Chemistry
Subject Code: CHM315114
2014 External Examination Information Sheet
Chemical Data and Constants
QUANTITY
APPROXIMATE VALUE
Standard atmospheric pressure
1.000 atm
101.3 kPa
760.0 mm Hg
Absolute zero temperature (zero kelvin)
−273˚C
Standard temperature & pressure (S.T.P.)
0˚C (273 K) and 101.3 kPa
Standard laboratory conditions (S.L.C.)
25˚C (298 K) and 101.3 kPa
Avogadro's constant (NA)
6.022 x 1023 mol−1
Ideal gas constant (R)
0.0821 L atm K−1 mol−1
8.31 J K−1 mol−1
8.31 L kPa K−1 mol−1
62.4 L mm Hg K−1 mol−1
Molar volume of an ideal gas (S.T.P.)
22.4 L mol−1
Molar volume of an ideal gas (S.L.C.)
24.5 L mol−1
Charge on the electron
−1.602 x 10−19 C
Faraday’s constant (F)
96 500 C mol−1
Specific heat of water (cw)
4.184 J g−1 K−1
Density of liquid water
1.00 g mL−1
One litre (1.00 L)
1000 mL or 1000 cm3
3
One cubic metre (1.00 m )
Unit prefixes:
nano (n)
micro (µ)
10−9
10−6
1000 L
milli (m)
10−3
kilo (k)
103
Page 1 of 10
mega (M)
106
giga (G)
109
tera (T)
1012
Chemical Information
n=
m
M
n = amount of substance (mol)
m = mass (g)
M = molar mass (g mol−1)
N = n NA
N = number of particles
NA = Avogadro's constant (see p.1)
c = concentration (mol L−1)
n = cV
V = volume of solution (L)
P1V1 P2 V2
=
T1
T2
Combined Gas Equation (n constant)
V = gas volume
P = gas pressure
PV = nRT
T = temperature (K)
R = Ideal Gas Constant (see p.1)
n(e−) = amount of electrons (mol)
n(e− ) =
q It
=
F F
q = electrical charge (C)
F = Faraday Constant (see p.1)
E = energy change (J)
E = VIt
V = potential difference (V)
I = electrical current (A)
t = time (s)
E = mcΔT
cf =
E VIt
=
ΔT ΔT
c = specific heat capacity (J g−1 K−1)
ΔT = temperature change (K)
−1
c f = calibration factor (J K )
ρ=
m
V
ρ = density (g mL−1 or g L−1)
Page 2 of 10
COMMON POSITIVE IONS (CATIONS)
1+
ammonium
hydrogen H
lithium Li
2+
+
NH 4
+
+
potassium K
silver Ag
barium Ba
+
3+
2+
aluminium Al
4+
3+
tin (IV) Sn 4+
calcium Ca 2+
chromium (III) Cr 3+
copper (II) Cu 2+
iron (III) Fe 3+
lead (IV) Pb 4+
iron (II) Fe 2+
+
lead (II) Pb 2+
sodium Na +
mercury (II) Hg
magnesium Mg
2+
2+
nickel (II) Ni 2+
tin (II) Sn 2+
zinc Zn
2+
COMMON NEGATIVE IONS (ANIONS)
1–
2–
ethanoate (acetate) CH 3COO
bromide Br
–
–
3–
2–
–
3–
phosphate PO 4
hydrogen phosphate HPO 4
dihydrogen phosphate H 2 PO 4
phosphide
P 3–
oxide O 2–
2–
–
sulfate SO 4
–
hydrogen carbonate HCO 3
hydrogen sulfate
nitride N
chromate
2–
dichromate Cr2 O 7
chloride Cl –
fluoride F
carbonate
3–
2–
CO 3
2–
CrO 4
HSO 4–
sulfide S2–
2–
sulfite SO 3
2–
hydrogen sulfide HS–
thiosulfate S2 O 3
–
hydrogen sulfite HSO 3
2–
oxalate C 2 O 4
hydroxide OH –
iodide I
–
–
nitrate NO 3
–
nitrite NO 2
–
permanganate MnO 4
hydride H
–
SOLUBILITY TABLE FOR COMMON IONIC COMPOUNDS
Negative Ions (anions)
Solubility of Compounds
–
ethanoates (acetates) ( CH 3COO )
nitrates
–
(NO 3 )
–
All soluble
chlorides (Cl )
All soluble except AgCl, PbCl 2 , HgCl 2
–
All soluble except AgBr, PbBr2 , HgBr2
bromides (Br )
–
All soluble except AgI, PbI 2 , HgI 2
iodides (I )
sulfates
2–
(SO 4 )
All soluble except BaSO 4 , CaSO 4 , SrSO 4 , PbSO 4 , Ag 2 SO 4 , SnSO 4
–
hydroxides (OH )
2–
2–
All insoluble except Li 2 CO 3, Na 2 CO 3, K 2 CO 3, Rb 2 CO 3, (NH 4 )2 CO 3
3–
All insoluble except Li3PO 4 , Na 3PO 4 , K 3PO 4 , Rb 3PO 4 , (NH 4 )3PO 4
carbonates (CO 3 )
phosphates (PO 4 )
sulfites
All insoluble except LiOH, NaOH, KOH, RbOH, NH 4 OH, Sr(OH)2 , Ba(OH)2
All insoluble except Li 2 S, Na 2 S, K 2 S, Rb 2 S, (NH 4 )2 S, MgS, CaS, SrS, BaS
sulfides (S )
2–
(SO 3 )
All soluble
All insoluble except Li 2 SO 3, Na 2 SO 3, K 2 SO 3, Rb 2 SO 3 (NH 4 )2 SO 3
Page 3 of 10
Chemical Equilibrium Formulae
For the equilibrium system:
xP + yQ
zR + wS
z
(where none of components P, Q, R or S is a solid)
w
[ R ] [S]
Kc =
x
y
[ P ] [Q ]
– #
–14
˚
–2
K w = !"H +(aq) #$!"OH (aq)
mol2 L at 25 C
$ = 1.00 ×10
NOTE: !H +(aq) # = !H 3O+(aq) #
"
$ "
$
pH = –log !"H +(aq) #$
!"H +(aq) #$ = 10 −pH
Common Coloured Aqueous Ions
COLOURED CATIONS
chromium (III)
cobalt (II)
copper (II)
iron (II)
iron (III)
manganese (II)
nickel (II)
COLOURED ANIONS
Cr3+
Co2+
Cu2+
Fe2+
Fe3+
Mn2+
Ni2+
green
pink
blue
pale green
orange/brown
pale pink
green
CrO42−
Cr2O72−
MnO4−
chromate
dichromate
permanganate
yellow
orange
purple
(*most other non listed aqueous ions
are colourless in solution)
Organic Chemistry
Alkanes:
Alkenes:
Alkynes:
Cyclic Alkanes:
Cyclic Alkenes:
Benzene C 6 H 6
C n H 2n+2
CH
C n H 2n
C n H 2n−2
C n H 2n
C n H 2n−2
CH
CH
CH
CH
CH
Stem Names
Carbon Atoms in Chain
Stem Name
1
2
3
4
5
6
7
8
9
10
meth-
eth-
prop-
but-
pent-
hex-
hept-
oct-
non-
dec-
Side chains and substitutes
methyl
ethyl
propyl
–Br
–Cl
–F
–I
bromo
chloro
fluoro
iodo
–CH 3
–C 2 H 5
–C3H 7
Prefixes
Atoms in molecule
Prefix
1
2
3
4
5
6
7
8
9
10
mono-
di-
tri-
tetra-
penta-
hexa-
hepta-
octa-
nona-
deca-
Page 4 of 10
Functional Groups
class of
compound
functional group
alcohols
R
example of
compound
C n H 2n+2 O
H
O
general formula
H
H
H
H
C
C
C
H
H
H
H
O
propan-1-ol
O
aldehydes
H
C n H 2n O
C n H 2n O 2
C
R
O
H
H
H
C
C
C
H
H
H
H
H
O
H
'
R
H
O
C n H 2n O 2
H
C
O
O
C
O
H
O
C n H 2n O
C
R
H
butanoic acid
R
esters
H
ethanal
O
carboxylic acids
C
H
H
ketones
C
H
C
R
O
'
H
C
C
C
C
H
H
pentan-3-one
H
H
C
C
H
H
H
C
H
H
H
O
H
C
O
H
C
R
H
methyl propanoate
alkyl halides
R
R
R
R
F
Cl
Br
l
C n H 2n+1X
H
H
H
H
H
C
C
C
C
H
H
H
H
1-chlorobutane
Page 5 of 10
Cl
Some Organic Reactions of Aliphatic Compounds
Alkyl halide RX
(X is F, Cl, Br or I).
Alkoxide eg (RCH2O–…..Na+)
+ ½H2
Alkane
HX(g)
Dilute. NaOH (aq)
Active
metal(eg Na)
H2
Loss of H2O
(use H2SO4(l))
Alkene
Secondary
RCHOHR'
Alcohol
+H2O(g)
Addition
polymerisation
(Catalyst)
Polymer
[O]
Ketone
RCOR'
Primary
RCH2OH
[O] using mild
oxidiser eg
acidified
dichromate
[O] with excess
stronger oxidiser
eg acidified
permanganate
Aldehyde
RCHO
Conc H2SO4
Ester
RCOOR'
Hydrolysis (in
presence of catalyst)
[O]
Salt (eg RCOO –…..Na+) + H 2O
Salt (eg RCOO–…..Na+ + ½H2
Salt (eg RCOO–…..Na+) + H 2O + CO2
base eg NaOH
or active metal
or carbonate
Carboxylic acid
RCOOH
Page 6 of 10
Carboxylic acid +
alcohol
RCOOH + R'OH
STANDARD REDUCTION POTENTIALS
AQUEOUS IONS (1 mol/L and 25˚C)
REDUCTION HALF EQUATIONS
VERY
STRONG
OXIDISERS
VERY
WEAK
REDUCERS
F2(g)
+
H2O2(aq) + 2H (aq)
3+
Au (aq)
–
+
MnO4 (aq) + 8H (aq)
Cl2(g)
2-
+
Cr2O7 (aq) + 14H (aq)
+
MnO2(s) + 4H (aq)
+
O2(g) + 4H (aq)
Br2(l)
–
+
NO3 (aq) + 4H (aq)
+
Ag (aq)
2+
Hg (aq)
–
+
NO3 (aq) + 2H (aq)
3+
Fe (aq)
+
O2(g) + 2H (aq)
I2(s)
O2(g) + 2H2O(l)
2+
INCREASING
STRENGTH
AS
OXIDISERS
Cu (aq)
+
SO4 (aq) + 4H (aq)
4+
Sn (aq)
+
S(s) + 2H (aq)
+
2H (aq)
2+
Pb (aq)
2+
Sn (aq)
2+
Ni (aq)
2+
Co (aq)
2+
Cd (aq)
2+
Fe (aq)
3+
Cr (aq)
2+
Zn (aq)
2H2O(l)
2-
2+
VERY
WEAK
OXIDISERS
Mn (aq)
3+
Al (aq)
2+
Mg (aq)
+
Na (aq)
2+
Ca (aq)
2+
Sr (aq)
+
K (aq)
+
Li (aq)
+
2e
–
–
+
+
+
2e
–
3e
–
5e
+
2e
–
–
+
+
+
+
6e
–
2e
–
4e
–
2e
+
3e
+
+
+
–
e
–
2e
–
e
+
+
+
–
e
–
2e
–
2e
+
4e
+
+
+
+
+
+
+
+
+
+
+
+
+
+
2e
–
2e
–
2e
–
2e
–
2e
–
2e
–
2e
–
2e
–
2e
–
2e
–
2e
–
3e
–
2e
–
2e
+
+
+
+
+
+
+
+
2e
–
3e
–
2e
–
e
–
2e
–
2e
–
e
–
e
–
–
–
–
–
E˚(volts)
+2.87
+1.78
+1.50
+1.49
2F (aq)
2H2O(l)
Au(s)
2+
Mn (aq) + 4H2O(l)
–
+1.36
–
+1.36
+1.28
+1.23
+1.09
2Cl (aq)
3+
2Cr (aq) + 7H2O(l)
2+
Mn (aq) + 2H2O(l)
2H2O(l)
2Br (aq)
NO(g) + 2H2O(l)
Ag(s)
Hg(l)
+0.96
+0.80
+0.78
+0.78
NO2(g) + H2O(l)
2+
Fe (aq)
H2O2(aq)
–
2I (aq)
–
4OH (aq)
INCREASING
STRENGTH
AS
REDUCERS
Cu(s)
–
OXIDATION HALF EQUATIONS
Page 7 of 10
+0.40
+0.34
+0.17
+0.15
+0.14
0.00
–0.13
–0.14
–0.25
–0.28
–0.40
–0.41
–0.74
–0.76
–0.83
SO2(g) + 2H2O(l)
2+
Sn (aq)
H2S(g)
H2(g)
Pb(s)
Sn(s)
Ni(s)
Co(s)
Cd(s)
Fe(s)
Cr(s)
Zn(s)
2OH (aq) + H2(g)
Mn(s)
Al(s)
Mg(s)
Na(s)
Ca(s)
Sr(s)
K(s)
Li(s)
+0.77
+0.68
+0.54
VERY
STRONG
REDUCERS
–1.18
–1.71
–2.38
–2.71
–2.87
–2.89
–2.92
–3.05
TABLE OF RELATIVE ATOMIC MASSES (BASED ON
Name
actinium
aluminium
americium
antimony
argon
arsenic
astatine
barium
berkelium
beryllium
bismuth
boron
bromine
cadmium
caesium
calcium
californium
carbon
cerium
chlorine
chromium
cobalt
copper
curium
dysprosium
einsteinium
erbium
europium
fermium
fluorine
francium
gadolinium
gallium
germanium
gold
hafnium
helium
holmium
hydrogen
indium
iodine
iridium
iron
krypton
lanthanum
lawrencium
lead
lithium
lutetium
magnesium
manganese
mendelevium
Symbol
Ac
Al
Am
Sb
Ar
As
At
Ba
Bk
Be
Bi
B
Br
Cd
Cs
Ca
Cf
C
Ce
Cl
Cr
Co
Cu
Cm
Dy
Es
Er
Eu
Fm
F
Fr
Gd
Ga
Ge
Au
Hf
He
Ho
H
In
I
Ir
Fe
Kr
La
Lr
Pb
Li
Lu
Mg
Mn
Md
Atomic
Number
Relative
Atomic
Mass
89
13
95
51
18
33
85
56
97
4
83
5
35
48
55
20
98
6
58
17
24
27
29
96
66
99
68
63
100
9
87
64
31
32
79
72
2
67
1
49
53
77
26
36
57
103
82
3
71
12
25
101
227.03
26.98
121.8
39.95
74.92
137.3
9.012
209.0
10.81
79.90
112.4
132.9
40.08
12.01
140.1
35.45
52.00
58.93
63.54
162.5
167.3
152.0
19.00
157.3
69.72
72.59
197.0
178.5
4.002
164.9
1.008
114.8
126.9
192.2
55.85
83.80
138.9
207.2
6.941
175.0
24.31
54.94
-
12
C = 12.00 )
Name
Symbol
Atomic
Number
mercury
molybdenum
neodymium
neon
neptunium
nickel
niobium
nitrogen
nobelium
osmium
oxygen
palladium
phosphorus
platinum
plutonium
polonium
potassium
praseodymium
promethium
protactinium
radium
radon
rhenium
rhodium
rubidium
ruthenium
samarium
scandium
selenium
silicon
silver
sodium
strontium
sulfur
tantalum
technetium
tellurium
terbium
thallium
thorium
thulium
tin
titanium
tungsten
uranium
vanadium
xenon
ytterbium
yttrium
zinc
zirconium
Hg
Mo
Nd
Ne
Np
Ni
Nb
N
No
Os
O
Pd
P
Pt
Pu
Po
K
Pr
Pm
Pa
Ra
Rn
Re
Rh
Rb
Ru
Sm
Sc
Se
Si
Ag
Na
Sr
S
Ta
Tc
Te
Tb
Tl
Th
Tm
Sn
Ti
W
U
V
Xe
Yb
Y
Zn
Zr
80
42
60
10
93
28
41
7
102
76
8
46
15
78
94
84
19
59
61
91
88
86
75
45
37
44
62
21
34
14
47
11
38
16
73
43
52
65
81
90
69
50
22
74
92
23
54
70
39
30
40
Page 8 of 10
Relative
Atomic
Mass
200.6
95.94
144.2
20.18
58.71
92.91
14.01
190.2
16.00
106.4
30.97
195.1
39.10
140.9
226.03
186.2
102.9
85.47
101.1
150.4
44.96
78.96
28.09
107.9
22.99
87.62
32.06
180.9
127.6
158.9
204.4
232.0
168.9
118.7
47.90
183.9
238.0
50.94
131.3
173.0
88.91
65.37
91.22
Symbol
Atomic number
PERIODIC TABLE OF ELEMENTS
5
B
Boron
10.81
Name
Relative atomic mass
I
II
1
2
1
Hydrogen
3
4
5
6
7
8
9
10
11
12
III
IV
V
VI
VII
VIII
13
14
15
16
17
18
H
2
Helium
1.008
3
Lithium
4.002
Li
6.941
11
Sodium
Na
4
Be
Beryllium
5
Boron
9.012
10.81
12.01
12
Mg
Magnesium
13
Al
Aluminium
14
Silicon
26.98
22.99
24.31
19
K
Potassium
20
Calcium
39.10
21
Sc
Scandium
22
Titanium
40.08
44.96
37
Rb
Rubidium
38
Sr
Strontium
39
Yttrium
85.47
87.62
55
Caesium
He
Cs
56
Barium
132.9
137.3
87
Fr
Francium
88
Radium
58–71 Lanthanide Series
90–103 Actinide Series
Ca
Ba
Ra
23
V
Vanadium
24
Cr
Chromium
25
Mn
Manganese
26
Iron
47.90
50.94
52.00
54.94
55.85
58.93
58.71
63.54
40
Zr
Zirconium
41
Nb
Niobium
42
Mo
Molybdenum
43
Tc
Technetium
44
Ru
Ruthenium
45
Rh
Rhodium
46
Pd
Palladium
47
Silver
88.91
91.22
92.91
95.94
101.1
102.9
106.4
107.9
57
La
Lanthanum
72
Hf
Hafnium
73
Ta
Tantalum
74
W
Tungsten
75
Re
Rhenium
76
Osmium
138.9
178.5
180.9
183.9
186.2
190.2
89
Ac
Actinium
104
Y
Rf
105
Db
59
Pr
Praseodymium
60
Nd
Neodymium
140.1
140.9
144.2
90
Th
Thorium
91
Pa
Protactinium
92
Uranium
58
Cerium
232.0
Ce
Ti
238.0
U
106
Sg
61
Pm
Promethium
93
Np
Neptunium
107
Bh
108
Fe
Os
27
Cobalt
77
Iridium
Co
Ir
192.2
Hs
109
Ni
28
Nickel
78
Platinum
Pt
195.1
Mt
110
29
Copper
Cu
Ag
Au
79
Gold
197.0
Uun
111
Uun
Zn
30
Zinc
31
Gallium
B
Ga
C
6
Carbon
7
Nitrogen
16
Sulfur
28.09
30.97
32.06
35.45
32
Ge
Germanium
33
Arsenic
34
Se
Selenium
35
Bromine
72.59
74.92
78.96
79.90
51
Sb
Antimony
52
Te
Tellurium
53
Iodine
121.8
127.6
126.9
84
Po
Polonium
85
Astatine
116
117
49
Indium
112.4
114.8
80
Hg
Mercury
81
Thallium
200.6
204.4
207.2
209.0
113
114
115
Uub
Sn
50
Tin
118.7
62
Sm
Samarium
63
Eu
Europium
64
Gd
Gadolinium
65
Tb
Terbium
66
Dy
Dysprosium
67
Ho
Holmium
68
Erbium
Er
150.4
152.0
157.3
158.9
162.5
164.9
167.3
94
Pu
Plutonium
95
Am
Americium
96
Cm
Curium
97
Bk
Berkelium
98
Cf
Californium
99
Es
Einsteinium
100
Fm
Fermium
9
Fluorine
16.00
48
Cd
Cadmium
112
O
15
P
Phosphorus
69.72
Tl
8
Oxygen
14.01
Si
65.37
In
N
82
Lead
Pb
83
Bismuth
Bi
19.00
S
17
Chlorine
70
Yb
Ytterbium
71
Lu
Lutetium
168.9
173.0
175.0
101
Md
Mendelevium
102
No
Nobelium
103
Lr
Lawrencium
69
Thulium
Tm
As
F
10
Neon
Ne
20.18
Cl
18
Argon
Ar
39.95
Br
36
Krypton
Kr
83.80
I
54
Xenon
Xe
131.3
At
86
Radon
118
Rn
General Periodic Trends
Atomic radii decreases
Nuclear charge increases
Cation size decreases
Anion size decreases
2
He
Ionic size increases
Nuclear charge increases
5
B
6
C
7
N
8
O
9
F
10
Ne
11
Na
12
Mg
13
Al
14
Si
15
P
16
S
17
Cl
18
Ar
19
K
20
Ca
21
Sc
22
Ti
23
V
24
Cr
25
Mn
26
Fe
27
Co
28
Ni
29
Cu
30
Zn
31
Ga
32
Ge
33
As
34
Se
35
Br
36
Kr
37
Rb
38
Sr
39
Y
40
Zr
41
Nb
42
Mo
43
Tc
44
Ru
45
Rh
46
Pd
47
Ag
48
Cd
49
In
50
Sn
51
Sb
52
Te
53
I
54
Xe
55
Cs
56
Ba
57
La
72
Hf
73
Ta
74
W
75
Re
76
Os
77
Ir
78
Pt
79
Au
80
Hg
81
Tl
82
Pb
83
Bi
84
Po
85
At
86
Rn
87
Fr
88
Ra
Shielding is constant
Ionisation energy increases
Electronegativity increases
Electronegativity decreases
4
Be
Ionisation energy decreases
3
Li
Shielding increases
Atomic radii increases
1
H