the masses or
percentages of the elements in
a compound.
Students should be able to calculate empirical formulae and molecular formulae.
Calculating relative formula/molecular mass (Mr) of a compound or element molecule
Composition by percentage (%) mass of elements
in a compound
Empirical formula and formula mass of a compound from reacting masses
(easy start, not using moles)
The mole concept
(Oxford AQA International GCSE Combined Science Double award)
a.
The relative formula mass of a substance, in grams, is known as one mole of that
substance.
Students should be able to use the relative formula mass of a substance to
calculate the number of moles
in a given mass of that substance and vice versa.
b.
One mole contains 6.02 × 1023
atoms or molecules. This number is known as Avogadro’s constant.
Introducing moles: The connection between moles, mass and formula mass - the basis of reacting mole ratio calculations
(relating reacting masses and formula
mass).
Using molar concentrations of solutions
(Oxford AQA International GCSE Combined Science Double award)
a.
The concentration of a solution is related to the mass of the solute (in terms
of number of moles) and the
volume of the solution. The concentration of a solution is calculated as
follows:
Concentration (mol/dm3) = number of moles/volume of solution (in dm3).
b.
The volumes of acid and alkali solutions that react with each other can be
measured by titration using a
suitable indicator.
Students should be able to carry out titrations using strong acids and strong
alkalis only (sulfuric,
hydrochloric and nitric acids only).
Required practical:
Establish the concentration of an unknown strong acid through titration with a
strong base.
c.
If the concentration of one of the reactants is known, the results of a
titration can be used to find the
concentration of the other reactant.
Students should know how to carry out a titration and be able to calculate the
chemical quantities in
titrations involving concentrations in mol/dm3
and in g/dm3
Molarity, volumes and solution
concentrations (and diagrams of apparatus)
Volumetric titration analysis calculations, acid-alkali titrations
(methods and diagrams of apparatus).
TRENDS WITHIN THE PERIODIC TABLE
(Oxford AQA International GCSE Combined Science Double award)
This section looks to both describe and explain trends within the periodic table
along with more detailed
knowledge and understanding of identified groups.
Group properties
(Oxford AQA International GCSE Combined Science Double award)
a.
The elements in Group 1 of the periodic table (known as the alkali metals):
•
are metals with low density (the first three elements in the group are less
dense than water)
•
react with non-metals to form ionic compounds in which the metal ion carries a
charge of +1. The
compounds are white solids that dissolve in water to form colourless solutions
•
react with water, releasing hydrogen
•
form hydroxides that dissolve in water to give alkaline solutions.
b.
In Group 1, the further down the group an element is, the more reactive the
element.
c.
The elements in Group 7 of the periodic table (known as the halogens) react with
metals to form ionic
compounds in which the halide ion carries a charge of –1.
d.
In Group 7, the further down the group an element is:
•
the less reactive the element
•
the higher its melting point and boiling point.
e.
A more reactive halogen can displace a less reactive halogen from an aqueous
solution of its salt.
f.
The trends in reactivity within groups in the periodic table can be explained
because the higher the energy
level of the outer electrons:
•
the more easily electrons are lost
•
the less easily electrons are gained.
Students should be able to explain the relative reactivities of the elements in
Group 1 and 7
Group 1
The Alkali Metals,
physical & chemical properties, uses
and
Quizzes-Worksheets section
(opens in new window for convenience)
Group 7
The Halogens,
physical & chemical properties
and
Quizzes-Worksheets section
(opens in new window for convenience)
THE RATE OF CHEMICAL CHANGE
(Oxford AQA International GCSE Combined Science Double award)
Rate of reaction
(Oxford AQA International GCSE Combined Science Double award)
a.
The rate of a chemical reaction can be found by measuring the amount of a
reactant used or the amount of
product formed over time:
Rate of reaction =
amount of reactant used /
time
Rate of reaction =
amount of product formed /
time
Students need to be able to interpret graphs showing the amount of product
formed (or reactant used up)
with time, in terms of the rate of the reaction.
Knowledge of specific reactions other than those in the subject content is
not
required, but students will
be expected to have studied examples of chemical reactions and processes in
developing their skills during
their study of this section.
b.
Chemical reactions can occur only when reacting particles collide with each
other and with sufficient
energy. The minimum amount of energy that particles must have to react is called
the activation energy.
c.
Increasing the temperature increases the speed of the reacting particles so that
they collide more
frequently and more energetically. This increases the rate of reaction.
d.
Increasing the pressure of reacting gases increases the frequency of collisions
and so increases the rate of
reaction.
e.
Increasing the concentration of reactants in solutions increases the frequency
of collisions and so increases
the rate of reaction.
f.
Increasing the surface area of solid reactants increases the frequency of
collisions and so increases the rate
of reaction.
Required practical:
Investigate factors affecting the rate of a reaction.
g.
Catalysts change the rate of chemical reactions but are not used up during the
reaction. Different reactions
need different catalysts.
Knowledge of named catalysts other than those specified in the subject content
is
not
required, but
students should be aware of some examples of chemical reactions and processes
that use catalysts.
h.
Catalysts are important in increasing the rates of chemical reactions used in
industrial processes to reduce
costs.
What do we mean by
the rate/speed of reaction? Examples, How do we measure rate? Experimental methods
Collision theory of
chemical reactions and activation energy
Effect of
changing concentration on rate
Effect of
changing pressure on rate
Effect of
changing particle size/surface area & stirring of a solid reactant on
rate
Effect of
changing temperature on rate
Effect of
using a catalyst on rate
Quizzes-Worksheets section
(opens in new window for convenience)
ENERGY CHANGES
(Oxford AQA International GCSE Combined Science Double award)
This section highlights that chemical reactions involve changes which require
energy to make them happen.
This is a fundamental concept which links to key ideas in biology and physics.
The section also involves
developing mathematical skills and also application of knowledge
Sub-index of energy changes-transfers
in chemical reactions notes
Exothermic and endothermic reactions
(Oxford AQA International GCSE Combined Science Double award)
a.
When chemical reactions occur, energy is transferred to or from the
surroundings.
Knowledge of delta H (ΔH) conventions and enthalpy changes, including the use of
positive values for
endothermic reactions and negative values for exothermic reactions, is required.
b.
An exothermic reaction is one that transfers energy to the surroundings.
Examples of exothermic reactions
include combustion, many oxidation reactions and neutralisation.
Students should be able to give examples of exothermic reactions including
combustion, oxidation and
neutralisation. Everyday uses of exothermic reactions include self-heating cans
(eg for coffee) and hand
warmers.
c.
An endothermic reaction is one that takes in energy from the surroundings.
Endothermic reactions include
thermal decompositions. Some sports injury packs are based upon endothermic
reactions.
d.
In some chemical reactions, the products of the reaction can react to produce
the original reactants. Such
reactions are called reversible reactions and are represented as follows:
If
A + B
==>
C + D is exothermic, then C + D ==> A + B is endothermic
For example:
blue
hydrated
copper
sulfate
== heat ==> white anhydrous copper sulfate + water (endothermic)
white
anhydrous
copper
sulfate
+ water ==> blue hydrated copper sulfate (exothermic, mixture heats up)
Heat changes in chemical/physical
changes - exothermic and endothermic
Reversible reactions and energy changes
e.
The amount of energy produced by a chemical reaction in solution can be
calculated from the measured
temperature change of the solution when the reagents are mixed in an insulated
container. This method
can be used for reactions of solids with water or for neutralisation reactions.
Calculating and explaining energy change
(Oxford AQA International GCSE Combined Science Double award)
a.
Simple energy level diagrams can be used to show the relative energies of
reactants and products, the
activation energy and the overall energy change of a reaction.
Students will be expected to understand simple energy level diagrams showing the
relative energies of
reactants and products, the activation energy and the overall energy change,
with a curved arrow to show
the energy as the reaction proceeds.
Students should be able to relate these to exothermic and endothermic reactions.
b.
During a chemical reaction:
•
energy must be supplied to break bonds
•
energy is released when bonds are formed.
Students should be able to calculate the energy transferred in reactions and
interpret simple energy level
diagrams in terms of bond breaking and bond formation (including the idea of
activation energy and the
effect on this of catalysts).
c.
In an exothermic reaction, the energy released from forming new bonds is greater
than the energy needed
to break existing bonds.
Students should be able to calculate the energy transferred in reactions using
bond dissociation energies
supplied.
d.
In an endothermic reaction, the energy needed to break existing bonds is greater
than the energy released
from forming new bonds.
e.
Catalysts provide a different pathway for a chemical reaction that has a lower
activation energy.
Students should be able to represent the effect of a catalyst on an energy level
diagram
Calorimeter methods of determining energy changes
and calculations from calorimeter results
ORGANIC CHEMISTRY
(Oxford AQA International GCSE Combined Science Double award)
Carbon compounds as
fuels
(Oxford AQA International GCSE Combined Science Double award)
Crude oil
(Oxford AQA International GCSE Combined Science Double award)
a.
Crude oil is a mixture of a very large number of compounds.
b.
Most of the compounds in crude oil are hydrocarbons, which are molecules made up
of hydrogen and
carbon atoms only.
c.
The many hydrocarbons in crude oil may be separated into fractions, each of
which contains molecules
with a similar number of carbon atoms, by evaporating the oil and allowing it to
condense at a number of
different temperatures. This process is called fractional distillation.
Students should know and understand the main processes in continuous fractional
distillation in a
fractionating column.
Knowledge of the names of specific fractions or fuels is
not
required
Fractional distillation of crude oil & uses of fractions,
What makes a good fuel?
Hydrocarbons
(Oxford AQA International GCSE Combined Science Double award)
a.
Most of the hydrocarbons in crude oil are saturated hydrocarbons called alkanes.
The general formula for
the homologous series of alkanes is CnH2n+2
Students should know that in saturated hydrocarbons all the carbon–carbon bonds
are single covalent
bonds.
b.
Alkane molecules can be represented in the following forms:
C2H6
or

Students should know that in displayed structures
represents a covalent bond.
Students should be able to recognise alkanes from their formulae in any of the
forms, but do not need to
know the names of specific alkanes other than methane, ethane and propane.
c.
Some properties of hydrocarbons depend on the size of their molecules. These
properties influence how
hydrocarbons are used as fuels.
Knowledge and understanding of trends in properties of hydrocarbons is limited
to:
•
boiling points,
viscosity and
flammability.
d.
Most fuels, including coal, contain carbon and/or hydrogen and may also contain
some sulfur. The gases
released into the atmosphere when a fuel burns may include carbon dioxide, water
(vapour), carbon
monoxide, sulfur dioxide and oxides of nitrogen. Solid particles (particulates)
may also be released. Solid
particles may contain soot (carbon) and unburnt fuels.
Sulfur dioxide and oxides of nitrogen cause acid rain, an increase in carbon
dioxide may result in climate
change, and solid particles cause global dimming
Students should be able to relate products of combustion to the elements present
in compounds in the fuel
and to the extent of combustion (whether complete or incomplete).
No details of how the oxides of nitrogen are formed are required, other than the
fact that they are formed
at high temperatures.
e.
The combustion of hydrocarbon fuels releases energy. During combustion, the
carbon and hydrogen in the
fuels are oxidised.
f.
Biofuels, including biodiesel and ethanol, are produced from plant material, and
are possible alternatives to
hydrocarbon fuels.
Students should know and understand the benefits and disadvantages of biofuels
in terms of:
•
use of renewable resources
•
their impacts on land use
•
their carbon footprint.
Students should know that ethanol for use as a biofuel is produced from a dilute
solution of ethanol
obtained by the fermentation of plant materials at a temperature between 20 °C
and 35 °C. Detailed
knowledge of the methods used to produce other biofuels is
not
required.
ALKANES - saturated hydrocarbons,
physical and chemical properties - combustion
Alcohols - Ethanol
- manufacture, properties and reactions
Biofuels,
biomass, biodiesel, comparison of alternative fuels
Obtaining useful substances from crude oil
(Oxford AQA International GCSE Combined Science Double award)
a.
Hydrocarbons can be broken down (cracked) to produce smaller, more useful
molecules. This process
involves heating the hydrocarbons to vaporise them. The vapours are either
passed over a hot catalyst or
mixed with steam and heated to a very high temperature so that thermal
decomposition reactions then
occur.
b.
The products of cracking include alkanes and unsaturated hydrocarbons called
alkenes. The general formula
for the homologous series of alkenes is CnH2n
Students should know that in unsaturated hydrocarbons some of the carbon–carbon
bonds are double
covalent bonds.
c.
Unsaturated hydrocarbon molecules can be represented in the following forms:
C3H6
or
Students should know that in displayed structures
represents a double bond.
Students should be able to recognise alkenes from their names or formulae, but
do
not
need to know the
names of individual alkenes other than ethene and propene.
d.
Alkenes react with bromine water, turning it from orange to colourless.
e.
Some of the products of cracking are useful as fuels
Cracking - a problem of supply and demand, other products
ALKENES - unsaturated hydrocarbons,
physical and chemical properties
Synthetic and naturally occurring polymers
(Oxford AQA International GCSE Combined Science Double award)
a.
Alkenes can be used to make polymers such as poly(ethene) and poly(propene). In
polymerisation
reactions, many small molecules (monomers) join together to form very large
molecules (polymers).
For example - the formation of the polymer poly(ethene) from the monomer ethene
Students should be able to recognise the molecules involved in these reactions
in the forms shown in
the subject content. They should be able to represent the formation of a polymer
from a given alkene
monomer.
Further details of polymerisation are
not
required.
b.
The properties of polymers depend on what they are made from and the conditions
under which they are
made. For example, low-density (LD) and high-density (HD) poly(ethene) are
produced using different
catalysts and reaction conditions.
c.
Thermosoftening polymers consist of individual, tangled polymer chains.
Thermosetting polymers consist
of polymer chains with cross-links between them so that they do not melt when
they are heated.
Extension Tier students should be able to explain thermosoftening polymers in
terms of intermolecular
forces.
d.
Polymers have many useful applications and new uses are being developed.
Examples include: new
packaging materials, waterproof coatings for fabrics, dental polymers, wound
dressings, hydrogels, and
smart materials (including shape memory polymers).
Students should consider the ways in which new materials are being developed and
used, but will not need
to recall the names of specific examples.
e.
Many polymers are not biodegradable, ie they are not broken down by microbes.
This can lead to problems
with waste disposal.
Knowledge of specific named examples is
not
required, but students should be aware of the problems that
are caused in landfill sites and in litter.
f.
Plastic bags are being made from polymers and cornstarch so that they break down
more easily.
Biodegradable plastics made from cornstarch have been developed
Addition polymers - plastics,
structure, manufacture and uses
e.g. PE, PP, PVC, PTFE, PS
More on the
uses of plastics, issues with using plastics, solutions and recycling
methods
Organic compounds – their structure and reactions
Alcohols
(Oxford AQA International GCSE Combined Science Double award)
a.
Alcohols contain the functional group –OH. Methanol, ethanol and propanol are
the first three members of
a homologous series of alcohols. Alcohols can be represented in the following
forms:
CH3CH2OH or
Students should be able to recognise alcohols from their names or formulae, but
do
not
need to know the
names of individual alcohols other than methanol, ethanol and propanol.
b.
Methanol, ethanol and propanol:
•
dissolve in water to form a neutral solution
•
react with sodium to produce hydrogen
•
burn in air
•
are used as fuels and solvents, and ethanol is the main alcohol in alcoholic
drinks.
c.
Ethanol can be oxidised to ethanoic acid, (a carboxylic acid) either by chemical
oxidising agents or by
microbial action. Ethanoic acid is the main acid in vinegar.
Alcohols - Ethanol
- manufacture, properties and reactions
Carboxylic acids
(Oxford AQA International GCSE Combined Science Double award)
a.
Ethanoic acid is a member of the homologous series of carboxylic acids, which
have the functional group
–COOH. The structures of carboxylic acids can be represented in the following
forms:
CH3COOH or
Students should be able to recognise carboxylic acids from their names or
formulae, but do
not
need to
know the names of individual carboxylic acids other than methanoic acid,
ethanoic acid and propanoic acid.
b.
Carboxylic acids:
•
dissolve in water to produce acidic solutions
•
react with carbonates to produce carbon dioxide
•
react with alcohols in the presence of an acid catalyst to produce esters
•
do not ionise completely when dissolved in water and so are weak acids
•
aqueous solutions of weak acids have a higher pH value than aqueous solutions of
strong acids with the
same concentration.
Students are expected to write balanced chemical equations for the reactions of
carboxylic acids.
Carboxylic acids
- chemistry and uses
PHYSICS
(Oxford AQA International GCSE Combined Science Double award)
FORCES AND THEIR EFFECTS
(Oxford AQA International GCSE Combined Science Double award)
This topic explores the interactions (forces) between objects that can change
their shape or the way they are
moving. Mathematical relationships can predict the resultant motion of an object
and applications illustrate
how forces can be used to achieve certain outcomes and avoid others.
Forces and their interactions
(Oxford AQA International GCSE Combined Science Double award)
a.
Objects interact by non-contact (field) forces (including gravity,
electrostatics, magnetism) and by contact
forces (including friction, air resistance, tension and normal contact force).
b.
Friction is a force between two surfaces, which impedes motion and may result in
heating. Air resistance is
a form of friction.
c.
Pairs of objects interact to produce a force on each other, which can be
represented as vectors.
d.
Scalars are quantities that have magnitude only. Vectors are quantities that
have direction as well as a
magnitude. A vector quantity may be represented by an arrow. The length of the
arrow represents the
magnitude and the direction of the arrow represents the direction of the vector
quantity.
Students should be aware that distance, speed and time are examples of scalars
and displacement,
velocity, acceleration, force and momentum are examples of vectors.
e.
Weight is the force acting on an object due to gravity. The weight of an object
depends on the gravitational
filed strength at the point where the object is. The weight of an object can be
calculated using the
equation:
Weight (N)
= mass (kg)
× gravitational field strength
(N/kg)
W = m × g
Students will
not
be expected to know the value of
g;
it will be given in any examination items.
f.
A force applied to an elastic object such as a spring will result in the object
stretching and storing elastic
potential energy.
g.
For an object behaving elastically, the extension is directly proportional to
the force applied, provided that
the limit of proportionality is not exceeded. The relationship between the
force,
F,
and the extension,
e,
is:
F
=
k
×
e
(where
k
is a constant).
h.
Required practical:
Investigate the relationship between force and extension for a spring
What are contact forces &
non-contact forces?, scalar & vector quantities, free body force diagrams
Mass and the effect of gravity force on it - weight, (mention of work done,
GPE and circular motion)
Elasticity and energy stored in a spring, experimental investigations and
calculations
Resultant forces
(Oxford AQA International GCSE Combined Science Double award)
a.
Whenever two objects interact, the forces they exert on each other are equal in
magnitude and opposite in
direction. This is Newton’s Third Law.
b.
A number of forces acting on an object may be replaced by a single force that
has the same effect on the
motion as all the original forces acting together. This single force is called
the resultant force.
Students should be able to determine the resultant of opposite or parallel
forces acting in a straight line and
determine the resultant of two coplanar forces by scale drawing.
c.
A non-zero resultant force acting on an object causes it to accelerate.
d.
Acceleration is the rate of change of velocity. An object can accelerate by
changing its direction even if it is
going at a constant speed. Deceleration is a negative acceleration. The average
acceleration,
a,
of an object
is given by the equation:
a
= ∆v / t (where
∆v
is the change in velocity and
t
is the time taken for the object to accelerate)
e.
The acceleration of an object can be calculated from the gradient of the
velocity–time graph.
f.
The distance travelled by an object can be calculated from the area under a
velocity–time graph.
g.
If the resultant force acting on an object is zero:
•
a moving object will continue to move at the same velocity
•
a stationary object will remain at rest.
This is Newton’s First Law.
h.
If the resultant force on an object is not zero, the object will accelerate in
the direction of the resultant
force. The relationship between the resultant force,
F,
acting on an object, its mass,
m,
and the
acceleration caused,
a,
is:
F
=
m
x a
This is Newton’s Second Law.
Newton's Laws of
Motion including F = ma calculations
Calculating resultant forces using vector
diagrams, also includes work done calculations
Speed and velocity - the relationship between
distance and time, distance-time graphs
Acceleration, velocity-time graph interpretation and calculations,
problem solving
Safety in public transport
(Oxford AQA International GCSE Combined Science Double award)
a.
When a vehicle travels at a steady speed in a straight line the resistive forces
are balancing the driving
force.
b.
The greater the speed of a vehicle the greater the braking force needed to stop
it in a certain distance. The
greater the braking force the greater the deceleration of the vehicle. Large
decelerations may lead to brakes
overheating and/or loss of control.
Students should understand that, for a given braking force, the greater the
speed, the greater the stopping
distance.
c.
The stopping distance of a vehicle is the sum of the distance the vehicle
travels during the driver’s reaction
time (thinking distance) and the distance it travels under the braking force
(braking distance). A driver’s
reaction time can be affected by tiredness, distractions, drugs and alcohol.
d.
When the brakes of a vehicle are applied, work done by the friction force
between the brakes and the wheel
reduces the kinetic energy of the vehicle and the temperature of the brakes
increases.
e.
A vehicle’s braking distance can be affected by adverse road and weather
conditions and poor condition of
the vehicle.
Students should understand that ‘adverse road conditions’ includes wet or icy
conditions. Poor condition of
the car is limited to the car’s brakes or tyres.
Reaction times, stopping distances, safety
aspects
ENERGY
(Oxford AQA International GCSE Combined Science Double award)
This topic starts with the principles of energy transfer and then explores it in
various contexts, such as
heating. It considers the idea that energy is never destroyed but may end up so
dissipated that it is of little
use.
Forces and energy
(Oxford AQA International GCSE Combined Science Double award)
a.
Work is done when a force causes an object to move through a distance. The
relationship between work
done,
W,
force,
F,
and distance,
d,
moved in the direction of the force is:
W
=
F x
d
b.
Energy is transferred when work is done. Work done against frictional forces
causes energy transfer by
heating.
Students should be able to discuss the transfer of kinetic energy in particular
situations, for example shuttle
re-entry into the atmosphere or meteorites burning up in the atmosphere and
braking systems on vehicles.
c.
The amount of elastic potential energy stored in a stretched spring (assuming
the limit of proportionality
has not been exceeded) can be calculated using the equation:
Ee
= ½ ×
k
×
e2
(E = stored energy, k = spring constant, e = spring extension, watch the units)
d.
An object gains gravitational potential energy when it is raised vertically
because work is done against the
gravitational force. The relationship between gravitational potential energy,
Ep
, mass,
m,
gravitational field
strength,
g,
and height,
h,
is:
Ep =
m
× g ×
h
e.
The kinetic energy of a moving object depends on its mass and its velocity. The
relationship between
kinetic energy,
Ek
, mass,
m
and velocity,
v,
is: Ek
=
½ ×
m ×
V2
Students should understand that when the mass of an object is doubled, if it is
travelling at the same speed
it will have twice the kinetic energy. They should understand that an object
travelling at twice the speed of
another object with the same mass will have four times the kinetic energy and
should be able to apply this
idea in the context of road safety.
f.
Power is the rate at which energy is transferred or the rate at which work is
done. The relationship between
power,
P,
work done,
W,
or energy transferred,
E,
and time,
t,
is: P = E / t and P = W / t (and watch the units, J, s
and W, 1W = 1J/s)
Mass and the effect of gravity force on it - weight, (mention of work done,
GPE and circular motion)
Elasticity and energy stored in a spring, experimental investigations and
calculations
Elastic
potential energy stores and calculations
Gravitational potential
energy and calculations
Kinetic
energy stores
and calculations
Types of energy & stores - examples compared/explained, calculations of
mechanical work done & power
Energy transfers, conservation and dissipation of energy
a.
When a system changes, energy is transferred. A system is an object or group of
objects.
Students should be able to identify when and where energy has been transferred
using concepts such as
kinetic energy, gravitational potential energy and elastic potential energy.
b.
A simple pendulum is an example of oscillating motion and energy is transferred
between kinetic energy
and gravitational potential energy.
c.
Energy can be transferred usefully, stored or dissipated, but cannot be created
or destroyed.
d.
When energy is transferred only part of it may be usefully transferred; the rest
is dissipated so that it is
stored in less useful ways. This energy is often described as being ‘wasted’.
e.
Friction and air resistance are forces that dissipate energy by heating the
surroundings.
f.
The efficiency of a device can be calculated using:
%
efficiency = 100 x (useful energy out) /
(total energy in)
and
also % efficiency =
(useful power out) /
(total power in)
(× 100
%)
Students may be required to calculate efficiency as a decimal or as a
percentage.
g.
The energy flow in a system can be represented using Sankey diagrams.
Students should be able to draw and interpret Sankey diagrams to show how the
overall energy in a system
is redistributed when the system is changed but there is no net change to the
total energy
Conservation of energy,
energy transfers-conversions, efficiency - calculations and
Sankey diagrams
Energy resources
(Oxford AQA International GCSE Combined Science Double award)
a.
Fuels are a useful store of energy; different fuels are suitable for different
situations and are selected
according to a range of factors, such as ease of storage, energy content and
safety.
b.
When a fuel is used, some energy is transferred to the surroundings. Some fuels
are more efficient than
others.
c.
There is a range of energy sources used on a national and global scale. Their
use has implications for
society in terms of factors including renewability and the environmental impacts
of extraction, use and
disposal.
d.
A range of technologies have been developed to provide energy in a renewable
way, such as wave power,
solar power and geothermal power.
Students should be aware of these and other examples and be able to identify
advantages and drawbacks
with their use.
Types of energy & stores - examples compared and explained
Renewable energy (1) Wind power and
solar power, advantages and disadvantages
Renewable energy (2) Hydroelectric power and
geothermal power,
advantages and disadvantages
Renewable energy (3) Wave power and tidal barrage power,
advantages and disadvantages
WAVES
(Oxford AQA International GCSE Combined Science Double award)
Waves, both transverse and longitudinal, carry energy from a source and can be
detected by a receiver. This
topic explores the properties of waves and their application to contexts such as
information communication
and sight.
General properties of waves
(Oxford AQA International GCSE Combined Science Double award)
a.
A wave is a disturbance caused by an oscillating source that transfers energy
and information in the
direction of wave travel, without transferring matter.
b.
In a transverse wave the oscillations are perpendicular to the direction of
energy transfer.
c.
In a longitudinal wave the oscillations are parallel to the direction of energy
transfer. Longitudinal waves
have areas of compression and rarefaction.
d.
Electromagnetic waves and water waves are transverse, sound waves are
longitudinal and mechanical
waves may be either transverse or longitudinal.
e.
Waves can be reflected, transmitted or absorbed (or a combination of these) at
the boundary between two
different materials.
f.
Waves can undergo refraction due to a change in speed and diffraction through a
narrow gap or at an edge.
Students should appreciate that for appreciable diffraction to take place the
wavelength of the wave has
to be comparable to the size of the obstacle or gap.
Students may be required to
apply these ideas to the
reduction of diffraction in optical instruments, ultrasound waves in medicine
and radio wave reception.
Required practical:
Investigate the refraction of light in glass blocks.
g.
Wave motion can be described in terms of their frequency, wavelength, period,
amplitude and wavefront.
Students should be able to explain the meaning of these terms.
h.
The relationship between wave speed,
v,
frequency,
f,
and wavelength,
λ,
is:
v
= f
×
λ
General
introduction to the types and properties of waves, ripple tank expts, how to do
wave calculations
Refraction and diffraction, the visible light
spectrum, prism investigations, ray diagrams explained
Electromagnetic spectrum,
sources, types, properties, uses (including medical) and dangers
The electromagnetic spectrum
(Oxford AQA International GCSE Combined Science Double award)
a.
Electromagnetic waves are transverse waves that transfer energy from the source
of the waves to an
absorber.
b.
Electromagnetic waves form a continuous spectrum and all types of
electromagnetic wave travel at the
same speed through a vacuum (space).
Students should know the order of electromagnetic waves within the spectrum,
grouped in terms of energy,
frequency and wavelength. They should appreciate that the wavelengths of the
electromagnetic spectrum
range from 10–15
m to 104
m and beyond.
c.
Visible light is the part of the electromagnetic spectrum that is detected by
our eyes; we see different
wavelengths as different colours.
d.
All objects emit and absorb infrared radiation. The hotter an object is the more
infrared radiation it radiates
in a given time.
•
Dark, matt surfaces are good absorbers and good emitters of infrared radiation.
•
Light, shiny surfaces are poor absorbers and poor emitters of infrared
radiation.
•
Light, shiny surfaces are good reflectors of infrared radiation.
e.
Radio waves, microwaves, infrared and visible light can be used for
communication.
f.
Electromagnetic waves have many practical applications. For example:
•
radio waves – television and radio systems (including Bluetooth)
•
microwaves – mobile phones and satellite television systems
•
infrared – TV remote controls, night vision devices, heating
•
visible light – photography, fibre optic communications
•
ultraviolet – security marking
•
X-rays – medical imaging
•
gamma rays – sterilising surgical instruments and killing harmful bacteria in
food.
g.
Excessive exposure of the human body to electromagnetic waves can be hazardous.
Low energy waves
have a heating effect and higher energy waves have enough energy to cause
ionisation (remove an electron
from an atom or molecule). For example:
•
microwaves – heating of body tissue
•
infrared – skin burns
•
ultraviolet – skin cancer and blindness
•
X-rays – high doses kill cells
•
gamma rays – genetic mutations.
Students should be able to describe simple protection measures against risks.
h.
X-rays are part of the electromagnetic spectrum. They have a very short
wavelength, high energy and
cause ionisation
i.
Properties of X-rays include:
•
they affect a photographic film in the same way as light
•
they are absorbed strongly by metal and bone
•
they are transmitted by healthy tissue.
j.
X-rays can be used to diagnose some medical conditions, for example in computed
tomography (CT)
scanning, bone fractures and dental problems. X-rays are also used to treat some
conditions, for example
in killing cancer cells.
k.
The use of high energy ionising radiation can be dangerous, and precautions need
to be taken to monitor
and minimise the levels of radiation that people who work with it are exposed to.
Electromagnetic spectrum,
sources, types, properties, uses (including medical) and dangers
Absorption
and emission of radiation - temperature & surface factors including global warming
Sound
(Oxford AQA International GCSE Combined Science Double award)
a.
Sound waves are longitudinal waves and cause vibrations in a medium, which are
detected as sound. The
range of human hearing is about 20 Hz to 20 000 Hz.
No
details of the structure of the ear are required.
b.
The pitch of a sound is determined by the frequency of vibrations of the source.
Its loudness is related to
the size of the amplitude of the disturbance.
c.
Sound waves can be reflected (echoes) and diffracted.
Sound waves, properties explained, speed measure,
uses of sound, ultrasound, infrasound, earthquakes
Reflection
(Oxford AQA International GCSE Combined Science Double award)
a.
When waves are reflected the angle of incidence is equal to the angle of
reflection.
b.
The normal is a construction line perpendicular to the reflecting surface at the
point of incidence.
c.
The image produced in a plane mirror is virtual, upright and laterally inverted.
Students will be expected to be able to construct ray diagrams to represent the
changing path of reflected
rays.
Section on reflection and mirror uses
PARTICLE MODEL OF MATTER
(Oxford AQA International GCSE Combined Science Double award)
The properties of materials can be understood in terms of constituent particles,
their motions and
interactions.
Kinetic theory
(Oxford AQA International GCSE Combined Science Double award)
a.
Kinetic theory can be used to explain the different states of matter and their
properties. The particles in
solids, liquids and gases have different amounts of energy.
Students should be able to recognise, use and compare simple diagrams to
represent key features of solids,
liquids and gases.
b.
The specific heat capacity of a substance is the amount of energy required to
change the temperature
of one kilogram of the substance by one degree Celsius. The relationship between
energy,
E,
mass,
m,
specific heat capacity,
c,
and temperature change, ∆θ,
is: E
=
m
× c ×
∆θ
c.
The specific latent heat of vaporisation of a substance is the amount of energy
required to change the
state of one kilogram of the substance from a liquid to a vapour with no change
in temperature. The
relationship between energy,
E,
mass,
m,
and specific latent heat of vaporization,
LV
, is:
E
=
m
×
LV
d.
The specific latent heat of fusion of a substance is the amount of energy
required to change the state of
one kilogram of the substance from a solid to a liquid with no change in
temperature. The relationship
between energy,
E,
mass,
m,
and specific latent heat of fusion,
LF
, is:
E
=
m
×
Lf
e.
The melting point of a solid and the boiling point of a liquid are affected by
impurities.
Throughout this section, students should be able to explain the shape of the
temperature–time graph for a
substance that is either cooled or heated through changes in state.
Particle theory models, internal energy, heat transfer in state changes and
latent heat
Specific heat capacity: how to determine it, use of data,
calculations and thermal energy stores
Energy transfers and particle motion
(Oxford AQA International GCSE Combined Science Double award)
a.
Energy may be transferred by conduction and convection.
Students should be able to explain, in terms of particles, how these energy
transfers take place. They
should understand in simple terms how the arrangement and movement of particles
determine whether a
material is a conductor or an insulator and understand the role of free
electrons in conduction through a
metal. They should be able to use the idea of particles moving apart to make a
fluid less dense, to explain
and apply the concept of convection.
b.
Energy may be transferred by evaporation and condensation.
Students should be able to explain evaporation, and the cooling effect this
causes, using kinetic theory.
Students should be able to discuss the factors that affect the rate of
evaporation.
c.
The rate at which an object transfers energy by heating depends on:
•
its surface area and volume
•
the material from which the object is made
•
the nature of the surface with which the object is in contact.
Students should be able to explain the design of devices in terms of energy
transfer, for example cooling
fins, and should be able to explain animal adaptations in terms of energy
transfer, for example relative ear
size of animals in cold and warm climates.
d.
The bigger the temperature difference between an object and its surroundings,
the faster the rate at which
energy is transferred by heating.
e.
Most substances expand when heated.
Students should understand that the expansion of substances on heating may be a
hazard (for example,
the expansion of roofs and bridges) or useful (for example, the bi-metallic
strip thermostat).
Introduction to heat transfer - conduction
(and thermal conductivity),
convection and radiation
ELECTRICITY AND MAGNETISM
(Oxford AQA International GCSE Combined Science Double award)
Electricity is convenient because it is easily transmitted over distances and
can be easily transferred in a range
of different ways. By controlling the flow of current and understanding the
factors that affect this flow it can
be used to make a range of applications work. Electricity is also a good context
for considering how energy
is transferred. Magnetism provides a connection with forces through the study of
fields and the way it can
produce and be produced by electricity.
Electrical circuits
(Oxford AQA International GCSE Combined Science Double award)
a.
Electrical charges can move easily through some substances; for example metals
have many charges
(electrons) that are free to move.
b.
Electric current is the rate of flow of electric charge. Charge flow,
Q,
current,
I,
and time,
t,
are linked by the
equation:
I = Q / t
c.
The voltage of a source is the energy supplied by a source in driving charges
round a complete circuit and is
measured in volts.
d.
Potential difference across a component measures the energy transfer by charges
and is measured in volts.
e.
The relationship between potential difference,
V,
energy transferred,
E,
and charge,
Q,
is: V = E / Q
Teachers can use either of the terms potential difference or voltage. Questions
will be set using the term
potential difference. Students will gain credit for the correct use of either
term.
Ohm's Law, experimental investigations of
resistance, I-V graphs, calculations V = IR, Q = It, E = QV
f.
Circuit diagrams use standard symbols.
Students will be required to interpret and draw circuit diagrams. Students
should know the following
standard symbols:
Students should understand the use of thermistors in circuits, for example
thermostats.
Electrical circuits and how to draw them, circuit symbols, parallel
circuits and series circuits explained
Students should understand the use of light-dependent resistors (LDRs) in
circuits, for example switching
lights on when it gets dark.
g.
Components resist the flow of charge through them. The greater the resistance
the smaller the current
for a given potential difference across the component. The resistance of a
component can be found by
measuring the current through and potential difference across, the component.
The relationship between
potential difference,
V,
current,
I,
and resistance,
R,
is:
V=
I
×
R
h.
The current through a resistor (at a constant temperature) is directly
proportional to the potential
difference across the resistor. This means that the resistance remains constant
as the current changes, graph (1) below.
i.
The resistance of components such as lamps, diodes, thermistors and LDRs is not
constant; it changes
with the current through the component.
j.
The resistance of a filament lamp increases as the temperature of the filament
increases, graph (2) above.
Ohm's Law, experimental investigations of
resistance, I-V graphs, calculations V = IR, Q = It, E = QV
Circuit devices and how are they used explained (e.g. thermistor, LDR, diode), relevant graphs
Students should be able to explain change in resistance in terms of ions and
electrons.
k.
An LED emits light when a current flows through it in the forward direction.
Students should be aware that the use of LEDs for lighting is increasing, as
they use a much smaller current
than other forms of lighting.
l.
The combined voltage of several sources in series is their sum.
m.
There are two ways of joining electrical components: in series and in parallel.
Some circuits include both
series and parallel parts.
n.
For components connected in series:
•
the combined resistance is the sum of the resistance of each component
•
the current is the same in each component
•
the total potential difference of the power supply is shared between the
components.
o.
For components connected in parallel:
•
the combined resistance is less than that of either component
•
the current from the supply splits in the branches
•
the potential difference across each component is the same.
p.
When an electrical charge flows through a resistor, the resistor gets hot
because of collisions between
moving charges and stationary atoms in the wire.
Students should understand that a lot of energy is wasted in filament bulbs by
heating. Less energy is
wasted in power saving lamps such as Compact Fluorescent Lamps (CFLs). They
should understand that
there is a choice when buying new appliances in how efficiently they transfer
energy.
Electrical circuits and how to draw them, circuit symbols, parallel
circuits and series circuits explained
Ohm's Law, experimental investigations of
resistance, I-V graphs, calculations V = IR
More on series and parallel circuits,
circuit diagrams, measurements and calculations
Magnetism and electromagnetism
(Oxford AQA International GCSE Combined Science Double award)
a.
Magnetic forces are strongest at the poles of a magnet. When two magnets are
brought close together
they exert a force on each other. Two like poles repel each other and two unlike
poles attract. Attraction and
repulsion between two magnetic poles are examples of non-contact forces.
Students should be able to predict the interaction between magnets given their
physical arrangement.
b.
The space around a magnet where a force acts on another magnet or on a magnetic
material (iron, steel,
cobalt, nickel) is called a magnetic field. The strength and direction of a
magnetic field change from one
point to another.
Students should be able to recognise magnetic field patterns using one or two
bar magnets. In a uniform
magnetic field the lines of the magnetic field are parallel.
c.
An induced magnet is a material that becomes a magnet when it is placed in a
magnetic field. Induced
magnetism always causes a force of attraction. When removed from the magnetic
field an induced magnet
loses most/all of its magnetism quickly.
Students should be able to explain how a magnet attracts a magnetic object by
inducing a magnetic field
around it.
d.
The earth has a magnetic field that is most concentrated at the magnetic north
and south poles.
Students should be able to explain how a plotting compass can be used to detect
the earth’s magnetic field
and to assist in navigation.
Magnetism
- magnetic materials - temporary (induced) and permanent magnets - uses
e.
A magnetic field is produced when an electric current flows through a wire. The
magnetic field lines are
concentric circles in a plane, perpendicular to the wire
The field is stronger closer to the wire.
•
Increasing the current makes the magnetic field stronger.
•
Reversing the current reverses the direction of the magnetic field lines.
f.
Shaping a wire to form a solenoid increases the strength of the magnetic field
created by a current through
the wire. The magnetic field inside a solenoid is strong and uniform.
g.
The magnetic field around a solenoid has a similar shape to that of a bar
magnet. Adding an iron core
increases the magnetic field strength. An electromagnet consists of a solenoid
with an iron core.
Students should be familiar with some typical uses of electromagnets.
Required practical:
Investigate the factors that determine the strength of an electromagnet
Electromagnetism, solenoid coils, uses of electromagnets
GENERATING AND DISTRIBUTING ELECTRICITY AND HOUSEHOLD
USE
In this topic magnetism and electromagnetism are studied in the context of their
uses in using current to
cause motion and vice versa and in changing the voltages of an ac supply. In so
doing the big ideas of field
forces and energy transfer are also used.
Using electricity in the home
(Oxford AQA International GCSE Combined Science Double award)
a.
Cells and batteries supply current that always passes in the same direction.
This is called direct current (dc).
b.
An alternating current (ac) is one that is repeatedly changing direction.
Students should be able to determine the period, and hence the frequency, of a
supply from diagrams.
They should be able to compare and calculate potential differences of dc
supplies and the peak potential
differences of ac supplies from diagrams.
c.
Mains electricity is an ac supply, which has a set frequency and voltage.
Knowledge of root mean square (rms) measurements and values are not required.
d.
There are a number of safety features that can be incorporated in electrical
systems and appliances. One of
these is earthing: if the metal body of an appliance becomes live through a
fault, the current is harmlessly
conducted away.
e.
If an electrical fault causes too great a current to flow, a fuse or a circuit
breaker in the live wire disconnects
the circuit. The current will cause the fuse wire to overheat and melt or the
circuit breaker to switch off
(‘trip’). A circuit breaker operates much faster than a fuse and can be reset.
f.
Appliances with metal cases are usually earthed. If a fault develops a large
current flows from the live wire
to earth. This melts the fuse and disconnects the live wire.
Students should be aware that some appliances are double insulated and therefore
have no earth wire
connection.
Usefulness of electricity, safety-fuses, energy transfer, cost & power calculations
The motor effect
(Oxford AQA International GCSE Combined Science Double award)
a.
A current carrying conductor has a magnetic field around the wire. When a
current carrying conductor
is placed in a magnetic field so that it cuts lines of magnetic force, the
magnet and the conductor exert
a force on each other. This is called the motor effect. The conductor will not
experience a force if it is
parallel to the magnetic field.
b.
The size of the force can be increased by:
•
increasing the strength of the magnetic field
•
increasing the size of the current
•
increasing the length of the conductor in the magnetic field.
c.
The direction of the force is reversed if either the direction of the current or
the direction of the magnetic
field is reversed.
Students should be able to identify the direction of the force using Flemings
left-hand rule.
d.
A coil of wire carrying a current in a magnetic field tends to rotate. This is
the basis of an electric motor.
Motor effect of an electric current
and Fleming's left-hand rule, F = BIL
Transferring electrical energy
(Oxford AQA International GCSE Combined Science Double award)
a.
Electrical appliances are designed to transfer energy.
Students should be able to give examples of such devices and identify the energy
transfers.
b.
The rate at which energy is transferred by an appliance is called the power. The
relationship between power,
P,
energy transferred,
E,
and time,
t,
is:
P
=
E /
t
c.
The power transfer,
P,
in any device is related to the current,
I,
flowing through it and potential difference,
V,
across it:
P =
×
I
V
Students should be able to calculate the current through an appliance from its
power and the potential
difference of the supply and from this determine the size of fuse needed.
d.
The relationship between energy transferred,
E,
potential difference,
V,
and charge,
Q,
is:
E =
V
×
Q
e.
The amount of energy an appliance transfers depends on how long the appliance is
switched on for and
its power rating. It is often more convenient to measure energy transfers in
domestic appliances in
kWh
instead of
J
due to the small size of the latter.
f.
The relationship between energy transferred,
E,
from the mains, power,
P,
and time,
t,
is:
E(kWh) =
P(kW)
x
t(h)
Students will
not
be required to convert between kilowatt-hours and joules.
Students should be able to calculate the cost of mains electricity given the
cost per kilowatt-hour and
interpret and use electricity meter readings to calculate total cost over a
period of time.
Usefulness of electricity,
safety-fuses, energy transfer, cost & power calculations, P = IV and
E = Pt
Ohm's Law, experimental investigations of
resistance, I-V graphs, calculations V = IR, Q = It, E = QV
NUCLEAR PHYSICS
(Oxford AQA International GCSE Combined Science Double award)
The structure of material is used to model what an atom consists of, what might
happen when atoms break
apart and when they fuse together. This provides ways of actually or potentially
generating power and explains
processes at the centre of stars.
Atomic structure
(Oxford AQA International GCSE Combined Science Double award)
The structure of material is used to model what an atom consists of, what might
happen when atoms break
apart and when they fuse together. This provides ways of actually or potentially
generating power and explains
processes at the centre of stars.
a. Atoms are very small, having a radius of about 10 -10 metres. The simple
model of an atom is a small central
positively charged nucleus composed of protons and neutrons, surrounded by
electrons. The radius of the
nucleus is much smaller than that of the atom with almost all of the mass in the
nucleus.
b. The scattering of alpha particles by thin metal foil provides evidence of the
distribution of mass in the
atom.
c. The relative masses and electric charges of protons, neutrons and electrons
are as follows:
Sub–atomic particle |
Relative mass |
Electric charge |
Comments |
Proton |
1 |
+1
(+ positive) |
In
the nucleus, a nucleon |
Neutron |
1 |
0
(zero) |
In the nucleus, a nucleon |
Electron |
1/1850 or 0.00055 very small |
–1
(– negative) |
NOT a nucleon. Electrons are arranged in energy levels or shells
in orbit around the nucleus |
d. In an atom the number of electrons is equal to the number of protons in the
nucleus. The atom has no
overall electrical charge.
e. In each atom its electrons are arranged at various distances from the
nucleus. Atoms may lose or gain
outer electrons to form charged particles called ions.
f. The atoms of a particular element always have the same number of protons, but
have a different number
of neutrons for each isotope. The total number of protons in an atom is called
its proton number or atomic
number. The total number of protons and neutrons in an atom is called its mass
number. Atoms can be
represented as shown:
:
mass number
of
23,
atomic number
11
for sodium
Ionizing radiation from the nucleus
(Oxford AQA International GCSE Combined Science Double award)
a.
Some atomic nuclei are unstable. The nucleus emits particles or radiation and
the nucleus changes to that
of a different element and becomes more stable. This is a random process called
radioactive decay.
b.
Energy is emitted by changes in the nucleus.
c.
Unstable nuclei emit alpha particles, beta particles, or neutrons, and
electromagnetic radiation as gamma
waves. Neither chemical nor physics processes affect this behaviour. These
substances are said to be
radioactive and although the general process follows a pattern this radioactive
decay is a random process.
It is impossible to predict when a particular atom might decay.
d.
Background radiation is around us all of the time. It comes from a range of
sources, such as radioactive
substances in the environment, from space or from devices such as X-ray machines
in hospitals.
e.
An alpha particle consists of two neutrons and two protons (i.e. a Helium
nucleus). A beta particle is
a high speed electron ejected from the nucleus as a neutron turns into a proton.
Gamma radiation is
electromagnetic radiation from the nucleus.
f.
Nuclear equations are used to represent radioactive decay.
Students will be required to balance equations for single alpha and beta decay,
limited to the completion
of atomic number and mass number. The identification of daughter elements from
such decays is not
required.
g.
Properties of the alpha, beta and gamma radiations are limited to their relative
ionising power, their
penetration through materials and their range in air.
Atomic structure, history, definitions,
examples and explanations including isotopes (GCSE chemistry)
Atomic
structure and fundamental particle knowledge needed to understand radioactivity
(GCSE physics)
What
is Radioactivity? Why does it happen? Three types of atomic-nuclear-ionising radiation
Detection of
radioactivity, its measurement
and radiation dose units,
ionising
radiation sources
- radioactive materials, background radiation
Alpha, beta & gamma radiation - properties of 3 types of radioactive
nuclear emission & symbols
,dangers of radioactive emissions - health and safety issues and ionising radiation
What
actually happens to the nucleus in alpha and beta radioactive decay and why? nuclear
equations!
Nuclear fission
(Oxford AQA International GCSE Combined Science Double award)
a.
Nuclear fission is the splitting of a large and unstable nucleus and the release
of energy.
b.
For fission to occur the uranium-235 or plutonium-239 nucleus must first absorb
a neutron to make the
nucleus unstable. The nucleus undergoing fission splits into two smaller nuclei,
releasing two or three
neutrons and energy. The amount of energy released during nuclear fission is
much greater than that
released in a chemical reaction involving a similar mass of material.
c.
A chain reaction occurs when neutrons from the fission go on to cause further
fission. In a nuclear reactor
control rods absorb fission neutrons to ensure that on average only one neutron
per fission goes on to
produce further fission and energy transfer.
Students should be able to sketch or complete a labelled diagram to illustrate
how a chain reaction may
occur.
d.
Nuclear reactions produce waste which may be dangerous due to its radioactive
nature and may remain so
for a long time, depending upon its half life and products. The disposal of such
waste needs to be managed
with care and is a factor that may influence the use of nuclear power for the
generation of electricity.
Nuclear Fission Reactions, nuclear power
as an energy resource
SPACE PHYSICS
(Oxford AQA International GCSE Combined Science Double award)
Space physics uses ideas about forces and motion, energy transfer, atomic
structure and fields to develop
explanations about the start and end of the universe and about how the Earth
receives energy from the
Sun. Space was one of the first challenges that civilisation tried to explain in
its attempts to account for day,
season, year and the appearance of the night sky and remains one of the most
challenging due to its scale and
complexity.
Life cycle of a star
(Oxford AQA International GCSE Combined Science Double award)
a.
Stars form when enough dust and gas (mainly hydrogen and helium) from space are
pulled together by
gravitational attraction. Smaller masses may form and be attracted by a larger
mass to become planets, or
even stars.
b.
During the ‘main sequence’ period of its life cycle, energy is released by the
fusion of hydrogen nuclei to
make helium nuclei in the core and a star is stable because the forces within it
are balanced.
The term ‘radiation pressure’ will
not
be required.
c.
The core (centre) of a star is where the temperature and density are greatest
and where most nuclear
fusion takes place.
d.
The more massive a star, the hotter its core and the heavier the nuclei it can
create by fusion.
e.
Stars change over time; they have a life cycle. This life cycle is determined by
the mass of the star.
f.
A main sequence star uses nuclear reactions to produce light and heat. When it
runs out of hydrogen, what
happens next in its life cycle depends upon its mass.
g.
A larger star will swell to become a red supergiant, in which helium nuclei fuse
to form carbon, followed by
further fusion that produces heavier nuclei such as nitrogen and oxygen. It
expands, cools and turns red.
The outer layers then blast away as a supernova is formed. The core then
collapses and depending upon
mass, it forms either a neutron star or a black hole.
h.
A smaller star, similar to our Sun, follows a different sequence, expanding to
become a red giant. It then
sheds out layers of gas, exposing the core as a white dwarf and finally cools to
become a black dwarf.
Students should be familiar with charts that show the life cycles of stars.
i.
Fusion processes in stars are the source of energy and produce all of the
naturally occurring elements.
These elements may be distributed throughout the universe by the explosion of a
massive star (supernova)
at the end of its life.
Students should be able to explain how stars are able to maintain their energy
output for millions of years,
why the early universe contained only hydrogen but now contains a large variety
of different elements and
that elements heavier than iron are formed in a supernova.
Solar system and orbital motion
(Oxford AQA International GCSE Combined Science Double award)
The life cycle of stars - mainly worked out from emitted
electromagnetic radiation
Nuclear
fusion reactions
a.
The Earth is one of eight planets orbiting the Sun (a medium sized star), which
together with other smaller
objects (asteroids, dwarf planets, comets) and moons orbiting several planets,
make up the solar system.
Students should be able to describe the principal differences between planets,
moons, the Sun, comets and
asteroids in terms of relative size and motion.
b.
Our universe is made up of:
•
thousands of millions of galaxies that are each made up of thousands of millions
of stars
•
our Sun is one of thousands of millions of stars in our galaxy called the Milky
Way.
c.
Planets orbit the Sun and a moon is a natural satellite of a planet. Artificial
satellites orbit the Earth and can
be in geostationary or low polar orbits.
d.
Gravity provides the centripetal force that keeps planets and satellites (both
natural and artificial) in orbit.
e.
The force of gravity acts towards the centre of the orbit. This unbalanced force
causes acceleration
towards the centre of the orbit, changing the direction of motion of the body
(its velocity) but not its
speed.
The equation for calculating centripetal force is not required.
f.
The centripetal force due to gravity decreases as the separation of orbiting
masses increases, resulting in
lower orbital speeds.
g.
At a particular separation of the masses, the centripetal force results in a
particular orbital speed. To stay
in a stable orbit at a particular distance, the planet or satellite moves at a
particular speed. A change in
orbital speed results in a change in orbital radius.
Students should be able to explain the motion of moons and artificial satellites
and be able to apply this
to the design of satellite placing where the speed will determine the radius of
the satellite’s final position
Astronomy - solar system, planets, moons, stars, galaxies and
use of telescopes and satellites
The exam PERIODIC TABLE
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