burette
Online Classes : Megalecture@gmail.com
107° H
D
N
H
H
N
25
H
negatively charged rod
OVERALL BONDING
WS 1
SECTION A
71
Which of the following exists in the solid state as a giant covalent lattice?
Why is a water molecule polar?
A ice
Molecules are bonded together by hydrogen bonds.
B iodine
B The oxygen and hydrogen atoms have different electronegativities.
C
silicon(IV) oxide
. oxygen
C The
atom has two lone pairs of electrons.
D tin(IV) chloride
D !Water is able to dissociate into ions.
A
[Turn over
9701/1/O/N/02
52
Why does copper wire conduct electricity when a potential difference is applied?
A.
Bonding electrons in the crystal lattice move.
B
Copper(II) ions move to the cathode.
C
The atoms of copper become ionised.
!D
The crystal lattice breaks down.
4
67
3
3
helium
at 2iodine
kPa pressure
Flask heated,
X contains
dm3 of
When
solid1iodine
readily
forms
vapour. and flask Y contains 2 dm of neon at 1 kPa
pressure.
What does this information suggest about the nature of the particles in these two physical states
If the
flasks are connected at constant temperature, what is the final pressure?
of
iodine?
8
5
4
A
1solid
!" kPa
A
ionic
atomic
B
ionic
molecular
C molecular
atomic
!D molecular
molecular
C
1 $" kPa
D
2 kPa
3
Which
about solids
the standard
enthalpymolecular
change oflattice?
formation of carbon dioxide is correct?
Which statement
of the following
has a simple
A
A
Itmagnesium
is equal to the
standard enthalpy change of combustion of carbon.
oxide
B
It is equal to twice the bond energy of the C=O bond.
B
C
C
D
.
!D
6
9
vapour
B
1 !# kPa
sodium
It is the energy released when one mole of carbon dioxide is formed from carbon at the
silicon(IV) oxide
[Turn over
temperature of combustion of the carbon.9701/1/M/J/02
Itsulphur
is the same for carbon dioxide produced from graphite and from diamond.
Measured
values
of the
pressure,
volume
and temperature of a known mass of a gaseous
Use
of the Data
Booklet
is relevant
to this
question.
compound are to be substituted into the equation
Hydrazine was used as a fuel for the Messerschmidt 163 rocket fighter in World War II and for the
pV = Gemini
nRT and Apollo spacecraft. It has the following formula.
American
in order to calculate the relative molecular
mass, H
Mr, of the compound.
H
N Nwould give the most accurate value of M ?
Which conditions of pressure and temperature
r
H
H
pressure
temperature
CEDAR COLLEGE
OVERALL BONDING WS 1
What is the enthalpy change of atomisation of 1 mol of gaseous hydrazine?
A
A
high
550 kJ
high
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26
6
12 Why does the exothermic reaction
5
∆H = –3 kJ mol–1
C(diamond) ⎯⎯⎯→ C(graphite)
not occur spontaneously?
A
A tetrahedral configuration is always more stable than a planar one.
B
Diamond has only strong covalent bonds whereas graphite has both covalent bonds and van
der Waals’ forces.
C
.
The change from diamond to graphite has a high activation energy.
!D
The density of graphite is less than that of diamond.
4
3
86 A substance commonly found in the house or garden has the following properties.
13
sketch
shows
the variation
of losing
first ionisation
energy
proton set
number
for six
5 The
Which
of thebelow
following
particles
would, on
an electron,
have with
a half-filled
of p orbitals?
elements of consecutive proton numbers between 1 and 18 (H to Ar).
•
It is combustible.
+
B N
C N–
D O
A C–
•
It is an electrical insulator.
6
•
It melts over a range of temperature.
Magnesium oxide is used to line industrial furnaces because it has a very high melting point.
What could the substance be?
Which type of bond needs to be broken for magnesium oxide to melt?
ionisation
A brass
energy
A co-ordinate
B
B
C.
C
D
!D
paper
covalent
poly(ethene)
ionic
silicon(IV) oxide
metallic
X
proton number
9
77
Use of the Data Booklet is relevant to this question.
What
is solid
the identity
of more
the element
X?kind of chemical bonding?
Which
exhibits
than one
In an experiment using a gas syringe, 0.10 g2of a gas is found to occupy 83.1 cm3, measured at
AA Mg
B Al
C Si
D P
brass
standard pressure (1.0 × 105 Pa) and 27 °C.
Section A
B copper
What
is theofrelative
masswith
of the
gas?to form compounds of general formula MO.
14 The
metals
Group molecular
II react readily
oxygen
For
each
C question
diamond there are four possible answers, A, B, C, and D. Choose the one you consider to
0.10 × 8.31 × 27
be correct.
A
When
each
of 5these
oxides is added to water, which forms the most alkaline solution?
D ice
1.0
× 10
× 83.1
!
A MgO
B× 300
CaO
C SrO
D BaO
0.10
18 Which
type ×of8.31
bonding
is never found in elements?
B
5
1.0 × 10 enthalpy
× 83.1 changes of formation of iron(II) oxide, FeO(s), and aluminium oxide,
8 The standard
–1
and –1676 kJ mol–1 respectively.
AAl2O
covalent
3(s), are –266 kJ mol
0.10
×each
8.31of× 27
15 One
mole
of
the
following
compounds is strongly heated and any gas produced is
C
5 × 83.1
–6 and pressure.
at
room
temperature
B.collected
ionic
1.0
×
10
×
10
What is the enthalpy change under standard conditions for the following reaction?
3 of gas likely to be collected?
0.10compound
× 8.31 × 300
CFrom
metallic
which
is 24 dm
D
3FeO(s)
+ 2Al (s) ! 3Fe(s) + Al 2O3(s)
5
–6
1.0 ×of
10any
× 83.1
× 10
[One mole
gas occupies
24 dm3 at room temperature and pressure.]
D van der Waals’ forces
AA
+ 8782kJ
MgCl
– 878
kJ
B BMgCO
3
C
C –1942
kJ
Mg(NO
3)2
D
D –2474
kJ
Mg(OH)
2
[W’15 2 Q1]
Arsenic chloride, AsCl 3, reacts with sodium borohydride, NaBH4.
2
9
Which substance, in 1 mol dm–3 aqueous solution, would have the same hydrogen ion
pAsCl 3 + qNaBH4 → rAsH3 + sNaCl + tBCl 3
concentration as 1 mol dm!3 of hydrochloric acid?
What
are the numbers
p, q, r, s and t when this equation is balanced correctly?
A ethanoic
acid
9701/1/O/N/03
B
nitricp acid
q
CA sodium
2 hydroxide
3
DB sulphuric
acid
3
3
CEDAR COLLEGE
C
4
3
r
s
t
2
3
1
3
3
2
4
3
3
OVERALL BONDING WS 1
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C
The electronegativity of fluorine is much higher than for other elements in the group.
D
There is hydrogen bonding between HF molecules.
27
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6
9
Three substances, R, S, T, have physical properties as shown.
electrical conductivity
mp / oC
substance
bp / oC
3 of solid
5
In which
hydrogen bonds
R process are801
1413broken?
of liquid
poor
good
A
H2S(l) → H2(g) 2852
3600
poor
good
B
NH
T3(l) → NH3(g)
3550
4827
good
not known
C 2HI(g) → H2(g) + I2(g)
What could be the identities of R, S and T ?
D CH4(g) → C(g) + 4H(g)
6
107
R
S
T
Which of the following least resembles an ideal gas?
A
NaF
KCl
Cu
A ammonia
B
NaBr
BaO
SiO2
B helium
C
NaCl
MgO
C [graphite]
C hydrogen
D
NaBr
CaO
C [diamond]
!D trichloromethane
The diagram shows part of the lattice structures of solids X and Y. [In X,
particles of different elements.]
© UCLES 2005
[Turn over
9701/01/M/J/05
X
represent
Y
What are the types of bonding present in X and Y?
!
X
Y
A
covalent
metallic
B
ionic
covalent
C
ionic
metallic
D
metallic
ionic
CEDAR COLLEGE
OVERALL BONDING WS 1
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© UCLES 2006
9701/01/M/J/06
[Turn over
E(C≡O) 1077 kJ mol–1
E(C–O): Megalecture@gmail.com
360 kJ mol–1
Online Classes
4 kJ mol–1
E(C–H) 28410
5 kJ mol–1
E(H–H) 436
What are the lattice structures of solid
diamond, iodine
and silicon(IV) oxide?
–1
3
–3
kJ molin a polystyrene beaker of negligible heat
E(O–H)
460
9 50 cm of 2.50 mol dm hydrochloric
acid was
placed
molecular
simple
molecular
capacity. Its giant
temperature
was recorded and
then
50 cm3 of 2.50 mol dm–3 NaOH at the same
What
is the enthalpy
change
of this
temperature
was quickly
added,
withreaction?
stirring. The temperature rose by 17 °C.
A
diamond, silicon(IV) oxide
iodine
–1
kJ
mol
A
–537
The resulting solution may be considered to have a specific heat capacity of 4.2 J g–1 K–1.
B
diamond, iodine
silicon(IV) oxide
B –101 kJ mol–1
What
molar enthalpy
change
of neutralisation of hydrochloric acid
C is an approximate
iodine value for the diamond,
silicon(IV)
oxide
–1
and
sodium
hydroxide
from
this
experiment?
C +101 kJ mol
D
silicon(IV) oxide
diamond, iodine
!D +537
−(50 kJ
x 4 mol
.2 x–1
17 )
1
−
A
J mol
(0.050 x 2 .5)
8
Which equation represents the standard enthalpy change of atomisation of bromine?
Which−(solid
a simple
molecular
lattice?
50 x 4 has
.2 x 17
)
125
1
B
J mol −
A Br(20(l)
.10→x 22Br(g)
.5 )
A calcium fluoride
−(100
x 4 .2 x 17 )
1
Br
B
C nickel
2(g) → 2Br(g) J mol −
(0.050 x 2 .5)
C silicon(IV)
oxide
1
C −
Br2(l)x 4→.2 Br(g)
2 (100
x 17 )
1
D
J mol −
D
sulfur
.
!
(50 x 2 .5)
D 21 Br2(g) → Br(g)
117
'
6
The reaction pathway diagram below illustrates the energies of reactants, products and the
9
In an experiment, 50.0 cm3 of a 0.10 mol dm–3 solution of a metallic salt reacted exactly with
25.0 cm3 of 0.10 molsubstance
dm–3 aqueous sodium sulphite.
R
S
T
transition
state
E1
/ oC
2852
3550
The half-equation for mp
oxidation
of sulphite ion 801
is shown below.
Three substances,
S and T, have physical properties as shown.
1310 transition
state of a R,
reaction.
bp / oC
14132−
3600
4827
+
–
SO 32− (aq)
E2 + H2O(I) → SO 4 (aq) + 2H (aq) + 2e
electrical conductivity
ofreactants
solid
poor
poor
good
energy
If the original oxidation number of the metal in the salt was +3, what would be the new oxidation
What could
be metal?
the identities of R, S and T ?
number
of the
E3
products
A +1
B +2 S
C T +4
D +5
R
10
A
MgO
NaCl
C [graphite]
reaction coordinate
Nitrogen
dioxide
according to the following equation.
B
MgO decomposes
NaClon heating SiO
2
Which expression represents the activation energy of the forward reaction?
(g)[graphite]
2NO(g) + O2(g)
C
NaCl
MgO 2NO2C
B E1 – E 3
C E2 – E 3
D (E1 – E2) – (E2 – E3)
A E1 – E 2
D
NaCl
SiO2into a 1 dm3 container
When
4 mol
of nitrogen MgO
dioxide were put
and heated to a constant
!
temperature, the equilibrium mixture contained 0.8 mol of oxygen.
11 In whichthe
change
van der Waals’
forces
have
be overcome?
theto
temperature
of the experiment?
valuewould
of theonly
equilibrium
constant,
Kc, at
What
© UCLES
2010is
9701/12/O/N/10
A
A
B
evaporation
0 .8 2 × 0 .8 of ethanol
B 1 .6 × 02 .8
42
2 .4
melting of ice
→2 C H OH(g)
C2H5OH(l)
C 1 .6 ×2 02.8 5
D
4
H2O(s) → H2O(l)
C
melting of solid carbon dioxide
CO2(s) → CO2(l)
D
solidification of butane
C4H10(l) → C4H10(s)
© UCLES 2011
CEDAR
© UCLESCOLLEGE
2007
9701/11/M/J/11
9701/01/O/N/07
1 .6 2 × 0 . 8
2 .4 2
[Turn
OVERALL BONDING
WSover
1
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For each question there
are four
possible
answers, A, B, C, and D. Choose the one you consider to
Online
Classes
: Megalecture@gmail.com
be correct.
29
1
14
Three elements, X, Y and Z, have the physical properties shown in the table.
element
melting point
/ °C
X
–7
boiling point
/ °C
density
/ g cm-3
3
5
59
3.12
Y helps to explain
98
0.97the compound CHCl 3 exist as
The presence of dipoles
why the 883
element Br2 and
liquids at room temperature.
Z
649
1107
1.74
Which types of dipole are involved?
What could be the identities of X, Y and Z?
Br2
X
Y
Z
induced dipoles and permanent
dipoles
Br2
Al
Si
induced dipoles and permanent
Br2
Na
Mg
dipoles
A
A
B
B
.
C
I2 inducedMg
Na
dipoles only
D
I2
! D
2
15
6
CHCl 3
induced dipoles and permanent
dipoles
induced dipoles only
induced dipoles and permanent
dipoles
Si
K
induced dipoles only
induced dipoles only
Use of the Data Booklet is relevant to this question.
Three compounds have the physical properties shown in the table.
Lead(IV) chloride will oxidise bromide ions to bromine. The Pb4+ ions are reduced to Pb2+ ions in
this reaction.
compound
P
Q
R
melting
point / is
°Cadded to 2852
993 bromide–119
If 6.980 g of lead(IV)
chloride
an excess of sodium
solution, what mass of
bromine would be produced?
boiling point / °C
3600
1695
39
B 1.598
g
C poor
3.196 g
D 6.392 g poor
A 0.799 g
conductivity
(solid)
poor
3
conductivity (liquid)
good
good
poor
Which element has an equal number of electron pairs and of unpaired electrons within orbitals of
conductivity
insoluble
good
insoluble
principal quantum
number (aqueous)
2?
A beryllium
What might be the identities of P, Q and R?
B carbon
C
nitrogen
P
D A oxygen
MgO
!
7
Q
R
KCl
NH3
B
MgO
NaF
C2H5 Br
C
SiO2
KCl
C2H5 Br
D
SiO2
NaF
HCl
For the equilibrium 2SO2(g) + O2(g)
© UCLES 2011
A
adding a catalyst
B
adding more O2
C
increasing the pressure
D
increasing the temperature
CEDAR COLLEGE
8
2SO3 (g), what will change the value of Kp ?
9701/11/O/N/11
OVERALL BONDING WS 1
Which pollutant, present in the exhaust www.youtube.com/megalecture
fumes of an internal combustion engine, has an element
in the +2 oxidation state and an odd number of electrons in one molecule of the pollutant?
4
In which species does the underlined atom have an incomplete outer shell?
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A
165
Al 2Cl 6
B
CH3+
C 30
Cl 2O
D
H2Cl C•
Which solid contains more than one kind of bonding?
A
iodine
B
silicon dioxide
C
sodium chloride
!D
zinc
3 4
Kak
•••/
•§
••
*t
a.
•
•
8
175
6
The
diagram
shows
the Maxwell-Boltzmann
energy
curves for molecules of a sample
Some
car paints
contain
small flakes of silica,
SiOdistribution
2.
Use
of the
Booklet temperatures.
is relevant to this question.
of a gas
at Data
two different
In the structure of solid SiO2
The
gasletter
laws on
canthe
be axes
summarised
in the
gas
equation.
Which
represents
theideal
most
probable
energy of the molecules at the lower
temperature?
● each silicon atom is bonded
to x oxygen atoms,
pV = nRT
qq.a.INT
••
Hm
o••
● each oxygen atom is bonded to y silicon atoms,
0.96 g of oxygen gas is contained in a glass vessel of volume 7000 cm3 at a .temperature of 30 °C.
A
● each bond is a z type bond.
F \
What is the pressure in the vessel?
What is the correct combination
of x, y and z in this statement?
B B2.1 kPa
C 10.8 kPa
D 21.6 kPa
A 1.1 kPa
•
I
•
•
7
x
y
z
oxygen
Two moles of compound P were placed in a vessel. The vessel was heated and compound P
A partly decomposed
2
covalent
silicon chemicals P, Q and
was
to1produce Q
and R. A dynamic equilibrium between
R was
B established.
2
1
ionic
At equilibrium
and the total number of moles present was (2 + x ).
C
4 x moles of R2were present
covalent
.
2
D
4
2
ionic
What is the equation for this equilibrium reaction?
!
C D
A P
2Q + R
9 BJohn
Dalton’s
theory, published in 1808, contained four predictions about atoms.
2P pair 2Q
+atomic
R
of elements
has chemical bonds of the same type between their atoms in the solid
186 Which
state?
is still considered to be correct?
CWhich
2P of his
Q +predictions
R
A aluminium and phosphorus
DA 2P
Q + are
2R very small in size.
All atoms
B chlorine and argon
B All the atoms of a particular element have the same mass.
C magnesium and silicon
C All the atoms of one element are different in mass from all the atoms of other elements.
D sulfur and chlorine
!
D 2012
No atom can be split into simpler parts.
© UCLES
9701/12/M/J/12
[Turn over
7
Ethanol has a boiling point of 78 °C. At 101 kPa and 79 °C ethanol vapour does not perfectly obey
gas equation
pV = nRT.
10 the
A student
calculated
the standard enthalpy change of formation of ethane, C2H6, using a method
based on standard enthalpy changes of combustion.
What is the reason for this?
He used correct values for the standard enthalpy change of combustion of ethane
Ethanol vapour is in equilibrium with ethanol liquid at 79 °C.
(–1560 kJ mol–1) and hydrogen (–286 kJ mol–1) but he used an incorrect value for the standard
enthalpy
of combustion
carbon.the
Hemolecules
then performed
hisvapour.
calculation correctly. His final
B
There change
are intermolecular
forcesofbetween
of ethanol
answer was –158 kJ mol–1.
A
C
The vapourisation of ethanol liquid is an endothermic process.
What
did he will
usenot
forobey
the standard
enthalpy
changeatofsuch
combustion
of carbon?
D
Vapours
the gas equation
perfectly
a low pressure.
A
–1432 kJ mol–1
B
–860 kJ mol–1
C
–430 kJ mol–1
CEDAR
D COLLEGE
–272 kJ mol–1
OVERALL BONDING WS 1
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.
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31 3
5
19
Two conversions are outlined below.
NH4+
NH3
C2H4
C2H6
What similar feature do these two conversions have?
5
A
a lone pair of electrons in the product
B
change in oxidation state of an element 3
C
in bond particles
angle of the
species
involved
. decrease
Which
of the following
would,
on losing
an electron, have a half-filled set of p orbitals?
D
!A
6
6
20
disappearance
of
B a N bond
C–
N–
C
+
D
O
Use
of the Data
Booklet
to this furnaces
question.because it has a very high melting point.
Magnesium
oxide
is usedistorelevant
line industrial
The
gas
laws
summarised
in thefor
ideal
gas equation.
Which
type
of can
bondbeneeds
to be broken
magnesium
oxide to melt?
A
pV = nRT
co-ordinate
B covalent
g of ethene gas is contained in a vessel at a pressure of 102 kPa and a temperature of 30 °C.
0.56
C ionic
What is the volume of the vessel?
D metallic
!A 49 cm3
B 494 cm3
7
7
C
48 900 cm3
D
494 000 cm3
Which solid exhibits more than one kind of chemical bonding?
Propanone has the molecular formula C3H6O.
A brass
The enthalpy change of combustion of hydrogen is –286 kJ mol–1.
B copper
The enthalpy change of combustion of carbon is –394 kJ mol–1.
C enthalpy
diamond change of combustion of propanone is –1786 kJ mol–1.
The
D ice
Using this information, what is the enthalpy change of formation of propanone?
8
A –1106 kJ mol–1
The standard enthalpy changes of formation of iron(II) oxide, FeO(s), and aluminium oxide,
–1
Al2O–540
–266
kJ mol–1 and –1676 kJ mol–1 respectively.
B
kJ mol
3(s), are
kJenthalpy
mol–1 change under standard conditions for the following reaction?
C
What–254
is the
D
+1106 kJ mol–1
3FeO(s) + 2Al (s) ! 3Fe(s) + Al 2O3(s)
8
A + 878
kJ set of conditions
B – 878 kJ
C likely
–1942tokJbehave Dideally?
–2474 kJ
Under
which
is a gas most
9
temperature
pressure
Which substance, in 1 mol dm–3 aqueous solution, would have the same hydrogen ion
concentration
as 1 mol dm!3 of hydrochloric
acid?
A
high
high
A B ethanoic high
acid
low
B C nitric acidlow
high
low
C D sodium hydroxide
low
D
sulphuric acid
CEDAR
© UCLESCOLLEGE
2012
9701/11/M/J/12
OVERALL BONDING
WS 1over
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32
3
213
The table gives the radii, in pm, of some ions. [1 pm = 10–12 m]
ion
radii
Na+
102
Mg2+
72
Cs+
167
Cl –
181
2–
O
140
Caesium chloride, CsCl, has a different lattice structure from both sodium chloride, NaCl, and
magnesium oxide, MgO.
CsCl lattice
NaCl and MgO lattice
Which factor appears to determine the type of lattice for these three compounds?
!
A
the charge on the cation
B
the ratio of the ionic charges
C
the ratio of the ionic radii
D
the sum of the ionic charges
© UCLES 2010
CEDAR COLLEGE
9701/12/O/N/10
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5
6
222
4
C The height of the peak, P, decreases and the activation energy does not
change.
Na2S2O3 reacts with
diluteClasses
HCl to give
a pale yellow precipitate. If 1 cm3 of 0.1 mol dm–3 HCl is
Online
: Megalecture@gmail.com
Hydrazine, N2H3 4, is used as a–3 rocket fuel because it reacts with oxygen as shown, producing
D The
peak,
P, increases
activation
energy
moves to the left.
added
to height
10 cm ofofthe
0.02
mol dm
Na2S2O3and
the
precipitate
forms
slowly.
33the
‘environmentally friendly’ gases.
If the experiment is repeated with 1 cm3 of 0.1 mol dm–3 HCl and 10 cm3 of 0.05 mol dm–3 Na
2S 2O3
O2(g)of→their
N2(g)
+ 2Hproperties
= –534
kJ table.
mol–1
N 2H
4(l) + Some
2O(g)
Substances
X,forms
Y andmore
Z arequickly.
all
solids.
physical
are∆H
given
in the
the
precipitate
Despite its use as a rocket fuel, hydrazine does not burn spontaneously in oxygen.
Why is this?
substance
X
Y
Z
–3
Which
explains
why hydrazine is
does
notwhen
burn0.05
spontaneously?
A
Thestatement
activation
energy
lower
3 is used.
melting
point
/ °C of the reaction
772
114 mol dm Na2S2O1610
Hydrazine
is a between
liquid.
mol dm–3 Na2S2O3 is
The
collisions
reactant
particles are more183
violent when 0.05 2205
boiling
point
/ °C
1407
used.
B The
activation
energy is too high.
electrical
conductivity
conducts
does not conduct
does not conduct
–3
C Theofreactant
the liquidparticles
state collide more frequently when 0.05 mol dm Na2S2O3 is used.
C The N N bond is very strong.
–3
D
The
reaction
proceeds
by asubstance
different pathway
What
type
of lattice
each
have? when 0.05 mol dm Na2S2O3 is used.
D
The
reaction
is could
exothermic.
A
B
6
7
X free radical substitution
Y
Z
Which stage
in the
of ethane by chlorine
will have the lowest activation
A 10.0 cm3 bubble of an ideal gas is formed on the sea bed where it is at a pressure of 2020 kPa.
energy?
A
giant molecular
simple molecular
ionic
Just below the sea surface the pressure is 101 kPa and the temperature is the same as the sea
●
A B Cl 2 → 2Cl
ionic
giant molecular
simple molecular
bed.
ionic
giant molecular
HCl molecular
B C Cl ● + C2H
6 → C2H5● +simple
What is the volume of the bubble when it rises to just below the sea surface?
ionic
giant molecular
● + Clmolecular
C D C2H5simple
2 → C2H5Cl + Cl ●
!A 10.0 cm3
B 20.2 cm3
C 200 cm3
D 2 020 000 cm3
D Cl ● + C2H5● → C2H5Cl
238
7
Four substances have the physical properties shown.
Measured values of the pressure, volume and temperature of a known mass of a gaseous
Which substance
is an
ionic solid?
compound
are to be
substituted
into the equation pV = nRT.
The measurements are used to calculate9701/12/M/J/14
the relative molecular
mass, Mr, of a compound.
electrical
electrical
electrical
boiling point
melting point
conductivity
conductivity
conductivity
Which conditions of pressure and temperature
would give theof
most
accurate value
of Mr?
molten
of aqueous
/ °C
/ °C
of solid
substance
solution
pressure
temperature
A
–115
–85
poor
poor
good
A
high
high
B
660
2470
good
good
insoluble
B
high
low
C
993
1695
poor
good
good
C
low
high
D
1610
2230
poor
poor
insoluble
! D
low
low
© UCLES 2014
8
24
:
Which solid contains more than one kind of bonding?
A
copper
B
diamond
C
ice
!
magnesium oxide
D
©
© UCLES
UCLES 2013
2014
CEDAR COLLEGE
9701/13/O/N/13
9701/13/M/J/14
[Turn over
OVERALL BONDING WS 1
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12
Which chlorine compound has bonding that can be described as ionic with some covalent
character?
Online Classes : Megalecture@gmail.com
A
4
2513
B
NaCl
MgCl2
AlCl
4 3
34
C
D
SiCl4
Methanol may be prepared by the reaction between carbon monoxide and hydrogen.
Al Cl3 reacts with LiAl H4 and (CH3 )3 N to give (CH3 )3 NAl H3 .
CO(g) + 2H2(g) → CH3OH(g)
Which statement about (CH3 )3 NAl H3 is correct?
The relevant average bond energies are given below.
A It contains hydrogen bonding.
!
8
26
E(C≡O) 1077 kJ mol–1
B
It is dimeric.
C
360 kJ mol–1
The Al atom has an incompleteE(C–O)
octet of electrons.
D
.
410 kJarranged.
mol–1
The bonds around the Al atom E(C–H)
are tetrahedrally
4
E(H–H) 436 kJ mol–1
Solid carbon dioxide, CO2, is similarE(O–H)
to solid iodine,
I2, in–1its structure and properties. Carbon is in
460 kJ mol
Group 14. Silica, SiO2, is a Group 14 compound.
What is the enthalpy change of this reaction?
Which statement about solid CO2 and solid SiO2 is correct?
–537 kJ mol–1
Both solids exist in a lattice structure.
–101 kJ mol–1
Both solids have a simple molecular structure.
+101 kJ mol–1
Both solids have atoms joined by single covalent bonds.
+537 kJ mol–1
Both solids change spontaneously to gas at s.t.p.
A
A
B
B
C
C
D
!D
© UCLES 2007
5
27
9
9701/01/M/J/07
Which solid has a simple molecular lattice?
An article in a science magazine contains the following statement.
A calcium fluoride
‘It is lighter than a feather, stronger than steel, yet incredibly flexible and more conductive than
B nickel
copper.’
C silicon(IV)
oxide is being described?
Which
form of carbon
sulfur
!AD buckminsterfullerene
:
56
28
3
B
diamond
Some
car paints
contain
small flakes
silica, SiO
2. energies of reactants, products and the
The reaction
pathway
diagram
belowofillustrates
the
state of a reaction.
Ctransition
graphene
In the structure of solid SiO2
D graphite
transition state
● each silicon atom
E1 is bonded to x oxygen atoms,
● each
atom change
is bonded
to y silicon
atoms,
10 Which equation
hasoxygen
an enthalpy
of reaction
which
corresponds to the standard enthalpy
change of atomisation of chlorine?
● each bond is a zE2type bond.
energy
reactants
1
Cl (g)
A 2 Cl 2(g)
What is the correct combination of x, y and z in these statements?
B
C
§
D
A
B
1
2
Cl 2(l)
Cl (g)
x
Cl 2(g)
Cl 2(l)
y
E3
products
z
2Cl (g)
2
2
2Cl (g)
1
covalent
1
ionic
reaction coordinate
D
Which expression
represents
activation
energy of the forward reaction?
4
2 of the
covalent
11 In C
an experiment,
2.00 mol
hydrogen
and 3.00 mol of iodine were heated together in a sealed
container
at2 –a Efixed
temperature.
B toE21reach
– E3 equilibrium
C E
D (E1 – The
E2) –container
(E2 – E3) had a fixed
AD E1 – Eand
2 4 allowed
3
ionic
!volume of 1.00 dm3. At equilibrium, there were 2.40 mol of iodine present in the mixture.
2HI(g)
H2(g) + I2(g)
Solid sulfur consists of molecules made up of eight atoms covalently bonded together.
© UCLES 2010
9701/12/O/N/10
What is the value of the equilibrium constant, Kc?
The bonding in sulfur dioxide is O=S=O.
A 0.107
B 0.357
C 0.429
D 2.33
6
enthalpy change of combustion of S8,
CEDAR COLLEGE
–1
S8(s)= –2376kJ mol
OVERALL BONDING WS 1
into gaseous atoms = 2232 kJ mol–1
energy required to break 1 mole S8(s) www.youtube.com/megalecture
–1
C
D
4
3
4
3
3
Online Classes : Megalecture@gmail.com
6
4
4
4
4
3
35
12 The graph below shows the variation of the first ionisation energy with proton number for some
The lettershave
used
not theproperties
usual symbols
thetable.
elements.
3 elements.
Three substances
theare
physical
shown for
in the
29
substance
melting point
/ °C
boiling point
/ °C
P
conductivity
(solid)
conductivity
(liquid)
conductivity
(aqueous)
U
420
907
good
good
insoluble
V
993
1695
poor
good
good
W
–70
58
poor
poor
hydrolyses, resulting
solution conducts well
first ionisation
kJ mol–1 of U, V and W?
What couldenergy
be the/identities
A
5
6
30
U
V
W
Na
KCl
SiCl 4
X
W
U
R
3
V
T
B
Na
NaF
C2H5Br
S
Which molecule has no overall dipole?
Q
C
Zn
KCl
HCl
B CH2Cl 2
C CHCl 3
D CCl 4
A CH3Cl
D
Zn
NaF
SiCl 4
proton number
!
Whichsolid
statement
about
elements
Which
contains
morethe
than
one typeisofcorrect?
bonding?
A iodine
P2015
and
©A
UCLES
X are in the same period in the9701/12/O/N/15
Periodic Table.
B
B
The general
silicon
dioxideincrease from Q to X is due to increasing atomic radius.
C
C
sodium
chloride
The small
decrease from R to S is due to decreased shielding.
D
D
zinc
The small decrease from U to V is due to repulsion between paired electrons.
[S’18 1 Q6]
7
13
31
Enthalpy
changes
of combustion
cantendency
be used to
enthalpy
changes of formation. The
Which element
shows
the greatest
to determine
form covalent
compounds?
following equation represents the enthalpy change of formation of butane.
A boron
4C(s) + 5H2(g) → C4H10(g)
B magnesium
By using the following standard enthalpy of combustion data, what is the value of the standard
C neonchange of formation,
enthalpy
, of butane?
D
328
potassium
substance
4
[W’16 2 Q13]
C(s)
–394
Solid carbon dioxide, CO2, is similar to solid iodine, I2, in its structure and properties. Carbon is in
Group 14. Silica, SiO2, is a Group 14
compound. –286
H2(g)
(g) SiO is –2877
4H10solid
correct?
Which statement about solid CO2Cand
2
¥
±
A
A
–1
–5883
kJ molexist
Both solids
in a lattice structure.
B
B
mol–1have a simple molecular structure.
–129
Both kJ
solids
C
C
mol–1have atoms joined by single covalent bonds.
+129
Both kJ
solids
D
D
–1
kJ molchange
+2197
Both solids
spontaneously to gas at s.t.p.
[M’16 Q8]
2–
Ethanedioate
C2O
with a suitable
reagent
to form CO2. A half-equation for this
An article in a ions,
science
magazine
the following
statement.
4 , react contains
reaction is shown.
‘It is2016
lighter than a feather, stronger than steel,
yet incredibly flexible and more conductive than
© UCLES
9701/12/O/N/16
copper.’
C2O42– → 2CO2 + 2e–
89
CEDAR
COLLEGE
Which
formisofcorrect?
carbon is being described?
Which
row
A
buckminsterfullerene
oxidation state of
OVERALL BONDING WS 1
www.youtube.com/megalecture
Decide whether each of the statements is or is not correct (you may find it helpful to put a tick against
the statements that you consider to be correct).
Online Classes : Megalecture@gmail.com
14 of
The responses A to D should be selected on the36
basis
A
B
Section B
SECTION
B C
D
For each of the questions in this section, one or more of the three numbered statements 1 to 3 may
1 and 2 only are 2 and 3 only are 1 only is correct
be correct. 1, 2 and 3 are
correct
correct
correct
Decide whether each of the statements is or is not correct (you may find it helpful to put a tick against
the statements that you consider to be correct).11
No other combination of statements is used as a correct response.
Section
B of
The responses A to D should be selected on
the basis
For
of the
questionshave
in this
section,
oneformula
or moreCH
of the
three numbered statements 1 to 3 may be
31 each
Which
compounds
the
empirical
2O?
A
B
C
D
correct.
12
1 methanal
1 onlyto put a tick against
2 and
1 andis2or is not correct
1, each
2 andof
3 the statements
Decide whether
(you3 may find it helpful
is
only
are
only
are
are
Thestatements
responses
A toacid
D should
be selected
on the basis of
the
that
you
consider
to be correct).
2 ethanoic
correct
correct
correct
correct
3 methylA methanoate
The responses
to D A
should be selectedBon the basis of C
D
No other combination of statements is used as a correct response.
1, 2 and 3 are
1 and 2 only are 2 and 3 only are 1 only is correct
A
B
C
D
correct are features
correct
132 Which of the following
of the structurecorrect
of metallic copper?
1, 2 and
3 are the
1 and
2 only
are 12of
2 and
are 1 only is correct
31 The diagram
illustrates
energy
changes
a set3ofonly
reactions.
correct
correct
correct
1 combination
ionic bonds of statements is used as a correct response.
No other
Section_ B
H = _134 kJ mol 1
2
delocalised
electrons
R
S
No other combination of statements
is used as a correct response.
For each
of the questions
in thisinto
section,
one is
or an
more
of the threereaction
numbered
). 3 may
33
The
conversion
of
graphite
diamond
endothermic
(∆Hstatements
= +3 kJ mol1–1to
3
lattice
of
ions
be correct.
④
2 Silicon tetrachloride, SiCl4, is a liquid
C(graphite)
→ C(diamond)
of low boiling
point. In the presence of water it decomposes
31
Decide whether each of the statements is or is not correct (you may find it helpful to put a tick against
to
form
silicon(IV)
oxide
and
hydrogen
chloride.
the statements
that you about
consider
be correct). extraction of aluminium are correct?
33
Which statements
thetocommercial
1
Which statements are correct?
H = +92 J mol
(I)?
What
types
of
bonding
occur
in
SiCl
The 1responses
A to D should
beisselected
on–the
basis
→diamond
Al. of is smaller than that of graphite.
The enthalpy
cathode
reaction
Al 3+ +4 3e
1 The
change
of atomisation
of
12 co–ordinate
The bond
liningenergy
ofbonding
the electrolytic
cell acts as the cathode.
2 The
of the C–C
is greater than that inDdiamond.
A
B bonds in graphite
C
_
_
1
12
23 covalent
bondingis purified Al
HO
= 75 Na
kJ mol
The enthalpy
electrolyte
3 The
changeTof combustion
diamond
2 3 in of
3AlF6. isU greater than that of graphite.
1, 2 and 3
1 and 2
2 and 3
1 only
van der
forces beonly
The 3responses
to D should
selected
areAWaals
are on the basis
onlyofare
is
Which
of the following statements
correct
correct are correct? correct
correct
3
34 Which
Which of
of the
the following
following statements
magnesiumare
compounds
mass when
by a below
bunsen
flame?
correct for lose
the sequence
of heated
compounds
considered
C into
from1left The
toAright?
enthalpyare
change
forBtheontransformation
U ⎯→
R isalkylsulphates
+ 42 kJ mol–1D
.for use as detergents,
32 Long-chain
alkanes
converted
an industrial scale
1 sodium
magnesium
carbonate
e.g.
lauryl of
sulphate.
No other
combination
statements is used as a correct response.
2NaF
The
enthalpy
for
the2transformation
⎯→3S is endothermic.
1, 2
and
3MgO change
and
2Tand
1 only
Al1N
SiC
2 magnesium
nitrate
are
only
are
only
are
3 The enthalpy change for the transformation RO⎯→ T is – 33 kJ mol–1 is
.
correct
correcttobetween
correct in each compound
correctincreases.
The
electronegativity
difference
the
elements
31 1
Use
of
the
Data
Booklet
is
relevant
this
question.
3 magnesium oxide
CH (CH
ONa
2 The formula-units of these
compounds
(have the same number of
2)10CH2O areS isoelectronic
and has been found in lobsters and seaweed
The technetium–99 isotope (99Tc)3 is radioactive
electrons).
No other
combination
of
statements
is
used
as
a
correct
response.
adjacent to nuclear fuel reprocessing plants.
O
3 The bonding becomes increasingly covalent.
99
Which statements are correct about an atom of Tc?
sulphate
434 Which pairs of compounds containsodium
one thatlauryl
is giant
ionic and one that is simple molecular?
1 It has
13 moreare
neutrons
than
protons.
35 Which
statements
reasons
why
sulphur dioxide is used as a food preservative?
1 Al 2deductions
O3 and Al 2about
Cl 6 the properties of this substance can be made from this structure?
What
2 It has 43 protons.
9701/1/O/N/02
1 SiO
It is and
a reducing
2
SiCl 4 agent and therefore an anti-oxidant.
2
It hasof99
nucleons.
13 Part
the
structure is polar and is water–attracting.
2 PItOprevents
alcohols forming sour-tasting acids.
3
4 10 and PCl 3
2 The alkyl chain is soluble in oil droplets.
3 It does not smell and therefore can be used in more than trace quantities.
532 Which of the following solids contain more than one type of chemical bond?
3 All the C-C-C bond angles are tetrahedral.
UCLES 2004
35 ©When
coal is burnt, gaseous oxides of9701/01/O/N/04
carbon and sulphur are formed which pollute the
1 brass (an alloy of copper and zinc)
One method
of preventing
such acid
pollution
involves
adding
calcium
carbonate
36 atmosphere.
Why is the addition
of concentrated
sulphuric
to solid
potassium
iodide
unsuitable
for to
thethe
burning
coal.
The
temperature
of
the
process
causes
the
decomposition
of
the
calcium
carbonate
preparation
of
hydrogen
iodide?
2 graphite
into calcium oxide.
13 ice
Hydrogen iodide is not displaced by sulphuric acid.
Which reactions will be important in helping to reduce atmospheric pollution?
2 Iodide ions are oxidised to iodine.
refining,
by sulphite.
the Claus process, the H2S is
33 1Many
crude oxide
oils contain
sulphur
as Hdioxide
Calcium
reacts with
sulphur
to form
calcium
2S. During
3converted
The product
is contaminated
compounds.
into solid
sulphur, whichby
is sulphur
then removed.
2 Calcium oxide reacts with sulphur dioxide and more air to form calcium sulphate.
[Turn overWS 1
9701/1/M/J/03
CEDAR COLLEGE
OVERALL BONDING
reaction I
2H2S(g) + 3O2(g) → 2H2O(l) + 2SO2(g)
3 Calcium oxide reacts with carbon monoxide to form calcium carbonate.
reaction II
2H2S(g) + SO2(g) → 2H2O(l) + 3S(s)
⑥
②
⑨
②
www.youtube.com/megalecture
correct
correct
correct
correct
31 The relative molecular mass of a molecule of chlorine is 72.
Online Classes : Megalecture@gmail.com
11
No Which
other combination
statements
is used
as a37
correct
properties ofofthe
atoms in this
molecule
are theresponse.
same?
Section B
1 radius
6 31 Which diagrams represent part of a giant molecular structure?
For each of the questions in this section, one or more of the three numbered statements 1 to 3 may
2 nucleon number
be correct.
11
1
2
3
3 relative isotopic mass
Decide whether each of
= C (you may find it helpful to put a tick against
= the
C statements is or is not correct
= Na
the statements that you consider to be correct).Section B
= Cl
32 each
Whichofmolecules
are planar?
For
the
questions
in
this
section,
one
or
more
of
the
three
numbered
statements
1
to
3
may
The responses A to D should be selected on the basis of
be correct.
11
1 BCl3
A
B
C
D
Decide
each of the statements is orSection
is not correct
(you may find it helpful to put a tick against
B
2 whether
NH3
the statements
that3 you consider1 to
be2correct).
1, 2 and
and
2 and 3
1 only
3
PH
3 are
For each of the
questions in thisonly
section,
of the
are one or moreonly
are three numbered isstatements 1 to 3 may
The
responses
A to D should becorrect
selected on the basis
of
be
correct.
correct
correct
correct
⑧
whether
of the statements
is or is is
notplaced
correctabove
(you may
find it helpful
tick
against
7Decide
33 Boron
is a
non-metallic
element
which
aluminium
in Group
the
Periodic
Aeach
B
C
Dto putIIIaof
No statements
other combination
ofconsider
statements
isnitrogen
used as known
a correct
the
that you
be
correct).
forms
a compound
with
asresponse.
boron nitride which has a graphite structure.
32 Table.
WhichItreactions
are redoxto
reactions?
④
1, 2 and 3
1 and 2
2 and 3
1 only
The responses
A2 +to
D should
selected
on2 +
the
basis
of
Which
of the
following
beSO
drawn
from
this information? is
2H
→beCaSO
+ can
Br
1 CaBr
2SO4 conclusions
2 + 2H
2O are
only4are
only
31 How mayare
nitrogen exist in compounds?
correct
correct
correct
correct
PO4nitride
)2 + 2HBr
CaBr
12 The
empirical
formula
of boron
is BN. 13
2 + 2H3PO
4 → Ca(H
A
B2bond
C
D
1 bonded
by a triple covalent
23 The
boron
and nitride
atoms
to be2 arranged
a hexagonal pattern.
CaBr
)2 +likely
2AgBr
2 +32AgNO
3 → Ca(NO
1,
2part
and
1
andis23are
andresponse.
3B alternately1inonly
2 as
of a cation
No other
combination
of statements
used as a Section
correct
arenitride has a layer
onlystructure
are
is the layers.
3 Boron
with vanonly
der are
Waals’ forces between
3 having
lost 3 electrons correct
to form an anion
correct
correct
correct
For
each
of
the
questions
in
this
section,
one
or
more
of
the
three
numbered
statements 1 to 3 may
33 Sodium hydrogensulfide, NaSH, is used to remove hair from animal hides.
8be
31 correct.
The Group IV elements carbon, silicon and germanium all exist in a diamond structure. The bond
lengths
in
these structures
areSH
–
No
combination
of statements
isgiven
used
as
correct response.
ionbelow.
areaquestion.
correct?
Which
statements
about
the
32 other
Use
of the
Data Booklet
is relevant
to
this
Decide whether each of the statements is or is not correct (you may find it helpful to put a tick against
99
1 isotope
It contains
18
electrons.
element
X and
C in lobsters
Si and seaweed
Ge adjacent to nuclear
the statements
that
consider
to behas
correct).
Tc you
is
radioactive
been found
The
31 How
may nitrogen plants.
exist in compounds?
fuel reprocessing
bond of
length
X– X /surround
nm
0.154
0.234
0.244
2 Three lone pairs
electrons
the
sulfur atom.
The1responses
A to
D should
be bond
selected on the
basis
of
bonded
by
a
triple
covalent
99
Which statements are correct about an atom of Tc?
3 Sulfur has an oxidation state of +2.
bond
2Whyasdoes
part the
cationlength increase down the group?
Aof amore
C
D
1 2005
It has 13
neutrons than B
protons.9701/01/O/N/05
© UCLES
[Turn over
overlapstate
decreases
31 inOrbital
an oxidation
of +5 down the group.
2 It 1,
has
protons.
2 43
and
3
1 and 2
2 and 3
1 only
2 Atomic
radius increases down
the group.
are
only
are
only
are
is
3 It has 99 nucleons.
31 3–
32 2–
correct
correct
correct
correct
P and down
sulfidethe
iongroup.
have the same number of which sub-atomic
32 The
ion 15increases
3 phosphide
Nuclear charge
16 S
particles?
© UCLES 2010
9701/11/M/J/10
33
Which of these substances have a giant structure?
9No
other
combination of statements is used as a correct response.
neutrons
32 1Sodium
ions can be formed from sodium atoms.
1 silicon(IV) oxide
Use2 of the
Data Booklet may be appropriate for some +questions.
electrons
Na(s) → Na (g)
2 baked clay found in crockery
3 protons
Which
quantitiesVare
required to calculate the enthalpy change of formation of gaseous sodium
) oxide
3 phosphorus(
31 ions?
Which statements about the atoms 23Na and 24Mg are correct?
10
33 Which substances have a giant structure?
1 enthalpy
They have
the same
number of
electron orbitals.
1
change
of atomisation
of filled
sodium
1 calcium oxide
2 first
They
have theenergy
sameofnumber
2
ionisation
sodiumof neutrons.
2
calcium
3 enthalpy
They arechange
both reducing
agents.
3
of formation
of sodium
3 baked clay found in crockery
⑨
⑤
④
32 Which compounds contain covalent bonds?
11
© UCLES 2012
1
aluminium chloride
2
ammonia
3
calcium fluoride
⑧
[Turn over
9701/12/O/N/12
[Turn over
33 Ethylene glycol, HOCH2CH2OH, is used as a de-icer. It allows ice to melt at temperatures below
0 °C.
© UCLES 2006
CEDAR
COLLEGE
© UCLES 2012
Which statements are correct?
1
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BONDING
over WS 1
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Ethylene glycol changes the extensive network of hydrogen bonds in ice.
correct
correct
correct
correct
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No other combination of statements is used as a correct response.
38
12
33 Which substances contain delocalised electrons?
34
1
cyclohexene
2
graphite
3
sodium
②
033 ]
Solids W, X, Y and Z are compounds of two different Group II metals. Some
of their
2 applications
[ 843
are described below.
Compound W is used as a refractory lining material in kilns.
Compound X is used as a building material. It can also be heated in a kiln to form compound Y.
When Y is hydrated, it forms compound Z which is used agriculturally to treat soils.
Which statements about these compounds are correct?
35
1
Adding W to water has less effect on pH than adding Y.
2
Adding Z to soil increases the pH of the soil.
3
The metallic element in Y reacts with cold water more quickly than the metallic element in W.
Which properties increase in the sequence hydrogen chloride, hydrogen bromide and hydrogen
iodide?
1
thermal stability
2
bond length
3
ease of oxidation
© UCLES 2013
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PAGE
39 220
BONDING WS 1
OVERALL BONDING WS 2
2
For
Examin
Use
111 (a) Give the full electron configuration of the following.
2K
'
2
352
pb
Is
(i) Mg ............................................................................................................................
(ii)
'
2K
2 pb
Is
.........................................................................................................................
Mg2+
2p4
'
is as
(iii) O ..............................................................................................................................
2k 2p2
Is
(iv) O2– ...........................................................................................................................
[2]
'
(b)
(i) Describe, with the aid of a diagram, the lattice structure of magnesium oxide.
:*
:
2-
(ii) Use your diagram to interpret and explain two physical properties of magnesium
oxide.
point
not
conduct
and
does
..................................................................................................................................
electricity
high melting
mas
It
..................................................................................................................................
..................................................................................................................................
..................................................................................................................................
(iii) State two large scale uses of magnesium oxide.
blast
of
the
insides
furnaces
..................................................................................................................................
Lining
Used
!
in
spark
.
..................................................................................................................................
pings
[5]
Electrical
.
•
CEDAR COLLEGE
CEDAR COLLEGE
Ceramics
insulators
.
.
.
BONDING WS 1
OVERALL BONDING WS 2
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40221
PAGE
2
122
(a) Salt, sodium chloride, forms transparent colourless crystals. Describe the bonding in
sodium chloride crystals, give the formula of each particle and sketch part of the crystal
structure.
:
For
Examiner’s
Use
:
[3]
(b) Explain why crystals of sodium chloride do not conduct electricity, but molten sodium
chloride does.
to
ions
are
The
free
In
form
..........................................................................................................................................
liquid
and
more
the
..........................................................................................................................................
carry
!
charge
.
......................................................................................................................................[2]
(c) (i)
(ii)
With the aid of a diagram of the cell, outline the manufacture of chlorine from brine
[ N' 03 QB
(aqueous sodium chloride).
Write the electrode equations, including state symbols.
anode ........................................................................................................................
cathode .....................................................................................................................
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COLLEGE
CEDAR
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WS2 1
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2
The
below gives
on someofoxides
of elements
in Period
3 of the
Periodic oxide.
Table.
(a)
Writetable
an equation
for data
the reaction
aluminium
with oxygen
to form
aluminium
Online Classes : Megalecture@gmail.com
PAGE
41 223
......................................................................................................................................[1]
oxide
Na O
MgO
Al O
SiO
P O
SO
2
2
3
2
4
10
3
33 Drawing
(b)
diagrams
appropriate,
terms of853
structure
melting
point /where
K
1193
3125 suggest
2345 in 1883
290and bonding,
explanations for the following.
boiling point / K
(i)
1548
3873
3253
2503
–
318
the high melting point and boiling point of Al2O3
(a) Write an equation for the reaction of aluminium with oxygen to form aluminium oxide.
A 1203......................................................................................................................................[1]
structure
ions
a
are
has
that
of
goin
These
held
(b) Drawing
diagramsby
where
appropriate,ionic
suggestbonds
in terms of
structuremake
and bonding,
strong
together
.
it
has
(ii)
explanations for the following.
difficult
very
(i)
a
to
break
Lattice
the
A 1203
SO
,
the high melting point and boiling point of Al2O3
and
melting
high
point
.
the low boiling point of SO3
exists
503
as
a
molecule
covalent
simple
intermolecular
boiling
and
by of SO
the low boiling point
3
(ii)
required
to
overcome
'
-
dipoles
bonds
these
point
boiling
its
hence
weak
by
induced
caused
forces
(iii)
together
held
is
is
den
The
.
less
is
energy
.
the melting point of SiO2 is much higher than that of P4O10
sick
exists
held
(iii)
Large
as
a
macromolecule
together by strong
and
covalent
is
bonds
-
.
required to
energy
to
bonds
Paolo
compared
theamounts
melting point of SiO
of 2 is much higher thanisthat of P4O10
these
overcome
which
is
weak
simple
a
IMF
covalent
structure
with
.
[7]
© UCLES 2004
!
9701/02/O/N/04
[7]
© UCLES 2004
CEDAR COLLEGE
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9701/02/O/N/04
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For
Examiner’s
Use
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PAGE
42225
4
5
24
Copper and iodine are both solids which have different physical and chemical properties.
Each element has the same face-centred crystal structure which is shown below.
For
Examiner’s
Use
The particles present in such a crystal may be atoms, molecules, anions or cations. In the
diagram above, the particles present are represented by
.
(a) Which type of particles are present in the iodine crystal? Give their formula.
Molecules
particle ....................................
.
T
2
formula ....................................
[2]
-
(b) When separate samples of copper or iodine are heated to 50 °C, the copper remains as
a solid while the iodine turns into a vapour.
(i)
Explain, in terms of the forces present in the solid structure, why copper remains a
solid at 50 °C.
is
in
held
a
metallic
lattice
copper
..................................................................................................................................
together
,
Where
cations
surrounded
ar
Iz
..................................................................................................................................
by electrons
.
Vander wants
non
weak
is
held
forces
together by
..................................................................................................................................
(ii)
.
Explain, in terms of the forces present in the solid structure, why iodine turns into a
vapour when heated to 50°C.
Waals
der
van
Is is held together by
..................................................................................................................................
weaker
'
50°C
at
overcome
are
forces
that
..................................................................................................................................
!
.
..................................................................................................................................
[4]
© UCLES 2006
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CEDAR COLLEGE
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BONDING WS 1
OVERALL BONDING WS 2
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On the diagram, sketch the π bond that is also present in ethene.
[1]
(a) Give the equation, with state symbols, for the reaction of phosphorus with chlorine to
form
phosphorus(V)
chloride,
PCl:5.Megalecture@gmail.com
Online
Classes
(e) Carbon,
hydrogen
and
ethene
each burn exothermically in an excess of air.
43
......................................................................................................................................[2]
∆H oc = –393.7 kJ mol–1
C(s) + O2(g) → CO2(g)
58 Suggest, in terms of the structure and bonding, explanations
(b)
the following.
H2(g) + ½O2(g) → H2O(l)
∆H oc =for–285.9
kJ mol–1
You should draw diagrams where you think they will help your answer.
C2H4(g) + 3O2(g) → 2CO2(g) + 2H2O(l)
the high melting point of sodium chloride
(i)
'
Use the data to calculate the standard enthalpy change of formation, ∆H of , in kJ mol–1,
held
is at 298
by
NaCl
of ethene
K. together
2C(s)
strong
(ii)
∆H oc = –1411.0 kJ mol–1
that
bonds
ionic
+ 2H2(g) → C2H4(g)
mine
.am
÷:
t.I.IT
o
energy
-
•
"
.
.
I:
the low melting point of silicon tetrachloride
silly
with
the
is
weak
covalent
simple
a
der
Vom
molecules
Waals
'
forces
[Total: 13]
.
[4]
!
© UCLESCOLLEGE
2007
CEDAR
© UCLES 2007
CEDAR COLLEGE
structure
= ................................. kJ mol–1
[3]
between
∆H of
9701/02/O/N/07
9701/02/O/N/07
[Turn
BONDING
WS 1over
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2
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PAGE
44233
Answer all the questions in the spaces provided.
6 The elements carbon and silicon are both in Group IV of the Periodic Table.
13
1
Carbon is the second most abundant element by mass in the human body and silicon is the
second most common element in the Earth’s crust.
For
Examiner’s
Use
Carbon and silicon each form an oxide of general formula XO2.
At room temperature, CO2 is a gas while SiO2 is a solid with a high melting point.
(a) Briefly explain, in terms of the chemical bonds and intermolecular forces present in each
compound, why CO2 is a gas and SiO2 is a solid at room temperature.
in
which
bond ,
covalent
macromolecule
si 02
exists
as
..........................................................................................................................................
for it to melt ,
overcome
need to be
regaining lots of energy
..........................................................................................................................................
covalent
with
Waals
weak
der
molecule
van
CO2 is a simple
..........................................................................................................................................
forces
that
.
'
tip
easily
....................................................................................................................................
[3]
overcome
are
at
r
.
.
(b) Draw a simple diagram to show the structure of SiO2. Your diagram should contain at
least two silicon atoms and show clearly how many bonds each atom forms.
••
•
•
j.MY
.
Silicon
oxygen
.
÷•o.¥
i.
.
.
k
point
connected
Key
'
here
'
to
!
each
© UCLES 2009
CEDAR COLLEGE
CEDAR COLLEGE
oxygen
is
4
to
that
each
silicon
and
oxygens
2
in
silicon
[2]
s
.
9701/22/O/N/09
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PAGE
45235
4
7
15
2
Copper, proton number 29, and argon, proton number 18, are elements which have different
physical and chemical properties.
In the solid state, each element has the same face-centred cubic crystal structure which is
shown below.
For
Examiner’s
Use
The particles present in such a crystal may be atoms, molecules, anions or cations. In the
.
diagram above, the particles present are represented by
(a) Which types of particle are present in the copper and argon crystals?
In each case, give their formula.
element
particle
formula
Cations
copper
Ar
atoms
argon
at
cu
.
[2]
At room temperature, copper is a solid while argon is a gas.
(b) Explain these observations in terms of the forces present in each solid structure.
solid
held
state
cations
In the
Copper has
..........................................................................................................................................
firmly
,
in a
electrons
of de localised
metallic
sea
by strong
..........................................................................................................................................
it
gives
high
..........................................................................................................................................
bonds
.
This
on
the
other
stable
a
hand
has
weak
MP
with
structure
.
caused
IMI
..........................................................................................................................................
Argon
,
,
These
overcome
induced
forces
dipoles
are
..........................................................................................................................................
easily
by
at
the
room
temperature
....................................................................................................................................
by
energy
.
.
!
© UCLES
2010
CEDAR
COLLEGE
CEDAR COLLEGE
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.................................................................................................................................... [2]
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46
7
[Total: 10]
8 Separate samples of the oxides MgO and SiO are melted.
16
(d)
2
For
Examiner’s
Use
Each molten sample is then tested to see whether or not it conducts electricity.
Suggest what would be the results in each case. Explain your answers.
moving
atomic
will
have
free
compound
MgO .................................................................................................................................
,
molten
when
ions
..........................................................................................................................................
.
..........................................................................................................................................
ionic
ions
Not
SiO2 .................................................................................................................................
no
,
.
..........................................................................................................................................
!
..........................................................................................................................................
[4]
[Total: 12]
4
9 (c) Cerium is a lanthanoid metal that shows similar chemical reactions to some elements in the
third period. Most of cerium’s compounds contain Ce3+ or Ce4+ ions.
(i) Cerium shows the same structure and
bonding as a typical metal.
© UCLES 2010
9701/22/M/J/10
CEDAR COLLEGE
Draw a labelled diagram to show the structure and bonding in cerium.
-
to
①
00
[Turn over
BONDING WS 1
-
-
[2]
(ii) Cerium(IV) oxide, CeO2, is a ceramic.
Suggest two physical properties of cerium(IV) oxide.
Point
1. .........................................................................................................................................
High Melting
insulator
Elictrical
2. .........................................................................................................................................
[2]
.
!
© UCLES
2010
CEDAR
COLLEGE
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over
OVERALL BONDING
WS
2
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47 239
PAGE
4
19
10
(d) Sodium and silicon also react directly with chlorine to produce the chlorides shown.
chloride
melting
point / °C
difference between the
electronegativities of the elements
NaCl
801
2.2
SiCl 4
–69
1.3
(i) Describe what you would see during the reaction between sodium and chlorine.
would
react
chlorine
Sodium
with
,
.............................................................................................................................................
rapidly
giving
The
.............................................................................................................................................
bright yellow I orange light
yellow I green gas
.
solid forms
disappears and white
.......................................................................................................................................
[2]
.
(ii) Explain the differences between the melting points of these two chlorides in terms of their
structure and bonding. You should refer to the difference between the electronegativities
of the elements in your answer.
t
structure
lattice
NaCl has a
goin
NaCl structure and bonding ...............................................................................................
in
ions
bonds
ionic
with
place
holding the
.............................................................................................................................................
strong
.
molecular
simple
SiCl 4 structure and bonding ................................................................................................
molecules
btw
induced dipoles
covalent
bonding and
.............................................................................................................................................
structure
with
.
'
in
difference
explanation .........................................................................................................................
electronegativity
Large
es
to
form ions
electrons
leads to a
NaCl
in
transfer of
.............................................................................................................................................
held
These
electrostatic
are
then
.............................................................................................................................................
together by strong
force
attraction
of
.
.............................................................................................................................................
melting point
giving
Nau
high
in
difference
small
For
the
silly
.............................................................................................................................................
electronegativity
a
,
!
in
to
induced
and
shape leads
.......................................................................................................................................
[4]
symmetry
dipoles
energy
© UCLES 2015
CEDAR COLLEGE
CEDAR COLLEGE
as
to
that
IMF
break
,
dom of
resulting
9701/21/M/J/15
in
require
low
M
a
.
P
lot
and
of
[Total: 20]
B. P
.
BONDING WS 1
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.
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48
4
112
Structure and bonding can be used to explain many of the properties of substances.
(a) Copper, ice, silicon(IV) oxide, iodine and sodium chloride are all crystalline solids.
Complete the table with:
● the name of a type of bonding found in each crystalline solid,
● the type of lattice structure for each crystalline solid.
crystalline solid
type of bonding
copper
Metallic
ice
Covalent
silicon(IV) oxide
covalent
iodine
covalent
sodium chloride
ionic
type of lattice structure
Metallic
hydrogen
simple
lattice
bonded
molecular
Macromolecular
molecular
simple
Giant
ionic
lattice
[5]
(b) (i) Name the strongest type of intermolecular force in ice.
.......................................................................................................................................
[1]
Hydrogen branding
(ii) Draw a fully labelled diagram of two water molecules in ice, showing the force in (i) and
how it forms.
ft
H
H
\
J
I
O
• •
-
•
✓
•
I
Hydrogen
,
'
"
ft
H
lol
•
•
•
t
-
[3]
!
CEDAR COLLEGE
.
H
•
© UCLES 2017
bonding
9701/21/M/J/17
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