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Brown's Chemistry Advanced Level Inorganic Chemistry Periodic Table
Revision Notes
Part
4. Revising Survey of Period 2 Li to Ne
4.1 Survey of the selected physical and
chemical properties of individual elements of Period 2 including, where
appropriate, the reactions with oxygen, chlorine, water and chemical
character of oxide/hydroxide
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All my advanced A level
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GCSE Level
periodic table revision notes
Part 4. Survey
of Period
2: Li across to Ne (8 elements, Z = 3
to 10)
A summary of the
physical and chemical characteristics of the elements of period 2,
lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine and neon.
4.1 Survey of the individual elements Li, Be, B, C,
N, O, F and Ne
Sub-index for this
page: lithium
* beryllium * boron *
carbon * nitrogen * oxygen *
fluorine * neon
 Z = 3 lithium
Li in Group
1 Alkali Metals
-
The
structure of the element:
-
Physical properties:
-
Group, electron configuration
(and oxidation states):
-
Reaction of
element with oxygen:
-
Reaction of
oxide with water:
-
Reaction of
oxide or hydroxide with common mineral acids:
-
Li2O behaves as a
basic oxide dissolving to form
the chloride, sulphate and nitrate salt in the relevant dilute acid.
-
The
hydroxide MOH is a strong base and alkali (since a soluble base) and
similarly forms salts.
-
Li2O(s) + 2HCl(aq)
==> 2LiCl(aq) + H2O(l)
-
Li2O(s) + H2SO4(aq)
==>
Li2SO4(aq) + H2O(l)
-
Li2O(s) + 2HNO3(aq)
==> 2LiNO3(aq) + H2O(l)
-
In all cases the
ionic equations are
-
Reaction of
oxide with strong bases/alkalis:
-
Reaction of
element with chlorine:
-
Reaction of
chloride with water:
-
Reaction of
element with water:
-
Other comments:
-
Links to other pages
on site:
 Z = 4 Beryllium
Be in Group 2 Alkaline Earth
Metals
-
The
structure of the element:
-
Physical properties:
-
Group, electron configuration
(and oxidation states):
-
Reaction of
element with oxygen:
-
Reaction of oxide with
water:
-
Reaction of
oxide with acids:
-
Behaves as a
basic oxide dissolving to form
the chloride, sulphate and nitrate salt in the relevant dilute acid.
-
BeO(s)
+ 2HCl(aq) ==>
BeCl2(aq) + H2O(l)
-
BeO(s)
+ H2SO4(aq) ==>
BeSO4(aq) + H2O(l)
-
BeO(s)
+ 2HNO3(aq) ==>
Be(NO3)2(aq) + H2O(l)
-
In all cases the
ionic equation is:
BeO(s) + 2H+(aq)
==> Be2+(aq) + H2O(l)
-
Reaction of
oxide with strong bases/alkalis:
-
The oxide also
behaves as an acidic oxide by dissolving in strong soluble bases
to form beryllate(II) salts.
-
BeO(s)
+ 2NaOH(aq) + H2O(l) ==>
Na2[Be(OH)4](aq)
-
e.g. forming sodium
beryllate(II) with sodium hydroxide.
-
ionic equation:
BeO(s)
+ 2OH-(aq) + H2O(l)
==> [Be(OH)4]2-(aq)
-
Therefore beryllium
oxide is an amphoteric oxide, because of this dual acid-base
behaviour.
-
Reaction of
element with chlorine:
-
Reaction of chloride
with water:
-
Reaction of
element with water:
-
Other comments:
-
Beryllium shows
considerable anomalous behaviour compared to the rest of Group 2
(Mg to Ra) e.g. the covalent chloride and the amphoteric oxide. It
also has a maximum co-ordination number of 4, e.g. in the tetra-aqa
beryllium(II) ion and the beryllate(II) ion shown above. This applies to all the period 2
elements, but for period 3 e.g. magnesium, the maximum co-ordination number is 6.
-
Links to other pages
on site:
TOP OF PAGE
and sub-index
Z = 5
Boron B in Group 3/13
-
The
structure of the element:
-
Physical properties:
-
Group, electron configuration
(and oxidation states):
-
Reaction of element with oxygen:
-
Reaction of
oxide with water:
-
Reaction of
oxide with acids:
-
Reaction of
oxide with strong bases/alkalis:
-
Reaction of element with chlorine:
-
Reaction of
chloride with water:
-
Reaction of element with water:
-
Other comments:
-
Links to other pages
on site:
TOP OF PAGE
and sub-index
 Z = 6 Carbon C
in Group 4/14
-
The
structure of the element:
-
Non-metal existing as
three allotropes covalently bonded. Diamond (tetrahedral bond
network) and graphite (layers of connected hexagonal rings) have
giant covalent structures Cn where n is an extremely
large number, and a series of large molecules (3rd allotrope) called fullerenes
e.g. C60.
-
Bonding
details and diagrams of the allotropes of carbon.
-
Physical properties:
-
Group, electron configuration
(and oxidation states):
-
Gp4; e.c. 2,4 or 1s22s22p2; (can
be +2,
but usually +4) e.g.
-
(+2) CO, (+4) CO2 and CCl4 etc.
-
Reaction of element with oxygen:
-
Reaction of
carbon dioxide with water:
-
Quite soluble to form
a weakly acid solution of pH 4-5. So called carbonic acid, H2CO3,
does not really exist, but the dissolved carbon dioxide reacts
with water to form hydrogen/oxonium ions and hydrogencarbonate
ions. The equilibrium is very much on the left - hence the fizz in
'fizzy drinks'!
-
Reaction of
oxide with acids:
-
Reaction of
oxide with bases/alkalis:
-
It is a weakly
acidic oxide dissolving sodium hydroxide solution to form sodium
carbonate.
-
CO2(g) + 2NaOH(aq)
==> Na2CO3(aq) + H2O(l)
-
ionic equation:
CO2(g) + 2OH-(aq) ==> CO32-(aq)
+ H2O(l)
-
With excess of
carbon dioxide, sodium hydrogencarbonate is formed.
-
CO2(g) + Na2CO3(aq) + H2O(l) ==> 2NaHCO3(aq)
-
ionic equation:
CO2(g) + CO32-(aq) + H2O(l) ==> 2HCO3-(aq)
-
Reaction of element with chlorine:
-
Reaction of
chloride with water:
-
Reaction of element with water:
-
Other comments:
-
Links to other pages
on site:
TOP OF PAGE
and sub-index
 Z = 7 Nitrogen
N in Group 5/15
-
The structure of the
element:
-
Physical properties:
-
Group, electron configuration
(and oxidation states):
-
Gp5; e.c. 2.5 or 1s22s22p3;
Variety of oxidation states from -3 to +5 e.g.
-
NH3
(-3), N2O (+1), NO (+2), NCl3 (+3), NO2
(+4) and N2O5 and HNO3 (+5).
-
Reaction of element with oxygen:
-
At high temperatures
e.g. in car engines, nitrogen(II) oxide (nitrogen monoxide)
is formed.
-
and the nitrogen(II)
oxide rapidly reacts in air to form nitrogen(IV) oxide (nitrogen
dioxide).
-
The theoretical highest oxide
is N2O5 nitrogen(V) oxide (nitrogen
pentoxide) and does exist.
-
Reaction of
oxides with water:
-
Nitrogen(IV) oxide
dissolves to form an acidic solution of weak nitrous acid and
strong nitric acid.
-
NO and N2O are
neutral oxides but nitrogen(V) oxide is strongly acidic and
dissolves to form nitric acid.
-
Reaction of
oxides with acids:
-
Reaction of
oxides with bases/alkalis:
-
Nitrogen(IV) oxide
or nitrogen dioxide forms sodium nitrite and sodium nitrate with sodium
hydroxide solution.
-
2NO2(g) + 2NaOH(aq)
==> NaNO2(aq) + NaNO3(aq)
+ H2O(l)
-
ionic equation:
2NO2(g) + 2OH-(aq)
==> NO2-(aq) + NO3-(aq)
+ H2O(l)
-
As well as being a
neutralisation reaction, it is also a redox reaction, the oxidation
states of oxygen (-2) and hydrogen (+1) do not change BUT the
oxidation state of nitrogen changes from two at (+4) to one at (+3) and
one at (+5). The simultaneous change of an element into an lower and
upper oxidation sate is sometimes called disproportionation.
-
Reaction of element with chlorine:
-
Reaction of
chloride with water:
-
Reaction of element with water:
-
Other comments:
-
Links to other pages
on site:
TOP OF PAGE
and sub-index
 Z = 8 Oxygen O in Group 6/16
-
The structure of the
element:
-
Non-metal existing as
diatomic molecule, O2, with a double covalent
bond.
-
It has two
allotropes: 'normal oxygen' O2 (dioxygen above) and the
highly unstable and reactive gas ozone, O3 (trioxygen).
-
Physical properties
of the element:
-
Group, electron configuration
(and oxidation states):
-
Gp6; e.c. 2,6 or 1s22s22p4; Normally
(-2) e.g. H2O, CO2 etc. but can have
other ox. states ...
-
e.g. H2O2 (-1), F2O
(+2).
-
Reaction of element with oxygen:
-
Reaction of
oxide with water, acids
or bases/alkalis: Not applicable.
-
Reaction of element with chlorine:
-
Reaction of
chloride with water:
-
Reaction of element with water:
-
Other comments:
-
Links to other pages
on site:
TOP OF PAGE
and sub-index
 Z = 9 Fluorine
F in Group 7/17 The Halogens
-
The structure of the
element:
-
Physical properties:
-
Group, electron
configuration (and oxidation states):
-
Gp7 Halogen; e.c. 2,7
or 1s22s22p5; (only
-1) e.g. HF, ClF, F2O (O is +2!)
-
An extremely
reactive element and readily combines with almost every other
element.
-
Reaction of element
with oxygen:
-
Reaction of
oxide with water:
-
Reaction of
oxide with acids:
-
Reaction of
oxide with bases/alkalis:
-
Reaction of element
with chlorine:
-
Can combine directly
or indirectly to form ClF, ClF3, ClF5 and
ClF7.
-
e.g.
Cl2(g)
+ F2(g) ==> 2ClF(g)
-
Reaction of
chloride with water:
-
Reaction of element
with water:
-
Other comments:
-
Links to other pages
on site:
TOP OF PAGE
and sub-index
 Z = 10 Neon
Ne in Group 0/18 The Noble Gases
-
The
structure of the element:
-
Physical properties:
-
Group, electron configuration
(and oxidation states):
-
Reaction with anything:
-
Other comments:
-
Links to other pages
on site:
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WHAT NEXT?
PLEASE NOTE
GCSE Level periodic table notes are on separate webpages
Sub-index for this
page:
lithium * beryllium * boron
* carbon * nitrogen *
oxygen * fluorine *
neon
Period 2-4 survey
sub-index: 4.1 Period 2 Survey of the
individual elements, 4.2 Period
2 element trends and explanations of physical properties * 4.3 Period 2 element trends in bonding,
structure, oxidation state, formulae & reactions,
5.1
Period 3 survey of elements,
5.2 Period 3 element trends
& explanations of physical properties, 5.3
Period 3 element trends in bonding, structure, oxidation
state, formulae & reactions, 6.1
Survey of
Period 4 elements, 6.2 Period 4 trends in physical properties, 6.3
Period 4 trends in bonding, formulae and
oxidation state, 6.4 Important element trends down a Group
Advanced
Level Inorganic Chemistry Periodic Table Index:
Part 1
Periodic Table history
Part 2
Electron configurations, spectroscopy,
hydrogen spectrum,
ionisation energies *
Part 3
Period 1 survey H to He *
Part 4
Period 2 survey Li to Ne * Part
5 Period 3 survey Na to Ar *
Part 6
Period 4 survey K to Kr AND important
trends down a group *
Part 7
s–block Groups 1/2 Alkali Metals/Alkaline Earth Metals *
Part 8
p–block Groups 3/13 to 0/18 *
Part 9
Group 7/17 The Halogens *
Part 10
3d block elements & Transition Metal Series
*
Part 11
Group & Series data & periodicity plots All
11 Parts have
their own sub-indexes near the top of the pages
Group numbering and the modern periodic
table
The original group numbers of
the periodic table ran from group 1 alkali metals to group 0
noble gases. To account for the d block elements and their
'vertical' similarities, in the modern periodic table, groups 3
to group 0 are numbered 13 to 18. So, the p block elements are
referred to as groups 13 to group 18 at a higher academic level,
though the group 3 to 0 notation is still
used, but usually at a lower academic level. The 3d block
elements (Sc to Zn) are now considered the head (top) elements
of groups 3 to 12.
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Brown's Chemistry for revising
Advanced Level Inorganic Chemistry Periodic Table
Revision Notes. Website content © Dr
Phil Brown 2000+. All copyrights reserved on Doc Brown's chemistry revision notes, images,
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permitted. Advanced level revision notes on the trends and
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Be(OH)2(s) + 2HCl(aq)
N.