2
(e) All gases diffuse.
(i)
Choose from the list of formulae the gas which diffuses most quickly.
Draw a circle around your answer.
CO
(ii)
CO2
CH4
NO2
SO2
[1]
Explain
your answer to (i).
........................................................................................................................................ [1]
(f)State one adverse effect of carbon monoxide on human health.
............................................................................................................................................... [1]
(g) Carbon dioxide, CO2, is a reactant in photosynthesis.
N
ame the two products of photosynthesis.
................................................................... and ������������������������������������������������������������������� [2]
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(h) Complete the dot-and-cross diagram in Fig. 1.1 for a molecule of CO2.
Show outer shell electrons only.
O
C
Fig. 1.1
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O
[2]
[Turn over
4
2Lithium, sodium and potassium are Group I elements.
(a) Name the type of bonding in these elements.
............................................................................................................................................... [1]
(b) Sodium reacts with cold water to form hydrogen gas and a solution of a strong alkali.
(i)
State the test for hydrogen gas.
test .......................................................................................................................................
positive result .......................................................................................................................
[1]
(c) Lithium has two naturally occurring types of atoms, 6Li and 7Li.
(i)
State the name given to atoms of the same element with different nucleon numbers.
........................................................................................................................................ [1]
(ii)
Complete
Table 2.1 to show the number of protons, neutrons and electrons in the atom
and ion of lithium shown.
Table 2.1
6
Li
7
Li+
protons
neutrons
electrons
[3]
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5
(iii)
Table 2.2 shows the relative abundance of the two naturally occurring atoms of lithium.
Table 2.2
atom
6
Li
7
Li
relative abundance
10%
90%
Calculate the relative atomic mass of lithium to one decimal place.
relative atomic mass = .............................. [2]
(d) Potassium oxide, K2O, is an ionic compound.
omplete Fig. 2.1 to show the electronic configurations of the ions in potassium oxide.
C
Show the charges on the ions.
......
K
......
O
Fig. 2.1
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......
K
[3]
[Turn over
6
3The Haber process is used to manufacture ammonia.
(a) State the main source of each gas used in the Haber process.
nitrogen .......................................................................................................................................
hydrogen .....................................................................................................................................
[2]
(b) The equation for the Haber process is shown.
N2(g) + 3H2(g)
2NH3(g)
∆H = –92 kJ / mol
The reaction is reversible. The forward reaction is exothermic.
(i)
State what is meant by the symbol ∆H.
........................................................................................................................................ [1]
(ii)
∆H
for the forward reaction is –92 kJ / mol.
State why this value shows that the forward reaction is exothermic.
........................................................................................................................................ [1]
(iii)
State the typical conditions and name the catalyst used in the Haber process.
temperature .............................. °C
pressure .................................. kPa
catalyst ..........................................
(iv)
[3]
omplete Table 3.1 to show the effect, if any, when the typical conditions in the Haber
C
process are changed. Use only the words increases, decreases or no change.
Table 3.1
change to
typical conditions
effect on the rate of
the forward reaction
temperature increases
increases
effect on the concentration
of NH3(g) at equilibrium
pressure decreases
no catalyst
decreases
[4]
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(v)
Explain in terms of collision theory why increasing the temperature increases the rate of
the reaction.
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
..............................................................................................................................................
........................................................................................................................................ [3]
(c) Ammonia reacts with an acid to form ammonium sulfate, (NH4)2
(iii)
Calculate the percentage composition by mass of nitrogen in (NH4)2SO4.
percentage of nitrogen = ............................... % [2]
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9
(d) Hydrated copper(II) sulfate is a coloured compound. It exists as hydrated crystals which
contain water molecules.
(i)
State the term given to water molecules present in hydrated crystals.
........................................................................................................................................ [1]
(ii)
State
the colour of hydrated copper(II) sulfate crystals.
........................................................................................................................................ [1]
(iii)
Write the formula of hydrated copper(II) sulfate.
........................................................................................................................................ [2]
(e)Copper(II) oxide is formed when copper(II) nitrate, Cu(NO3)2, is heated.
2Cu(NO3)2(s) → 2CuO(s) + 4NO2(g) + O2(g)
(iii)
0.0200 moles of Cu(NO3)2 is heated.
Calculate the mass of 0.0200 moles of Cu(NO3)2.
mass = .............................. g [2]
(iv)Calculate the total volume of gas, in dm3 at r.t.p., produced when 0.0200 moles of
Cu(NO3)2 is heated.
volume = .............................. dm3 [2]
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MARK SCHEME
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12
V
Cr
Mn
Co
27
Ni
28
Cu
29
Zn
30
Fe
57–71
56
55
0620/42/F/M/23
–
90
89
232
thorium
actinium
–
Th
Ac
140
cerium
139
lanthanum
59
231
protactinium
Pa
91
141
praseodymium
Pr
–
58
Ce
–
Db
dubnium
Rf
rutherfordium
La
57
actinoids
105
181
Ta
tantalum
73
93
niobium
Nb
41
51
vanadium
238
uranium
U
92
144
neodymium
60
Nd
–
Sg
seaborgium
106
184
W
tungsten
74
96
molybdenum
Mo
42
52
chromium
–
neptunium
Np
93
–
promethium
61
Pm
–
Bh
bohrium
107
186
Re
rhenium
75
–
technetium
Tc
43
55
manganese
–
plutonium
Pu
94
150
samarium
62
Sm
–
Hs
hassium
108
190
Os
osmium
76
101
ruthenium
Ru
44
56
iron
–
americium
Am
95
152
europium
63
Eu
–
Mt
meitnerium
109
192
Ir
iridium
77
103
rhodium
Rh
45
59
cobalt
–
curium
Cm
96
157
gadolinium
64
Gd
–
Ds
darmstadtium
110
195
Pt
platinum
78
106
palladium
Pd
46
59
nickel
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
Ra
radium
Fr
francium
89–103
178
104
137
88
133
87
Hf
hafnium
Ba
barium
lanthanoids
Cs
72
91
zirconium
Zr
40
48
titanium
caesium
89
yttrium
88
strontium
85
rubidium
Y
39
45
Sr
38
40
Ca
Rb
37
39
K
scandium
–
berkelium
Bk
97
159
terbium
65
Tb
–
Rg
roentgenium
111
197
gold
Au
79
108
silver
Ag
47
64
copper
–
californium
Cf
98
163
dysprosium
66
Dy
–
Cn
copernicium
112
201
Hg
mercury
80
112
cadmium
Cd
48
65
zinc
calcium
Ti
26
potassium
Sc
25
31
24
–
einsteinium
Es
99
165
holmium
67
Ho
–
Nh
nihonium
113
204
Tl
thallium
81
115
indium
In
49
70
gallium
Ga
27
20
24
19
23
aluminium
Al
13
11
boron
magnesium
23
1
sodium
22
B
C
N
7
O
8
VI
F
9
VII
2
VIII
–
fermium
Fm
100
167
erbium
68
Er
–
Fl
flerovium
114
207
lead
Pb
82
tin
119
Sn
50
73
germanium
Ge
32
28
silicon
Si
14
12
carbon
–
mendelevium
Md
101
169
thulium
69
Tm
–
Mc
moscovium
115
209
Bi
bismuth
83
122
antimony
Sb
51
75
arsenic
As
33
31
phosphorus
P
15
14
nitrogen
–
nobelium
No
102
173
ytterbium
70
Yb
–
Lv
livermorium
116
–
Po
polonium
84
128
tellurium
Te
52
79
selenium
Se
34
32
sulfur
S
16
16
oxygen
–
Lr
lawrencium
103
175
lutetium
71
Lu
–
Ts
tennessine
117
–
At
astatine
85
127
iodine
I
53
80
bromine
Br
35
35.5
chlorine
Cl
17
19
fluorine
–
Og
oganesson
118
–
Rn
radon
86
131
xenon
54
Xe
84
krypton
36
Kr
40
argon
18
Ar
20
neon
Ne
10
4
helium
6
V
hydrogen
5
IV
He
Mg
21
relative atomic mass
name
atomic symbol
atomic number
Key
III
H
1
Group
Na
9
11
7
Be
beryllium
Li
4
3
lithium
II
I
The Periodic Table of Elements
12
0
