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GCSE Questions
and Answers
Atomic Structure
and Bonding
6 consecutive CCEA GCSE Chemistry papers: 2002-7
1
From our “Learning Outcomes”
I
II
1
H
1
2
Li
2.1
Be
2.2
3
Na
2.8.1
Mg
2.8.2
4
K
Ca
2.8.8. 2.8.8.2
1
III
IV
V
VI
VII VII
I
He
2
B
2.3
C
2.4
N
2.5
O
2.6
F
2.7
Ne
2.8
Al
Si
P
S
Cl
Ar
2.8.3 2.8.4 2.8.5 2.8.6 2.8.7 2.8.8
2
2002, Paper 2
1a) Magnesium is an element. It has an
atomic number of 12 and the main
isotope of magnesium has a mass
number of 24.
(i) Define the term “atomic number”
_____________________________
__________________________ [1]
1a) Magnesium is an element. It has an
atomic number of 12 and the main
isotope of magnesium has a mass
number of 24.
(i) Define the term “atomic number”
Number of protons (in the nucleus)
[1]
(ii) What are isotopes?
_____________________________
___________________________[2]
(iii) How many neutrons are present in
the nucleus of an atom of
magnesium?
___________________________[1]
(ii) What are isotopes?
Atoms of the same element/same
atomic number of protons [1] with
different mass numbers/different
numbers of neutrons [1]
(iii) How many neutrons are present in
the nucleus of an atom of
magnesium?
12
[1]
b)
Magnesium and hydrogen both react
vigorously with the oxygen in air;
magnesium produces magnesium oxide and
hydrogen produces water.
(i)
Show the bonding present in a molecule of
oxygen gas and in a molecule of water by
means of a diagram. (Outer shell
electrons).
Oxygen [3]
Water [4]
(i)
Show the bonding present in a molecule of
oxygen gas and in a molecule of water by
means of a diagram. (Outer shell
electrons).
Oxygen: In the molecule – 4e- shared [1]
outer shells correct [1] 2 O atoms [1]
Water: outer shell of H correct [1] outer
shell of O correct [1] 2e- in each bond [1]
2 H atoms and 1 O atom [1]
(ii)
Using full electronic arrangements explain
how atoms of magnesium combine with atoms of
oxygen to form magnesium oxide. (charges on
the particles should be given.)
_______________________________________
_____________________________________ [6]
(iii) What type of bonding is present in magnesium
oxide?
_____________________________________ [1]
11
I
II
1
H
1
2
Li
2.1
Be
2.2
3
Na
2.8.1
Mg
2.8.2
4
K
Ca
2.8.8. 2.8.8.2
1
III
IV
V
VI
VII VII
I
He
2
B
2.3
C
2.4
N
2.5
O
2.6
F
2.7
Ne
2.8
Al
Si
P
S
Cl
Ar
2.8.3 2.8.4 2.8.5 2.8.6 2.8.7 2.8.8
12
(ii)
Using full electronic arrangements explain
how atoms of magnesium combine with atoms of
oxygen to form magnesium oxide. (charges on
the particles should be given.)
Mg O
→ Mg2+ [1] O2- [1]
2, 8, 2 [1] 2, 6 [1]
2, 8 [1]
2, 8 [1]
(iii) What type of bonding is present in magnesium
oxide?
Ionic / electrovalent [1]
From our “Learning Outcomes”
14
c)
Magnesium has a melting point of 649◦C and it is
malleable. The melting point of magnesium
oxide is 2800◦C.
(i)
Explain clearly why magnesium is malleable.
_______________________________________
_____________________________________ [3]
c)
Magnesium has a melting point of 649◦C and it is
malleable. The melting point of magnesium
oxide is 2800◦C.
(i)
Explain clearly why magnesium is malleable.
Layers [1] of ions slides over each other [1] idea
of no disruption to structure / sea of electrons
hold structure together [1]
(ii)
Explain fully why magnesium oxide has a very
high melting point.
_____________________________________
_____________________________________ [3]
d)
The reaction between hydrogen andoxygen is
exothermic.
(i)
Explain why it is necessary to heat the
hydrogen/oxygen mixture for the reaction to
start.
_______________________________________
_____________________________________ [2]
(ii)
Explain fully why magnesium oxide has a very
high melting point.
Strong bonds [1] large amount of energy / heat
[1] required to break [1] bonds.
d)
The reaction between hydrogen andoxygen is
exothermic.
(i)
Explain why it is necessary to heat the
hydrogen/oxygen mixture for the reaction to
start.
Break bonds [1] in reactants [1]
(ii)
Explain, in terms of bonds, why the reaction
between hydrogen and oxygen is exothermic.
______________________________________
___________________________________ [4]
(ii) Explain, in terms of bonds, why the reaction between
hydrogen and oxygen is exothermic.
More energy [1] is released [1] when the bonds are
made [1] in water than when the bonds are broken [1]
in the hydrogen and oxygen.
2003, Paper 1
1
At the start of the twentieth
century the structure of the atom
was largely unknown.
Experimental work carried out
over a number of years helped
scientists to develop different
models of atom.
a)
Complete the paragraph below by filling in the
missing words.
In 1897 Thomson proposed the plum-pudding
model of the atom. He suggested that the
protons and electrons were all mixed together in
an atom with the ___________ embedded in a
positive sphere. This model was disproved by
Rutherford who proposed that an atom consisted
of a small nucleus surrounded by __________.
The neutron was discovered by ___________ in
1932 and it was then thought the nucleus
contained ___________ and ___________. [5]
a)
Complete the paragraph below by filling in the
missing words.
In 1897 Thomson proposed the plum-pudding
model of the atom. He suggested that the
protons and electrons were all mixed together in
an atom with the electrons embedded in a
positive sphere. This model was disproved by
Rutherford who proposed that an atom consisted
of a small nucleus surrounded by electrons. The
neutron was discovered by Chadwick in 1932
and it was then thought the nucleus contained
protons and neutrons. [5]
b)
It is now known that most atoms contain
protons, electrons and neutrons.
Complete the table below to show the
relative mass and charge of each particle.
[3]
Particle Relative Mass Relative Charge
Proton
Electron
Neutron
b)
It is now known that most atoms contain protons,
electrons and neutrons. Complete the table
below to show the relative mass and charge of
each particle. [3]
Particle Relative Mass
Proton
1
1
Electron
1840
Accept a range
1
1800
Neutron
Relative Charge
+1
-1
1
2000
Or approximately zero
Do not accept zero
1
0
c)
All atoms have a mass number and
an atomic number. Calcium has a
mass number of 40 and an atomic
number of 20.
(i) What is meant by the term “mass
number”?
_____________________________
__________________________ [1]
c)
All atoms have a mass number and
an atomic number. Calcium has a
mass number of 40 and an atomic
number of 20.
(i) What is meant by the term “mass
number”?
Number of protons plus neutrons [1]
ii) Draw a labelled diagram of an atom
of calcium showing the position and
number of the proton, neutrons and
electrons.
[4]
ii) Draw a labelled diagram of an atom
of calcium showing the position and
number of the proton, neutrons and
electrons.
[4]
2, 8, 8, 2 [1]
20 p+ [1]
20 nO [1]
protons + neutrons
in nucleus [1]
iii) Explain why an atom of calcium is
electrically neutral.
_____________________________
__________________________ [2]
iii) Explain why an atom of calcium is
electrically neutral.
There are equal [1] numbers of
protons and electrons [1]
d) Calcium, on heating, burns in
oxygen gas to produce a white
powder called calcium oxide.
(i) State the type of bonding found in:
calcium ____________________ [1]
oxygen ____________________ [1]
calcium oxide _______________ [1]
d) Calcium, on heating, burns in
oxygen gas to produce a white
powder called calcium oxide.
(i) State the type of bonding found in:
calcium metallic
oxygen covalent
calcium oxide ionic
[1]
[1]
[1]
(ii) Explain, using full electronic
structures, how calcium and oxygen
bond to produce calcium oxide. You
may use a diagram to help you.
______________________________
______________________________
___________________________ [5]
(ii)
Explain, using full electronic structures, how
calcium and oxygen bond to produce calcium
oxide. You may use a diagram to help you.
Ions held together by electrostatic forces [1]
Or alternatively;
e)
Graphite, like calcium oxide, has a
high melting point yet its structure is
very different from calcium oxide.
Describe the bonding in graphite.
_____________________________
_____________________________
__________________________ [3]
From our “Learning Outcomes”
Layered structure
Each carbon strongly (covalently) bonded to three
others in the same layer
Each carbon additionally “weakly bonded” to a
carbon in both the sheets above & below
37
e)
Graphite, like calcium oxide, has a high melting
point yet its structure is very different from
calcium oxide. Describe the bonding in graphite.
Layered structure [1] each carbon covalently
bonded [1] to three [1] other carbon atoms weak
forces between the layers [1] Max [3] / [4].
For a diagram only the marks
can be awarded for two or more
layers [1] two or more
hexagons [1] labelled weak
bonds drawn between the
layers
[1]
2003, Paper 2
3
Many scientists contributed to the
development of the Periodic Table of
the elements.
a)
Define what is meant by the term
“element”.
_____________________________
___________________________ [2]
3
Many scientists contributed to the
development of the Periodic Table of
the elements.
a)
Define what is meant by the term
“element”.
A (pure) substance which cannot be
broken down [1] by chemical means
[1] or contains only one type [1] of
atom [1]
The following list shows a selection of elements from
the Periodic Table.
Aluminium
Neon
Silicon
Chlorine
Oxygen
Sodium
Magnesium
Phosphorus
sulphur
Each element may be used once, more than once or not
at all.
b) From the elements list choose:
(i) two elements in the same Group of
the Periodic Table.
__________ and __________ [2]
(ii) three metallic elements
__________, __________ and
__________ [3]
b) From the elements list choose:
(i) two elements in the same Group of
the Periodic Table.
Oxygen [1] and Sulphur [1]
(ii) three metallic elements
Magnesium [1], Sodium [1] and
Aluminium [1]
(iii) an element with seven electrons in
the outer shell
__________________________ [1]
(iv) a semi-metal and give a reason why
it can be classified in this way.
Element ______________________
Reason _______________________
__________________________ [2]
(iii) an element with seven electrons in
the outer shell
Chlorine
[1]
(iv) a semi-metal and give a reason why
it can be classified in this way.
Element Silicon [1]
Reason It has properties of both
metals and non-metals, e.g. it
conducts electricity [1]
46
c)
Element X reacts vigorously with
cold water to produce a compound
with formula XOH and hydrogen
gas. In which Group of the Periodic
Table is element X found?
__________________________ [1]
c)
Element X reacts vigorously with
cold water to produce a compound
with formula XOH and hydrogen
gas. In which Group of the Periodic
Table is element X found?
Group I / Group l / alkali metals [1]
d)
Atoms are extremely small. The
radius of a hydrogen atom is
approximately 0.000 000 000 1 m.
Atoms of different elements are of
different sizes.
(i) how does the atomic size change on
going down Group II?
___________________________ [1]
d)
Atoms are extremely small. The
radius of a hydrogen atom is
approximately 0.000 000 000 1 m.
Atoms of different elements are of
different sizes.
(i) how does the atomic size change on
going down Group II?
It increases
[1]
(ii) How does the atomic size change on
moving across Period 3 from sodium
to chlorine?
___________________________ [1]
(ii) How does the atomic size change on
moving across Period 3 from sodium
to chlorine?
It decreases
[1]
e)(i)Barium is a typical Group II
element. Complete the table below
to show the formulae of the
compounds named. [3]
Name of Compound Formula of Compound
Barium oxide
Barium chloride
Barium sulphate
e)(i)Barium is a typical Group II
element. Complete the table below
to show the formulae of the
compounds named. [3]
Name of Compound
Barium oxide
Barium chloride
Barium sulphate
Formula of Compound
BaO
BaCl2
BaSO4
(ii) Using your knowledge of the
Periodic Table, predict whether
barium will react more vigorously
or less vigorously than calcium.
Explain your answer.
_____________________________
_____________________________
__________________________ [2]
(ii) Using your knowledge of the
Periodic Table, predict whether
barium will react more vigorously
or less vigorously than calcium.
Explain your answer.
Barium will react more vigorously
[1] (than calcium). Barium is below
Ca in Group II/the reactivity
increases as the group is descended
[1]
(iii) Write a balanced, symbol equation
to show how barium reacts with
cold water.
__________________________ [2]
I
II III IV
V
VI VII
H+
Li+ Be2+
Na+ Mg2+ Al3+
F
3
N
2
O
Cl
58
(iii) Write a balanced, symbol equation
to show how barium reacts with
cold water.
Ba + 2H2O → Ba(OH)2 + H2 [2]
2004, Paper 2
4
Atoms contain different number of
protons, neutrons and electrons.
a)(i) Name the particle which has a positive
charge.
_______________________________ [1]
(ii) Name the particle which has the smallest
mass.
_______________________________ [1]
4
Atoms contain different number of
protons, neutrons and electrons.
a)(i) Name the particle which has a positive
charge.
Proton
[1]
(ii) Name the particle which has the smallest
mass.
Electron
[1]
(iii) Which of these particles are found in the
nucleus?
______________________________ [2]
(iii) Which of these particles are found in the
nucleus?
Protons [1] neutrons [1]
[2]
b)
(i)
35
17
37
17
Cl and Cl are isotopes of chlorine.
Explain what you understand by the term
isotope.
_______________________________
_______________________________ [2]
b)
35
17
37
Cl and17
Cl are isotopes of chlorine.
(i)
Explain what you understand by the term
isotope.
Atoms of the same element/with the same
number of protons/atomic number [1] but
a different number of neutrons/mass
number [1]
[2]
(ii) Complete the following table to give the
number of each of the particles for the two
isotopes of chlorine.
Particle Name
Proton
Neutron
Electron
35
17
Cl
37
Cl
17
(ii) Complete the following table to give the
number of each of the particles for the two
isotopes of chlorine.
Particle Name
35
17
Proton
Neutron
Electron
17[1]
18[1]
17[1]
Cl
37
Cl
17
17[1]
20[1]
17[1]
c)
The compound calcium chloride can be
made from the reaction between calcium
atoms and chlorine atoms.
(i)
Show, using a diagram, the electronic
configuration of a calcium atom.
[2]
c)
The compound calcium chloride can be
made from the reaction between calcium
atoms and chlorine atoms.
(i)
Show, using a diagram, the electronic
configuration of a calcium atom.
[2]
(ii) Explain why a calcium atom is electrically
neutral.
_______________________________
_______________________________ [2]
(iii) Show using a diagram, the electronic
configuration of a calcium ion and give its charge.
(ii) Explain why a calcium atom is electrically
neutral.
_______________________________
_______________________________ [2]
(iii) Show using a diagram, the electronic
configuration of a calcium ion and give its charge.
(iv) Give the formula of calcium chloride.
_______________________________ [1]
(v) Would you expect calcium chloride to be a
solid, liquid or gas at room temperature?
Explain your answer.
_______________________________
_______________________________
_______________________________ [3]
(iv) Give the formula of calcium chloride.
CaCl2
[1]
(v) Would you expect calcium chloride to be a
solid, liquid or gas at room temperature?
Explain your answer.
Solid [1] (the ions are held together by)
strong [1] electrostatic forces [1]
[3]
d)(i) Complete the following table for methane
and oxygen.
Oxygen
Molecular
Dot and cross diagram
Type of Bonding
Physical state at room
temperature
O2
Methane
d)(i) Complete the following table for methane
and oxygen.
Molecular
Oxygen
Methane
O2
CH4 [1]
[1]
Covalent [1]
Covalent [1]
Dot and cross diagram
Type of Bonding
Physical state at room
temperature
(ii) Explain fully why both oxygen and
methane have low melting points.
_______________________________
_______________________________
_______________________________ [4]
(ii) Explain fully why both oxygen and
methane have low melting points.
Little/low energy/heat required to break
[1] weak intermolecular forces/weak
bonds [1] between molecules [1]
[4]
2005, Paper 2
1a) An atom of the element sodium may be
23
written as 11 Na where 23 is the mass
number and 11 is the atomic number.
(i)
What is meant by the term element?
_______________________________
_______________________________ [2]
(ii) Explain fully what is meant by the term
atomic number.
_______________________________ [1]
1a)
An atom of the element sodium may be written as
23
Na where 23 is the mass number and 11 is the
11
atomic number.
(i)
What is meant by the term element?
Substance containing only one type [1] of atom
[1] (or cannot be broken down into anything
simpler [1] by chemical means [1])
[2]
(ii)
Explain fully what is meant by the term atomic
number.
Number of protons
[1]
(iii) Complete the table below giving the
number of protons, neutrons and electrons
present in an atom of Na and give the
arrangement of the electrons.
[4]
23
11 Na
Number of Protons
Number of Neutrons
Number of Electrons
Electron arrangement
(iii) Complete the table below giving the
number of protons, neutrons and electrons
present in an atom of Na and give the
arrangement of the electrons.
[4]
23
11 Na
Number of Protons
Number of Neutrons
Number of Electrons
Electron arrangement
11 [1]
12 [1]
11 [1]
2, 8, 1 [1]
(iv) Explain what happens to an atom of
sodium when it forms an ion. You may
use an ionic equation to answer this
question.
_______________________________
_______________________________
_______________________________ [3]
(iv) Explain what happens to an atom of
sodium when it forms an ion. You may
use an ionic equation to answer this
question.
Na → Na+ + e- or loses [1] electron [1] to
form Na+ [1]
[3]
b)
The table below gives details of the electronic
arrangement of four ions formed from elements
represented by the letters A, B, C and D. The
letters do not represent the symbols for elements.
Element Ion Formed Electronic Arrangement
A
A2, 8
B
B2+
2, 8
C
C22, 8
D
D3+
2, 8
(i)
Element
Ion Formed
Electronic Arrangement
A
B
C
D
AB2+
C2D3+
2, 8
2, 8
2, 8
2, 8
Using your knowledge of the Periodic
Table, identify the elements represented by
the letters:
A _____________________________ [1]
B _____________________________ [1]
C _____________________________ [1]
D _____________________________ [1]
(i)
Using your knowledge of the Periodic
Table, identify the elements represented by
the letters:
A F/Fluorine
B Mg/Magnesium
C O/Oxygen
D Al/Aluminium
[1]
[1]
[1]
[1]
B2+ and A- form a compound in which the
bonding is described as ionic.
(ii) What is the formula of the compound
formed between these two ions?
_______________________________ [1]
(iii) Explain fully what is meant by the ionic
bond.
_______________________________
_______________________________
_______________________________ [3]
B2+ and A- form a compound in which the
bonding is described as ionic.
(ii) What is the formula of the compound
formed between these two ions?
BA2 or MgF2
[1]
(iii) Explain fully what is meant by the ionic
bond.
Attraction [1] of oppositely [1] charged [1]
ions or ions are held together by
electrostatic [2] forces [1]
[3]
89
c)
Carbon and silicon are elements in group
IV of the Periodic Table. They have
similar properties and form compounds
with similar formulae.
Methane and silane are compounds of the
group IV elements with hydrogen.
(i)
Suggest a formula for silane.
_______________________________ [1]
c)
Carbon and silicon are elements in group
IV of the Periodic Table. They have
similar properties and form compounds
with similar formulae.
Methane and silane are compounds of the
group IV elements with hydrogen.
(i)
Suggest a formula for silane.
SiH4
[1]
(ii) Draw a diagram to show how atoms of
carbon and hydrogen bond to form a
molecule of methane. Only outer shell
electrons need to be shown.
[4]
(ii) Draw a diagram to show how atoms of
carbon and hydrogen bond to form a
molecule of methane. Only outer shell
electrons need to be shown.
[4]
1 C and 4 H atoms [1]
4 electrons in outer shell of C atom [1]
1 electron in outer shell of each H atom [1]
2 electrons in each bond [1]
d)
Carbon and silicon both form dioxides: carbon
dioxide and silicon dioxide. Carbon dioxide is a
gas and silicon dioxide forms quartz crystals
which have a melting point of 1610°C.
(i)
Complete the table to give the type of bonding
and structure in carbon dioxide and quartz.
Substance
Type of Bonding Structure
Carbon Dioxide
Quartz
d)
Carbon and silicon both form dioxides: carbon
dioxide and silicon dioxide. Carbon dioxide is a
gas and silicon dioxide forms quartz crystals
which have a melting point of 1610°C.
(i)
Complete the table to give the type of bonding
and structure in carbon dioxide and quartz.
Substance
Type of Bonding Structure
Carbon Dioxide Covalent [1]
Molecular [1]
Quartz
Covalent [1]
Giant [1]
(ii) Describe the structure of quartz.
_______________________________
_______________________________ [2]
(iii) Describe fully why quartz has a high
melting point.
_______________________________
_______________________________
_______________________________ [3]
Silica (SiO2)
There is a
repeating
unit in this
structure:
97
(ii) Describe the structure of quartz.
Each silicon atom bonded to 4 oxygen
atoms [1] each oxygen atom bonded to 2
silicon atoms [1] (Max [2])
[2]
(iii) Describe fully why quartz has a high
melting point.
Large amount of energy [1] needed to
break [1] strong bonds [1]
[3]
2006, Paper 1
5a) The table gives some information about
the elements calcium and oxygen.
(i) Complete the table below
Electronic
Element Atomic Arrangement
number
Atom
Ion
Calcium
Oxygen 8
Symbol
Atom
Ion
Ca2+
2, 8, 8, 2
2, 8
5a) The table gives some information about
the elements calcium and oxygen.
(i) Complete the table below
Electronic
Element Atomic Arrangement
number
Atom
Ion
Calcium 20 [1]
Oxygen 8
2, 8, 8, 2 2, 8, 8 [1]
2, 6 [1]
2, 8
Symbol
Atom
Ion
Ca [1]
O [1]
Ca2+
O2- [1]
(ii) Calcium atoms react with non-metal atoms
like oxygen to form calcium ions. Explain
in terms of electrons, what happens when
atoms of calcium form calcium ions.
_______________________________
_______________________________ [3]
Quality of written communication
[2]
(ii) Calcium atoms react with non-metal atoms
like oxygen to form calcium ions. Explain
in terms of electrons, what happens when
atoms of calcium form calcium ions.
2 [1] electrons [1] lost / transferred [1] [3]
Quality of written communication
[2]
(iii) Oxygen has two isotopes. Explain what is
meant by the term isotope.
_______________________________ [2]
(iii) Oxygen has two isotopes. Explain what is
meant by the term isotope.
Same element / same atomic number /
same number of protons [1]. Different
mass number / different number of
neutrons [1]
[2]
(iv) Atoms of oxygen, like most atoms, contain
protons, neutrons and electrons. Complete
the table below for each type of particle.
Particle
Relative
Charge
Relative
Mass
Number in
one atom of
16
8
Electron
Neutron
Proton
O
(iv) Atoms of oxygen, like most atoms, contain
protons, neutrons and electrons. Complete the
table below for each type of particle.
Particle
Relative
Charge
Relative Mass Number in
one atom of
16
8
Accept
8
O
Electron
-1
 1 


 1840 
 1 
 1 





 1800 
 2000 
Neutron
0
Or almost 0
1
Proton
+1
1
8
8
v)
The bonding in calcium is metallic.
Explain what is meant by metallic
bonding. You may use a labelled diagram
to help answer this question.
_______________________________
_______________________________
_______________________________ [3]
v)
The bonding in calcium is metallic.
Explain what is meant by metallic
bonding. You may use a labelled diagram
to help answer this question.
Regular / layers / attraction of [1] of
positive centres / ions [1] sea of
delocalised electrons [1]
[3]
(vi) Explain why metals like calcium are
malleable.
_______________________________
_______________________________
_______________________________
_______________________________ [3]
(vi) Explain why metals like calcium are
malleable.
Layers [1] slide over each other [1] idea of
without disrupting structure / electrons
hold structure together [1]
[3]
b)
The diagram below shows an atom of an
element X, where:
e represents an electron;
n represents a neutron; and
p represents a proton
(i)
Name the element X.
_______________________________ [1]
(ii) State the Group to which element X
belongs.
_______________________________ [1]
(i)
Name the element X.
Boron
[1]
(ii) State the Group to which element X
belongs.
Group III
[1]
(iii) What is the mass number of this atom of
element X?
_______________________________ [1]
(iv) Name the part of the atom which is shaded
grey.
_______________________________ [1]
(iii) What is the mass number of this atom of
element X?
11
[1]
(iv) Name the part of the atom which is shaded
grey.
Nucleus
[1]
2007, Paper 1
1a) The element chlorine exists as diatomic
molecules. The diagram below represents
the bonding in a chlorine molecule.
(i)
Explain why chlorine exists as diatomic
molecules rather than as chlorine atoms.
_______________________________
_______________________________ [1]
(ii) Name the type of bonding found in a
chlorine molecule.
_______________________________ [1]
(i)
Explain why chlorine exists as diatomic
molecules rather than as chlorine atoms.
To become stable/to gain a full outer shell
(of electrons)
[1]
(ii) Name the type of bonding found in a
chlorine molecule.
Covalent
[1]
(iii) Explain as fully as possible how the two
chlorine atoms bond together.
_______________________________
_______________________________ [2]
(iii) Explain as fully as possible how the two
chlorine atoms bond together.
Idea of pair [1] of shared electrons [1] [2]
b)
The element chlorine reacts with metals
like sodium and calcium to form metal
chlorides.
(i)
Write the formula of sodium chloride
_______________________________ [1]
b)
The element chlorine reacts with metals
like sodium and calcium to form metal
chlorides.
(i)
Write the formula of sodium chloride
NaCl
[1]
Sodium ion Na+
Chloride ion Cl
123
(ii) Explain in detail how atoms of calcium
combine with atoms of chlorine to form
calcium chloride. You must use a diagram
in your answer.
_______________________________
_______________________________
_______________________________ [6]
(ii)
Explain in detail how atoms of calcium combine
with atoms of chlorine to form calcium chloride.
You must use a diagram in your answer.
[6]
In diagram outer electrons can be paired.
Attraction of oppositely charged ions/electrostatic
attraction [1]
(iii) What type of bonding is found in calcium
chloride?
_______________________________ [1]
(iii) What type of bonding is found in calcium
chloride?
Ionic
[1]
c)
The physical properties of a substance
depend on its bonding and structure. For
each of the following substances, describe
the structure and state two physical
properties of the substance.
(i)
Methane, CH4
Structure: _______________________ [1]
Physical Properties:
1. _____________________________ [1]
2. _____________________________ [1]
(i)
Methane, CH4
Structure: Molecular / simple covalent /
simple molecular
[1]
Physical Properties:
Low melting / boiling point / gas [1], Nonconductor [1], low density [1],
compressible [1]. Any other appropriate
physical property. Max [2]
(ii) Diamond
Structure: _______________________ [1]
Physical Properties:
1. _____________________________ [1]
2. _____________________________ [1]
Diamond:
Each carbon atom is
covalently bonded to 4
others
The repeating unit is a
tetrahedron composed of
5 carbons
 Diamond has a giant
structure
132
(ii) Diamond
Structure: Giant molecular /
Macromolecular / Giant covalent
[1]
Physical Properties:
High melting/boiling point/solid [1], nonconductor [1], insoluble in water [1],
Crystalline [1], Hard [1]. Any other
appropriate physical property. Max [2]
(iii) Sodium Oxide, Na2O
Structure: _______________________ [1]
Physical Properties:
1. _____________________________ [1]
2. _____________________________ [1]
(iii) Sodium Oxide, Na2O
Structure: Ionic (lattice
[1]
Physical Properties:
High melting/boiling point/solid [1] brittle
[1], conducts (electricity) when
molten/aqueous [1], soluble (in water) [1],
easy to cleave [1]. Any other appropriate
physical property. Max [2]
d)
Describe the bonding and structure in a
typical metal like sodium. You may use a
labelled diagram to help answer this
question.
_______________________________
_______________________________ [3]
d)
Describe the bonding and structure in a
typical metal like sodium. You may use a
labelled diagram to help answer this
question.
Delocalised electrons [1] layers/regular
arrangement/lattice [1] of positive
centres/ions [1] electrostatic attraction [1].
Max [3]
I
II
1
H
1
2
Li
2.1
Be
2.2
3
Na
2.8.1
Mg
2.8.2
4
K
Ca
2.8.8. 2.8.8.2
1
III
IV
V
VI
VII VII
I
He
2
B
2.3
C
2.4
N
2.5
O
2.6
F
2.7
Ne
2.8
Al
Si
P
S
Cl
Ar
2.8.3 2.8.4 2.8.5 2.8.6 2.8.7 2.8.8
138
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Do consider using others in this Series of Ten.
139