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Chemical Bonding Tutorial
Section A: Review Questions
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1 Which of the following statements explains why copper conducts
electricity when a
potential difference is applied?
A Copper(II) ions move to the cathode
B The crystal lattice breaks down
C Electrons combine with copper(II) ions
D Bonding electrons in the crystal lattice move
2 Which bonding type does not correspond to its description of
physical properties?
Bonding type Physical properties
A Giant covalent High melting point, conducts electricity when
in solution but not
when solid
B Simple covalent Low melting point, does not conduct
electricity in any state
C Metallic Variety of melting points, conducts electricity when
solid and
when molten
D Ionic High melting point, conducts electricity when molten but
not
when solid
3 The C2H2 molecule is linear.
What can be deduced from this about the numbers of and pi bonds
present in the
molecule?
pi
A 2 2
B 2 3
C 3 1
D 3 2
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4 Why is the molecule of BCl3 planar, whereas the molecule of
PH3 is pyramidal?
A The boron atom has no d-orbitals available for bonding.
B The boron atom in BCl3 has 6 electrons in its valence shell,
while the phosphorous
atom in PH3 has 8.
C The repulsion between chlorine atoms is greater than that
between hydrogen atoms.
D The covalent radius of phosphorus is greater than that of
boron.
5 MBTE is a constituent of petrol.
What are the values of angle P and angle Q in a molecule of
MTBE?
Angle P Angle Q
A 90 105
B 90 180
C 109 105
D 109 180
6 AlCl3 reacts with LiAlH4 and (CH3)3N to give (CH3)3NAlH3.
Which statement about (CH3)3NAlH3 is correct?
A It contains hydrogen bonding
B It is dimeric
C The Al atom is electron deficient
D The shape about the Al atom is tetrahedral
7 Why is the boiling point of methane greater than that of neon?
[Ar: H, 1; C, 12; Ne, 20]
A A molecule of methane has a greater mass than a molecule of
neon.
B A molecule of methane has more electrons than a molecule of
neon.
C Molecules of methane have stronger intermolecular forces than
those of neon.
D Molecules of methane form hydrogen bonds, but those of neon do
not.
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8 Which of the following solids consists of atoms or molecules
held together only by van der
Waals forces?
A CO2
B Cu
C H2O
D MgO
9 Which of the following molecules will not form a hydrogen bond
with another of its own
molecules?
A CH3CHO
B CH3NH2
C CH3OH
D NH3
10 When heated, solid iodine readily forms iodine vapour.
What does this information suggest about the nature of the
particles in these 2 physical
states of iodine?
Solid Vapour
A ionic atomic
B ionic molecular
C molecular atomic
D molecular molecular
11 Which set of properties could apply to a non-ionic compound
which has a giant lattice?
Physical state at room
temperature
Electrical conductivity in
molten state
Melting point / C
A liquid Does not conduct -114
B liquid Does not conduct Melts over a range
C solid Conducts well 808
D solid Does not conduct 1610
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The responses A to D should be selected on the basis of
A B C D
1, 2 and 3
are correct
1 and 2
only are correct
2 and 3
only are correct
1 only
is correct
No other combination of statements is used as a correct
response.
12 Which of the following are features of the structure in
metallic copper?
1 Ionic bonds
2 Delocalised electrons
3 Lattice of ions
13 In microwave ovens, the wave energy produced is absorbed by
certain polar molecules.
Which of the following would absorb microwave energy?
1 C2H5OH
2 NaCl
3 SiO2
14 The boiling points of pentane and 2,2-dimethylpropane are 36
C and 9 C respectively.
Which of the following suggested factors help to account for
this difference in boiling
points?
Pentane 2,2-dimethylpropane
1 The molecule of 2,2-dimethylpropane is more compact than that
of pentane.
2 The covalent bonds in pentane are stronger than those in
2,2-dimethylpropane.
3 There is more effective hydrogen bonding in pentane than in
2,2-dimethylpropane.
15 Many ceramic materials based on silicon(IV) oxide have
recently been developed. Which
properties apply to these materials?
1 They are heated during manufacture and form solids.
2 They are heat-resistant solids.
3 They are good conductors of electricity due to delocalised
electrons.
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16 a) Explain what is meant by sigma () and pi (pi) bonds.
Illustrate your answers with
suitable diagrams.
Refer to lecture notes Page 13 and 14.
b) How many sigma () and pi (pi) bonds are present in the
propene (C3H6) molecule?
8, 1pi
17 For the following particles,
draw their dot-and-cross diagrams
count the total number of lone pairs and bond pairs
state their shapes according to VSEPR theory
draw their shapes
give the bond angles about the central atom
state whether they are polar or non polar (only applicable for
molecules)
Particle Dot-and-cross diagram / Structure
Bond pairs
/ Lone
pairs
Shape, Bond
Angle, Polarity
NF3
!
3 bp
1 lp
Trigonal
pyramidal 107
SiF4
!
4 bp
0 lp
tetrahedral
109
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Particle Dot-and-cross diagram / Structure
Bond pairs
/ Lone
pairs
Shape, Bond
Angle, Polarity
CH2Cl2
!
4 bp
0 lp
tetrahedral
109
ICl3
!
3 bp
2lp
T shape
90
ClO
NH2
2 bp
2 lp
Bent
105
H3O+
3 bp
1 lp
Trigonal
pyramidal
107
NO3
3 bp
0 lp
Trigonal planar
120
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Particle Dot-and-cross diagram / Structure
Bond pairs
/ Lone
pairs
Shape, Bond
Angle, Polarity
AlH4
4 bp
0 lp
tetrahedral
109
BrCl2
2 bp
3 lp
Linear
180
I3
2 bp
3 lp
Linear
180
SO42
!
4 bp
0 lp
tetrahedral
109
18 a) Describe the bonding present in
(i) solid krypton, 36Kr,
Solid krypton exists as a lattice of atoms with weak van der
Waals forces between Kr
atoms.
(ii) solid rubidium, 37Rb.
Rubidium has a giant metallic lattice with strong metallic bonds
between the cations
and the sea of delocalised electrons.
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b) Use your descriptions of their bonding to explain why the
boiling point of krypton is
152C whereas that of rubidium is 686C, despite their having
nearly the same
relative atomic mass, Ar.
More energy is required to overcome the stronger
metallic bonds in Rb than the weak van der Waals
forces in Kr. Hence Rb has a higher b.p. than Kr.
19 The table below gives the boiling points of four organic
compounds:
formula relative molecular mass boiling point /oC
A CH3CH2CH2CH2CH3 72 36
B (CH3)4C 72 10
C CH3CH2CH2CH2OH 74 117
D CH3CH2OCH2CH3 74 35
By comparing i) A with B, ii) A with C and iii) C with D,
suggest explanations for the
differences in the boiling points within each of the three
pairs.
i) A with B
Both A and B have simple molecular structure with weak
van der Waals forces between molecules.
A has a straight chain structure while B has a more
spherical shape due to its highly branched structure.
The vdW forces between A molecules are stronger than that of B
due to the large
surface area of contact. More energy is required to overcome the
stronger vdW forces,
higher bp.
ii) A with C
Both A and C have simple molecular structure. There are weak van
der Waals forces
between A molecules, and H-bonds between C molecules.
More energy is required to overcome the stronger H-bonds than
vdW forces, so C has
a higher bp.
iii) C with D
Both C and D have simple molecular structure. There are H-bonds
between C
molecules and pd-pd interactions between D molecules.
More energy is required to overcome the stronger H-bonds than
pd-pd interactions, so
C has a higher bp.
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20 Explain the following observations in terms of the structure
and bonding present.
a) 4-hydroxybenzoic acid is more soluble in water than
2-hydroxybenzoic acid.
OH
O OH
4-hydroxybenzoic acid
O OH
OH
2-hydroxybenzoic acid
!
!
In 2-hydroxybenzoic acid, COOH and OH
groups are close to each other.
They can form intramolecular H-bonds
This reduces the chance of forming H-bonds
with water molecules.
Hence it is less soluble in water
b) In benzene solution, the measured relative molecular mass of
methanoic acid is
approximately 92.0. Explain the observation and include a
relevant diagram in your
answer.
In benzene solution, methanoic acid dimerises through
hydrogen bonds.
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Section B: Discussion Questions
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1 In which of the following pairs does the first substance have
a higher melting point than the
second?
First Second
A CH3CH2OCH3 CH3CH2NHCH3
B (CH3)3CH CH3CH2CH2CH3
C RbCl KCl
D
2 The concepts of bond energy, bond length and bond polarity are
useful when comparing
the behaviour of similar molecules.
Compared with the HCl molecule, the bond __X__ of the HI
molecule is __Y__.
Which pairs of words correctly complete the above sentence?
X Y
1 energy greater
2 length greater
3 polarity less
3 In which of the following reactions is the bond angle in the
product greater than that in the
reactant?
1 H2O (l) + H+ (aq) ! H3O
+ (aq)
2 C2H4 (g) + H2 (g) ! C2H6 (g)
3 CO2 (g) + OH- (aq) ! HCO3
- (aq)
C
O
OH
OHC
O
OH
OH
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4 Carbon forms double bonds with each of the Group VI elements
oxygen, sulfur and
selenium. In each case, the double bond is polar.
In the molecules CO2, COS and COSe, the polarities of these
double bonds do not
necessarily cancel.
Overall polarity of molecule
CO2 0
COS 0.71
COSe 0.73
Which factors could account for these observations?
1 The C=S bond is more polar than the C=Se bond.
2 The C=O bond is more polar than the C=S bond.
3 The C=Se bond is more polar than the C=O bond.
5 In 1985, a molecular form of carbon, C60, called
buckerministerfullerene, was discovered in
the products formed when graphite was vapourised. The structure
proposed for the
molecule is a roughly spherical collection of atoms in the shape
of hexagons and
pentagons, very much like a soccer ball.
Which of the following properties is expected of
buckerministerfullerene?
1 It dissolves in various organic solvents.
2 It has a high melting and boiling point.
3 It can conduct electricity.
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6 When magnesium is burnt in air, a mixture of the ionic solids
magnesium oxide, MgO,
and magnesium nitride, Mg3N2, is formed.
a) Explain why magnesium metal is deformed by an applied force,
whereas magnesium
oxide is shattered.
Mg has a giant metallic lattice with strong metallic
bonds between cations and the sea of delocalised electrons. MgO
has a giant ionic
lattice of cations and anions with strong ionic bonds between
ions.
When a force is applied to Mg, the cation layers slide past one
another, but the sea
of delocalised electrons move to prevent repulsion between the
cations. Hence, the
metal is deformed.
When a force is applied to MgO, the lattice is displaced
slightly and the ions with
similar charge come together and repel. Hence, the lattice
breaks apart and shatters.
b) Use a dot-and-cross diagram to describe the bonding in
Mg3N2.
c) State the factors that affect the magnitude of the lattice
energy of an ionic
compound.
!
q qLattice energy | |
r r
+
+ +!
(proportional to product of the ionic charge and inversely
proportional to the sum of
the ionic radii)!
q+ and q- represent the charges on the cation and anion, and r+
and r- the ionic
radius of the cation and anion.
d) How would you expect the magnitudes of the lattice energies
of the oxides of the
Group!II elements to vary down the group?
Down group II, the ionic radius of the group II cations
increases due to increasing
number of filled electron shells.
The sum of the ionic radii increases and the magnitude of the
lattice energy
decreases.
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e) Suggest how the magnitude of the lattice energy of Mg3N2
might compare to that of
MgO. Explain your answer.
The magnitude of the lattice energy will increase as N3- is
triply charged and the
product of the ionic charge will increase. (Charge is a more
important factor than
ionic radius.)
7 Antimony, Sb, is in Group V of the Periodic Table. It forms a
series of salts which contain
the SbF5n anion, the structure of which is a square-based
pyramid.
Deduce the total number of electrons around the antimony atom,
the value of n and the
oxidation number of Sb in this ion. [2]
Total number of electrons around Sb = 12.
(1 lone pair and 5 bond pairs ard Sb since the shape is square
pyramidal.)
n = 2, Oxidation number of Sb = +3
8 Hydrogen cyanide, HCN, is a weak acid that is extremely
poisonous and volatile. A
hydrogen cyanide concentration of 300 mg/m3 in air will kill a
human within 1060 minutes.
a) Draw the dot and cross diagram for HCN and predict its
shape.
linear about C
b) Draw the structural formula of the cyanide anion formed upon
dissociation of HCN in
water. Do you notice anything unusual about it?
The negative charge is on the less electronegative C.
(Explain that the cyanide ion is a special case.)
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Page 14 of 18
c) Explain why HCN is so volatile.
HCN has a simple molecular structure with pd-pd interactions
between molecules.
These interactions are weak and require little energy to
overcome, so low bp, high
volatility.
d) HCN, N2 and CO are isoelectronic. The bond energy of the
nitrogen-nitrogen bond in
the nitrogen molecule is 944kJ mol1, whereas the bond energy of
the carbon-oxygen
bond in the carbon monoxide molecule is 1074 kJ mol1. Explain
this observation.
The NN bond is non polar but the CO bond is polar.
There is extra attraction due to partial charges in the
bond.
9 a) Draw structures and state the bond angles for the following
particles.
(i) NO2+ (ii) NO3
(iii) N2O5
180 120 120 about N and 105 about O
b) NO2 has a bond angle of 134 and NO2 has a bond angle of 115,
although VSEPR
theory predicts that both bond angles should be 120.
Explain.
(Both 2 bp, 1 lp.)
When there are have 3 electron pairs around the central atom,
the shape should be
trigonal planar, bond angle 1200.
For NO2-, lp lp repulsion is greater than that of bp bp
repulsion. The bond pairs are
forced to go closer to each other, causing the angle to be
smaller than 120o.
There is only 1 lone electron on N in NO2 (instead of a lp). 1
lone electron will not exert
as large a repulsion on the bond pairs as compared to a bond
pair. Hence, the angle is
smaller than 120o.
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Page 15 of 18
10 It is known that AlCl3 and NH3 react readily.
a) Draw the dot-and-cross diagram of the product of this
reaction. Predict the likely shape
of the product.
tetrahedral about Al and N
b) Explain why these two molecules form a product when they
react in a molar ratio of
1:1.
NH3 has a lone pair available for donation. AlCl3 is electron
deficient and has an
empty, energetically accessible orbital to accept electrons.
c) Similar products may be obtained when the following compounds
are reacted together.
Suggest the structures and shapes of their products.
(i) BeC!2 and NH3
tetrahedral about Be and N
(ii) BF3 and NaF
tetrahedral about B
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Page 16 of 18
11 In 1886, Henri Moissan succeeded in obtaining fluorine by the
electrolysis of molten
potassium difluoride, KHF2, which is an ionic compound
containing one cation and one
anion.
a) Write the formulae of the ions present in KHF2.
K+, HF2
b) Suggest a structure for the anion and state what types of
bonding occur within it.
c) Explain why KHF2 has a melting point of 239 C, but that of KF
and HF are 858 C and
84 C respectively.
KHF2 and KF have giant ionic lattice structure with strong ionic
bonds between ions.
HF has a simple molecular structure with hydrogen bonds between
molecules.
A lot more energy is required to overcome strong ionic bonds
compared to hydrogen
bonds. So HF has the lowest boiling point.
The ionic bond between K+ and F- is stronger than that between
K+ and HF2- as the
size of the HF2 ion is larger. More energy is required to
overcome, higher boiling
point.
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Page 17 of 18
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Section C: Assignment (15 marks)
7->$!)(!9(.$!&1-)!JE!9')!&(!+(9:/$&$!&1'%!-%%'0)9$)&6!!
1 Nitrate, NO3-, and phosphate, PO4
3-, are oxoanions of nitrogen and phosphorus
respectively.
a) Draw dot-and-cross diagrams to show the bonding in NO3- and
PO4
3-. Hence, deduce
the shapes and state the bond angles around the nitrogen and
phosphorus atom. [4]
![1] [1]
Trigonal planar, 120 [1] Tetrahedral, 109 [1]
b) Explain why it is not possible for nitrogen to form an
oxoanion with a formula of NO43-.
[1]
Nitrogen has no empty and energetically accessible 3d orbitals
to expand its octet.
2 This question is on the properties of halogens and their
compounds.
a) Halogens like Cl2 and I2 are soluble in the non-polar solvent
CCl4. However, the
interhalogen compound, ICl, is insoluble in CCl4. Explain why.
[2]
Cl2 and I2 are soluble in CCl4 as they can form van der Waals
interactions with CCl4.
[1]
ICl is insoluble in CCl4 as the energy released during the
formation of vdW interactions
with ICl is not enough to overcome the permanent dipole
permanent dipole
interactions between ICl molecules (and vdW forces between CCl4
molecules). [1]
The hydrogen halides undergo thermal decomposition according to
the following
equation.
2HX ! H2 + X2 (where X represents the halogen)
b) Why is the rate of thermal decomposition of hydrogen fluoride
slower than that of
hydrogen iodide? [2]
The HF bond is shorter than the HI bond. [1] There is less
degree of orbital overlap
and less energy is required to break the bond. [1]
15
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Nanyang Junior College H2/H1 Chemistry JC1 2014
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Page 18 of 18
3 Ethanoic acid, CH3COOH, is the main component of vinegar.
a) Explain, with illustrations, why ethanoic acid is soluble in
water. [2]
Soluble as they can form hydrogen bonds with water [1]
Drawing showing at least 1 H-bond (with +, -, lone pairs, hash
lines) [1]
b) Ethanoic acid (Mr = 60.0) is a liquid while magnesium
fluoride (Mr = 62) is a solid at
r.t.p. Explain. [2]
Ethanoic acid has simple molecular structure with
hydrogen bonds between molecules.
Magnesium fluoride has giant ionic lattice with Mg2+ and
F- ions held together by strong ionic bonds. [1]
More energy is required to overcome the stronger ionic bond so
MgF2 has a higher
melting point and is a solid at rtp, while ethanoic acid is a
liquid. [1]
c) Ethanoic acid undergoes neutralisation with sodium hydroxide
to form sodium
ethanoate.
CH3COOH + NaOH ! CH3COO-Na+ + H2O
Is sodium ethanoate soluble in water? Draw a diagram to explain.
[2]
Soluble. Sodium ethanoate dissociates into its ions in water.
These ions can form ion-
dipole interactions with water. [1]
[1]
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