Which metal is more reactive than magnesium? [mr-2]
Gold
Sodium
Iron
Aluminium
Which metal is more reactive than hydrogen but less reactive than carbon? [mr-3]
Gold
Sodium
Iron
Aluminium
Which metal is less reactive than sodium but cannot be extracted using carbon? [mr-4]
Gold
Potassium
Iron
Aluminium
Which is formed when a metal reacts with cold water? [mr-5]
a metal hydroxide
a salt
carbon dioxide
an oxide
Which is a compound formed when a metal reacts with an acid? [mr-6]
a metal hydroxide
a salt
hydrogen
an oxide
Which is formed when a metal reacts with either water or an acid? [mr-7]
a metal hydroxide
a salt
hydrogen
an oxide
Which is formed when a heated metal reacts with steam? [mr-8]
a metal hydroxide
a salt
carbon dioxide
an oxide
Information is given below on the reactivity of four metals Wa, Xb, Yc and Zd (NOT their real chemical symbols) ... Metal Wa does not readily react with dilute acid Metals Xb and Yc react slowly with acid Metal Zd will displace Yc from the
sulfate salt solution of Yc, YcSO4(aq). Metal Zd will NOT displace Xb from the chloride salt solution of Xb, XbCl2(aq). If their reactivity order is from the most reactive (1) (2) (3) (4) to the least reactive ... which metal corresponds to (1), the most reactive of the four metals? [mr-9]
metal Xb
metal Zd
metal Yc
metal Wa
Information is given below on the reactivity of four metals Wa, Xb, Yc and Zd (NOT their real chemical symbols) ... Metal Wa does not readily react with dilute acid Metals Xb and Yc react slowly with acid Metal Zd will displace Yc from the
sulfate salt solution of Yc, YcSO4(aq). Metal Zd will NOT displace Xb from the chloride salt solution of Xb, XbCl2(aq). If their reactivity order is from the most reactive (1) (2) (3) (4) to the least reactive ... which metal corresponds to (2), the 2nd most reactive of the four metals? [mr-10]
metal Xb
metal Zd
metal Yc
metal Wa
Information is given below on the reactivity of four metals Wa, Xb, Yc and Zd (NOT their real chemical symbols) ... Metal Wa does not readily react with dilute acid Metals Xb and Yc react slowly with acid Metal Zd will displace Yc from the
sulfate salt solution of Yc, YcSO4(aq). Metal Zd will NOT displace Xb from the chloride salt solution of Xb, XbCl2(aq). If their reactivity order is from the most reactive (1) (2) (3) (4) to the least reactive ... which metal corresponds to (3), the 3rd most reactive of the four metals? [mr-11]
metal Xb
metal Zd
metal Yc
metal Wa
Information is given below on the reactivity of four metals Wa, Xb, Yc and Zd (NOT their real chemical symbols) ... Metal Wa does not readily react with dilute acid Metals Xb and Yc react slowly with acid Metal Zd will displace Yc from the
sulfate salt solution of Yc, YcSO4(aq). Metal Zd will NOT displace Xb from the chloride salt solution of Xb, XbCl2(aq). If their reactivity order is from the most reactive (1) (2) (3) (4) to the least reactive ... which metal corresponds to (4), the least reactive of the four metals? [mr-12]
metal Xb
metal Zd
metal Yc
metal Wa
From the four elements listed, which is a metal which is most likely to be found in the ground as the metal itself? [mr-13]
copper
hydrogen
iron
magnesium
From the four elements listed, which is a non-metal with no metallic character at all? [mr-14]
copper
hydrogen
iron
magnesium
From the four elements listed, which is a metal that displaces hydrogen from acids but not from cold water? [mr-15]
copper
gold
iron
magnesium
From the four elements listed, which is a metal that cannot be extracted by displacement with carbon? [mr-16]
copper
hydrogen
iron
magnesium
Which is formed by the reaction of heated magnesium with steam? [mr-17]
magnesium oxide + hydrogen
magnesium hydroxide + hydrogen
magnesium chloride + hydrogen
magnesium
sulfate + hydrogen
Which is formed by the reaction of magnesium with cold water? [mr-18]
magnesium oxide + hydrogen
magnesium hydroxide + hydrogen
magnesium chloride + hydrogen
magnesium
sulfate + hydrogen
Which is formed by the reaction of magnesium with hydrochloric acid? [mr-19]
magnesium chloride + water
magnesium hydroxide + hydrogen
magnesium chloride + hydrogen
magnesium
sulfate + chlorine
Which is formed by the reaction of magnesium with
sulfuric acid? [mr-20]
magnesium
sulfate + water
magnesium hydroxide +
sulfur dioxide
magnesium chloride + hydrogen
magnesium
sulfate + hydrogen
Which of A to D is less reactive than copper? [mr-21]
Platinum
Potassium
Zinc
Magnesium
Which is more reactive than magnesium? [mr-22]
Platinum
Potassium
Zinc
Tin
Which is more reactive than hydrogen but less reactive than carbon? [mr-23]
Platinum
Potassium
Zinc
Magnesium
Which is less reactive than sodium but cannot be extracted from its ore using carbon? [mr-24]
Platinum
Potassium
Zinc
Magnesium
Which is found in rocks as the metal itself? [mr-25]
Gold
Carbon
Zinc
Potassium
Which is a non-metal with a little metallic character? [mr-26]
Gold
Carbon
Zinc
Potassium
Which is a metal that displaces hydrogen from dilute acids but not from cold water? [mr-27]
Gold
Carbon
Zinc
Potassium
Which cannot be extracted from its ore with carbon? [mr-28]
Gold
iron
Zinc
Potassium
Which of these in contact with iron will cause rusting? [mr-29]
air and water
boiled saltwater
dry pure oxygen
pure boiled water
A steel pier in the sea rusts. The rust consists of? [mr-30]
iron carbonate
iron oxide
iron chloride
iron
sulfate
Which of these metals can be used in the 'sacrificial corrosion' method for protecting steel structures from rusting? [mr-31]
copper
lead
magnesium
gold
Which of these metals can be used in the 'sacrificial corrosion' method for protecting steel structures from rusting? [mr-32]
Rust readily forms if an iron object is surrounded by? [mr-45]
water with dissolved oxygen
water with no dissolved oxygen
boiled dilute acid
dry air
Which of the following cannot be predicted about metal X, given its position in the reactivity series of metals? [mr-46]
whether X reacts with acid to form hydrogen
whether X acts as a catalyst
the method of extraction of X from an ore
the product of reacting metal X with the
sulfate solution of another metal
Which will displace iron from iron oxide? [mr-47]
tin
copper
magnesium
silver
Road tankers carrying acid use steel tanks lined with glass. The glass is used because? [mr-48]
glass only reacts with alkalis
steel is not strong enough on its own
glass is flexible enough to withstand a crash
acid reacts with steel forming hydrogen
Corrosion occurs when a metal is attacked by? [mr-49]
oxygen
hydrogen
nitrogen
carbon dioxide
When scrap iron is added to blue copper
sulfate solution, a pinky-brown deposit is formed and a pale green solution is left above it. The pinky-brown deposit is? [mr-50]
steel
copper metal
iron
sulfate
rust
When scrap iron is added to blue copper
sulfate solution, a pinky-brown deposit is formed and a pale green solution is left above it. The pale green solution is of? [mr-51]
sulfuric acid
iron oxide
iron
sulfate
copper chloride
When iron becomes coated in rust, the chemical process is an example of? [mr-52]
electrolysis
electroplating
reduction
oxidation
The effect of connecting other metals to an iron nail was investigated. From the observations you can deduce? [mr-57]
iron rusts more quickly when attached to a less reactive metal
iron rusts more quickly when attached to a more reactive metal
iron is less reactive than tin
iron is more reactive than magnesium
The effect of connecting other metals to an iron nail was investigated. From the observations you can deduce? [mr-58]
iron rusts less quickly when attached to a less reactive metal
iron rusts less quickly when attached to a more reactive metal
iron is less reactive than tin
iron is more reactive than magnesium
The effect of connecting other metals to an iron nail was investigated. From the observations you can deduce? [mr-59]
iron rusts less quickly when attached to a less reactive metal
iron rusts more quickly when attached to a more reactive metal
iron is more reactive than tin
iron is more reactive than magnesium
The effect of connecting other metals to an iron nail was investigated. From the observations you can deduce? [mr-60]
iron rusts less quickly when attached to a less reactive metal
iron rusts more quickly when attached to a more reactive metal
iron is less reactive than tin
iron is less reactive than magnesium
The steel hulls of ships can be protected from rusting by bolting on blocks of? [mr-61]
zinc
tin
copper
iron
Steel pipes underground can be protected from rusting by attaching blocks of? [mr-62]
tin
magnesium
copper
iron
Aluminium window frames do not corrode away because the aluminium is? [mr-63]
not reactive enough with oxygen
not reactive enough with water
coated in a layer of aluminium oxide
not capable of forming an oxide
Rust protection from galvanising steel car bodies is done by coating the metal in? [mr-64]
tin
copper
hard wearing paint
zinc
The rusting of iron is described as an oxidation because the iron atoms? [mr-65]
combine with oxygen atoms
gain electrons
combine with water molecules
are so reactive
Which reacts with water to form hydrogen? [mr-66]
zinc
potassium
copper
mercury
Copper can be used for roofing domes on buildings because it? [mr-67]
corrodes very slowly
cannot react with water and oxygen
forms a green carbonate layer on the surface
forms a black oxide layer on the surface
Salt water speeds up the corrosion of metals because it contains ions from salts like sodium chloride. Aluminium can be used for the upper structures of ships because the aluminium? [mr-68]
will not react at all with sea water
will not react with oxygen
is not capable of forming soluble aluminium chloride
is coated in a protective layer of aluminium oxide
In which reaction is a metal oxidised? [mr-69]
magnesium + water (steam) ==> magnesium oxide + hydrogen
carbon + oxygen ==> carbon dioxide
hydrogen + lead oxide ==> lead + water
copper oxide + carbon ==> copper + carbon dioxide
In which reaction is a solid non-metal oxidised? [mr-70]
magnesium + water (steam) ==> magnesium oxide + hydrogen
carbon + water ==> hydrogen + carbon monoxide
hydrogen + lead oxide ==> lead + water
copper oxide + hydrogen ==> copper + water
In which reaction is a gaseous non-metal oxidised? [mr-71]
magnesium + water ==> magnesium hydroxide + hydrogen
carbon + water ==> hydrogen + carbon monoxide
hydrogen + lead oxide ==> lead + water
copper oxide + carbon ==> copper + carbon dioxide
In which reaction is a metal oxide reduced? [mr-72]
magnesium + water ==> magnesium hydroxide + hydrogen
carbon + water ==> hydrogen + carbon monoxide
water (steam) + magnesium ==> magnesium oxide + hydrogen
copper oxide + carbon ==> copper + carbon dioxide
Four chemical changes are shown below as part, or full, word equations. Which can be described as an oxidation only? [mr-73]
carbon ==> carbon monoxide
lead oxide ==> lead
copper oxide + hydrogen ==> copper + water
carbon dioxide ==> carbon monoxide
Four chemical changes are shown below as part, or full, word equations. Which can be described as a reduction only? [mr-74]
carbon ==> carbon monoxide
lead oxide ==> lead
copper oxide + hydrogen ==> copper + water
carbon monoxide ==> carbon dioxide
Four chemical changes are shown below as part, or full, word equations. Which can be described as an oxidation and reduction (redox)? [mr-75]
carbon ==> carbon monoxide
lead oxide ==> lead
copper oxide + hydrogen ==> copper + water
carbon monoxide ==> carbon dioxide
Four chemical changes are shown below as part, or full, word equations. Which can be described as an oxidation and reduction (redox)? [mr-76]
carbon ==> carbon monoxide
lead oxide ==> lead
carbon dioxide ==> carbon monoxide
iron oxide + carbon ==> iron + carbon dioxide
Given the following four observations of the reactions of four metals ... (1) Metals F and G slowly react with water (2) Metal H will displace metal G form its chloride salt solution (3) Metal E will not react with dilute acids (4) Metal H will NOT displace metal F from its
sulfate salt solution What is their reactivity order, from the most to the least reactive? [mr-86]
F > H > G > E
H > E > F > G
E > G > H > F
H > G > F > E
Given the following five observations of the reactions of four metals with hydrogen (H), carbon (C) and other metal oxides ... (1) Metal Y can displace metal Z from its oxide (2) Carbon can displace metal W and metal X from their oxides (3) Hydrogen will displace metal W from its oxide (4) Hydrogen will NOT displace metal X from its oxide (5) Carbon will NOT displace metals Y and Z from their oxides What is their reactivity order, from the most to the least reactive? [mr-87]
(C) > W > X (H) > Y > Z
Y > Z > (C) > X > (H) > W
Z > Y > (C) > W > (H) > X
Y > W > (C) > X > (H) > Z
Underground pipes made of steel (alloy of iron) can be protected from rusting if you attach metal blocks made of a? [mr-88]
chromium alloy
less reactive metal than iron
metal more reactive than iron
a metal of similar reactivity
Stainless steel is made by alloying iron, nickel and ? [mr-89]
copper
aluminium
magnesium
chromium
Roofs of buildings made of copper weather to give a compound ? in colour. [mr-90]
green
orange
black
white
Roofs of buildings made of iron weather to give a compound ? in colour. [mr-91]
green
orange
black
white
When copper is heated in air, the oxide compound formed is ? in colour. [mr-92]
green
orange
black
white
When magnesium burns in air, the oxide compound formed is ? in colour. [mr-93]
green
orange
black
white
Given the following three observations of the reactions of four metals ... (1) Metal O will displace metal N from its chloride (2) Only metal L reacts with cold water (3) Metal N reacts faster with acid than metal M What is their reactivity order, from the most to the least reactive? [mr-94]
L > O > N > M
O > L > N > M
L > N > O > M
M > O > N > L
Given the following ionic redox equation for the displacement of copper from copper(II)
sulfate using zinc metal ... Zn(s) + Cu2+(aq) ==> Zn2+(aq) + Cu(s) In the reaction which is oxidised? [mr-41]
Zn(s)
Cu2+(aq)
Zn2+(aq)
Cu(s)
Given the following ionic redox equation for the displacement of copper from copper(II)
sulfate using zinc metal ... Zn(s) + Cu2+(aq) ==> Zn2+(aq) + Cu(s) In the reaction which is reduced? [mr-42]
Zn(s)
Cu2+(aq)
Zn2+(aq)
Cu(s)
Given the following ionic redox equation for the displacement of copper from copper(II)
sulfate using zinc metal ... Zn(s) + Cu2+(aq) ==> Zn2+(aq) + Cu(s) In the reaction which is formed by an electron loss or oxidation process? [mr-43]
Zn(s)
Cu2+(aq)
Zn2+(aq)
Cu(s)
Given the following ionic redox equation for the displacement of copper from copper(II)
sulfate using zinc metal ... Zn(s) + Cu2+(aq) ==> Zn2+(aq) + Cu(s) In the reaction which is formed by an electron gain or reduction process? [mr-44]
Zn(s)
Cu2+(aq)
Zn2+(aq)
Cu(s)
A simple battery cell can be made by connecting two metal strips dipped into a conducting solution of ions to form a complete circuit. The copper-zinc cell gives a voltage of 1.10 V. What voltage would be produced by a magnesium-iron cell? [mr-53]
1.90 V
2.80 V
2.45 V
2.35 V
A simple battery cell can be made by connecting two metal strips dipped into a conducting solution of ions to form a complete circuit. The copper-zinc cell gives a voltage of 1.10 V. What voltage would be produced by a zinc-silver cell? [mr-54]
0.04 V
1.56 V
1.25 V
0.41 V
A simple battery cell can be made by connecting two metal strips dipped into a conducting solution of ions to form a complete circuit. The copper-zinc cell gives a voltage of 1.10 V. Which combination of metals will give a voltage of 0.79 V? [mr-55]
magnesium-copper
tin-zinc
copper-iron
tin-silver
A simple battery cell can be made by connecting two metal strips dipped into a conducting solution of ions to form a complete circuit. The copper-zinc cell gives a voltage of 1.10 V. Which combination of metals will give a voltage of 0.95 V? [mr-56]
zinc-silver
tin-zinc
copper-iron
tin-silver
Given the following equation: Mg(s) + ? ==> MgCl2(aq) + H2(g) Which of A-D is missing ? [mr-77]
2HCl(aq)
H2Cl2(aq)
HCl(aq)
(HCl)2(aq)
Given the following equation: Ca(s) + 2H2O(l) ==> ? + H2(g) Which of A-D missing ? [mr-78]
CaOH2(aq)
Ca(OH)2(aq)
2CaOH(aq)
Ca2OH(aq)
Given the following equation: Zn(s) + H2SO4(aq) ==> ? + H2(g) Which of A-D is missing ? [mr-79]
2ZnSO4(aq)
Zn2SO4(aq)
ZnSO4(aq)
Zn(SO4)2(aq)
Given the following equation: Mg(s) + ? ==> MgO(s) H2(g) Which of A-D is missing ? [mr-80]
OH(g)
H2O2(g)
OH2(g)
H2O(g)
Given the following equation: Zn(s) + ? ==> ZnSO4(aq) + Fe(s) Which of A-D is missing ? [mr-81]
FeSO4(aq)
Fe2SO4(aq)
Fe(SO4)2(aq)
H2SO4(aq)
Given the following equation: ? + 3Zn(s) ==> 2Fe(s) + 3ZnSO4(aq) Which of A-D is missing ? [mr-82]
2FeSO4(aq)
Fe2(SO4)3(aq)
3FeSO4(aq)
Fe(SO4)3(aq)
Given the following equation: 2Al(s) + 3CuO(s) ==> ? + 3Cu(s) Which of A-D is missing ? [mr-83]
2AlO3(s)
AlO3(s)
Al2O3(s)
Al3O2(s)
Given the following equation: 2K(s) + 2H2O(l) ==> ? + H2(g) Which of A-D is missing ? [mr-84]
KOH(aq)
KOH2(aq)
K2OH(aq)
2KOH(aq)
The rusting of iron is described as an oxidation because the iron atoms? [mr-85]
lose electrons
lose oxygen atoms
combine with water
are not very reactive
Which of the following is a definition of oxidation? [mr-95]
gain of electrons
loss of electrons
gain of hydrogen
loss of oxygen
Which of the following is a definition of reduction? [mr-96]
gain of oxygen
loss of electrons
gain of electrons
loss of hydrogen
Which of the following is a definition of reduction? [mr-97]
gain of oxygen
loss of electrons
loss of hydrogen
loss of oxygen
Galvanising, means 'coating with zinc', and is used to protect iron and steel objects from corrosion. The object can be dipped in a bath of molten zinc! but it is now mainly done by electrolysis. At the positive electrode? [mr-98]
zinc atoms lose electrons and form zinc ions
zinc ions gain electrons and form zinc atoms
zinc atoms gain electrons and form zinc ions
zinc ions lose electrons and form zinc atoms
Galvanising, means 'coating with zinc', and is used to protect iron and steel objects from corrosion. The object can be dipped in a bath of molten zinc! but it is now mainly done by electrolysis. At the negative electrode? [mr-99]
zinc atoms lose electrons and form zinc ions
zinc ions gain electrons and form zinc atoms
zinc atoms gain electrons and form zinc ions
zinc ions lose electrons and form zinc atoms
Galvanising, means 'coating with zinc', and is used to protect iron and steel objects from corrosion. The object can be dipped in a bath of molten zinc! but it is now mainly done by electrolysis. The process at the positive electrode is described as a ...?... reaction. [mr-100]
a displacement
a redox
an oxidation
a reduction
Galvanising, means 'coating with zinc', and is used to protect iron and steel objects from corrosion. The object can be dipped in a bath of molten zinc! but it is now mainly done by electrolysis. The process at the negative electrode is described as ...?... reaction. [mr-101]
a displacement
a redox
an oxidation
a reduction
Galvanising, means 'coating with zinc', and is used to protect iron and steel objects from corrosion. The object can be dipped in a bath of molten zinc! but it is now mainly done by electrolysis. The overall process is described as ...?... reaction. [mr-102]
a redox
a displacement
an oxidation
a reduction
Galvanising means coating an iron (Fe) or steel object with a layer of zinc (Zn) to protect it from corrosion. Steel cans can also be coated with tin (Sn), also to protect it from corrosion, including fruit juices in 'tin' cans. When the zinc coating is scratched through to the iron underneath, the iron still does not corrode
initially. However, if the tin surface is scratched through to the iron, the iron corrodes even faster compared to when there was no coating at. This means? [mr-103]
iron corrodes faster when connected to a more reactive metal
iron corrodes faster when connected to a less reactive metal
tin is more reactive than iron
zinc is less reactive than iron
Galvanising means coating an iron (Fe) or steel object with a layer of zinc (Zn) to protect it from corrosion. Steel cans can also be coated with tin (Sn), also to protect it from corrosion, including fruit juices in 'tin' cans. When the zinc coating is scratched through to the iron underneath, the iron still does not corrode
initially. However, if the tin surface is scratched through to the iron, the iron corrodes even faster compared to when there was no coating at. This means? [mr-104]
iron corrodes faster when connected to a more reactive metal
iron corrodes slower when connected to a less reactive metal
tin is less reactive than iron
zinc is less reactive than iron
Galvanising means coating an iron (Fe) or steel object with a layer of zinc (Zn) to protect it from corrosion. Steel cans can also be coated with tin (Sn), also to protect it from corrosion, including fruit juices in 'tin' cans. When the zinc coating is scratched through to the iron underneath, the iron still does not corrode
initially. However, if the tin surface is scratched through to the iron, the iron corrodes even faster compared to when there was no coating at. This means? [mr-105]
iron corrodes faster when connected to a more reactive metal
iron corrodes slower when connected to a less reactive metal
tin is less reactive than iron
zinc is less reactive than iron
Galvanising means coating an iron (Fe) or steel object with a layer of zinc (Zn) to protect it from corrosion. Steel cans can also be coated with tin (Sn), also to protect it from corrosion, including fruit juices in 'tin' cans. When the zinc coating is scratched through to the iron underneath, the iron still does not corrode
initially. However, if the tin surface is scratched through to the iron, the iron corrodes even faster compared to when there was no coating at. This means? [mr-106]
iron corrodes faster when connected to a more reactive metal
iron corrodes slower when connected to a less reactive metal
tin is more reactive than iron
zinc is more reactive than iron
Galvanising means coating an iron (Fe) or steel object with a layer of zinc (Zn) to protect it from corrosion. Steel cans can also be coated with tin (Sn), also to protect it from corrosion, including fruit juices in 'tin' cans. When the zinc coating is scratched through to the iron underneath, the iron still does not corrode
initially. However, if the tin surface is scratched through to the iron, the iron corrodes even faster compared to when there was no coating at. This means? [mr-107]
iron corrodes slower when connected to a more reactive metal
iron corrodes slower when connected to a less reactive metal
tin is more reactive than iron
zinc is less reactive than iron
A simple battery cell can be made by connecting two metal strips dipped into a conducting solution of ions to form a complete circuit. Some of the first 'batteries' were made from dipping strips of zinc and copper into their salt solutions, but even a solution of acid works too. The electrode potential (V) is a measure of how easily a metal loses electrons. The more negative the potential the more easily the metal atoms lose electrons. The potential difference of the cell (p.d. in Volts) is the difference between the two electrode potentials of the two metals (shown in the table compared to hydrogen). What voltage does this cell produce if copper and zinc electrodes are used? [mr-108]
0.42 V
1.10 V
0.76 V
0.34 V
A simple battery cell can be made by connecting two metal strips dipped into a conducting solution of ions to form a complete circuit. Some of the first 'batteries' were made from dipping strips of zinc and copper into their salt solutions, but even a solution of acid works too. The electrode potential (V) is a measure of how easily a metal loses electrons. The more negative the potential the more easily the metal atoms lose electrons. The potential difference of the cell (p.d. in Volts) is the difference between the two electrode potentials of the two metals (shown in the table compared to hydrogen). Which two metals will give a cell voltage of 1.25V? [mr-109]
copper and magnesium
zinc and iron
silver and iron
tin and zinc
A simple battery cell can be made by connecting two metal strips dipped into a conducting solution of ions to form a complete circuit. Some of the first 'batteries' were made from dipping strips of zinc and copper into their salt solutions, but even a solution of acid works too. The electrode potential (V) is a measure of how easily a metal loses electrons. The more negative the potential the more easily the metal atoms lose electrons. The potential difference of the cell (p.d. in Volts) is the difference between the two electrode potentials of the two metals (shown in the table compared to hydrogen). Which two metals will give a cell voltage of 0.65V? [mr-110]
copper and magnesium
zinc and iron
silver and iron
tin and zinc
A simple battery cell can be made by connecting two metal strips dipped into a conducting solution of ions to form a complete circuit. Some of the first 'batteries' were made from dipping strips of zinc and copper into their salt solutions, but even a solution of acid works too. The electrode potential (V) is a measure of how easily a metal loses electrons. The more negative the potential the more easily the metal atoms lose electrons. The potential difference of the cell (p.d. in Volts) is the difference between the two electrode potentials of the two metals (shown in the table compared to hydrogen). Which statement is TRUE if copper and zinc metal electrodes are used? [mr-111]
Zn(s) ==> Zn2+(aq) + 2e- occurs on the zinc plate
copper will deposit on the copper plate
Cu(s) ==> Cu2+(aq) + 2e- occurs on the copper plate
the zinc plate will turn red-brown in colour
A simple battery cell can be made by connecting two metal strips dipped into a conducting solution of ions to form a complete circuit. Some of the first 'batteries' were made from dipping strips of zinc and copper into their salt solutions, but even a solution of acid works too. The electrode potential (V) is a measure of how easily a metal loses electrons. The more negative the potential the more easily the metal atoms lose electrons. The potential difference of the cell (p.d. in Volts) is the difference between the two electrode potentials of the two metals (shown in the table compared to hydrogen). Which statement is TRUE if copper and zinc metal electrodes are used? [mr-112]
Zn2+(aq) + 2e- ==> Zn(s) occurs on the zinc plate
the zinc
electrode slowly dissolves
Cu(s) ==> Cu2+(aq) + 2e- occurs on the copper plate
the zinc electrode plate will turn red-brown in colour
The diagram shows the results of some sacrificial rust protection experiments. When silver is connected to iron, electrons transfer from iron to silver. This causes? [mr-113]
iron ions to change to iron atoms
silver atoms to change to silver ions
iron atoms to change to iron ions
silver ions to change to silver atoms
The diagram shows the results of some sacrificial rust protection experiments. When zinc is connected to iron, electrons transfer from zinc to iron. This causes? [mr-114]
iron ions to change to iron atoms
zinc ions to change to zinc atoms
iron atoms to change to iron ions
zinc atoms to change to zinc ions
If an iron sheet is dipped into a silver nitrate solution it becomes coated in grey layer of silver. The overall reaction is an example of? [mr-115]
displacement
reduction only
electrolysis
neutralisation
If an iron sheet is dipped into a copper
sulfate solution it becomes coated in pink-brown deposit of copper. This formation of the copper is an example of? [mr-116]
oxidation only
reduction only
electrolysis
neutralisation
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exam practice questions on the reactivity series of metals
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questions on the reactivity series of metals in a GCSE
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exam practice questions on the reactivity series of metals, useful for US grade 9-10 chemistry courses
Which metal is less reactive than copper? [mr-1]
Which is formed when a metal reacts with cold water? [mr-5]
Which is formed when a heated metal reacts with steam? [mr-8]
Which of these in contact with iron will cause rusting? [mr-29]
The effect of connecting other metals to an iron nail was investigated. From the observations you can deduce? [mr-57]
Aluminium window frames do not corrode away because the aluminium is? [mr-63]
Copper can be used for roofing domes on buildings because it? [mr-67]
Roofs of buildings made of iron weather to give a compound ? in colour. [mr-91]
A simple battery cell can be made by connecting two metal strips dipped into a conducting solution of ions to form a complete circuit. The copper-zinc cell gives a voltage of 1.10 V. What voltage would be produced by a magnesium-iron cell? [mr-53]
Galvanising, means 'coating with zinc', and is used to protect iron and steel objects from corrosion. The object can be dipped in a bath of molten zinc! but it is now mainly done by electrolysis. At the positive electrode? [mr-98]
Galvanising means coating an iron (Fe) or steel object with a layer of zinc (Zn) to protect it from corrosion. Steel cans can also be coated with tin (Sn), also to protect it from corrosion, including fruit juices in 'tin' cans. When the zinc coating is scratched through to the iron underneath, the iron still does not corrode
initially. However, if the tin surface is scratched through to the iron, the iron corrodes even faster compared to when there was no coating at. This means? [mr-103]
The diagram shows the results of some sacrificial rust protection experiments. When silver is connected to iron, electrons transfer from iron to silver. This causes? [mr-113]