APPENDIX I Elements, their Atomic Number and …

APPENDIX I

Elements, their Atomic Number and Molar Mass

Ac

Al

Am

Sb

Ar

As

At

Ba

Bk

Be

Bi

Bh

B

Br

Cd

Cs

Ca

Cf

C

Ce

Cl

Cr

Co

Cu

Cm

Db

Dy

Es

Er

Eu

Fm

F

Fr

Gd

Ga

Ge

Au

Hf

Hs

He

Ho

H

In

I

Ir

Fe

Kr

La

Lr

Pb

Li

Lu

Mg

Mn

Mt

Md

89

13

95

51

18

33

85

56

97

4

83

107

5

35

48

55

20

98

6

58

17

24

27

29

96

105

66

99

68

63

100

9

87

64

31

32

79

72

108

2

67

1

49

53

77

26

36

57

103

82

3

71

12

25

109

101

227.03

26.98

(243)

121.75

39.95

74.92

210

137.34

(247)

9.01

208.98

(264)

10.81

79.91

112.40

132.91

40.08

251.08

12.01

140.12

35.45

52.00

58.93

63.54

247.07

(263)

162.50

(252)

167.26

151.96

(257.10)

19.00

(223)

157.25

69.72

72.61

196.97

178.49

(269)

4.00

164.93

1.0079

114.82

126.90

192.2

55.85

83.80

138.91

(262.1)

207.19

6.94

174.96

24.31

54.94

(268)

258.10

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

Rutherfordium

Samarium

Scandium

Seaborgium

Selenium

Silicon

Silver

Sodium

Strontium

Sulphur

Tantalum

Technetium

Tellurium

Terbium

Thallium

Thorium

Thulium

Tin

Titanium

Tungsten

Ununbium

Ununnilium

Unununium

Uranium

Vanadium

Xenon

Ytterbium

Yttrium

Zinc

Zirconium

Symbol

Atomic

Number

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

Rf

Sm

Sc

Sg

Se

Si

Ag

Na

Sr

S

Ta

Tc

Te

Tb

Tl

Th

Tm

Sn

Ti

W

Uub

Uun

Uuu

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

104

62

21

106

34

14

47

11

38

16

73

43

52

65

81

90

69

50

22

74

112

110

111

92

23

54

70

39

30

40

Molar

mass/

(g mol¨C1)

200.59

95.94

144.24

20.18

(237.05)

58.71

92.91

14.0067

(259)

190.2

16.00

106.4

30.97

195.09

(244)

210

39.10

140.91

(145)

231.04

(226)

(222)

186.2

102.91

85.47

101.07

(261)

150.35

44.96

(266)

78.96

28.08

107.87

22.99

87.62

32.06

180.95

(98.91)

127.60

158.92

204.37

232.04

168.93

118.69

47.88

183.85

(277)

(269)

(272)

238.03

50.94

131.30

173.04

88.91

65.37

91.22

d

Element

he

Molar

mass/

(g mol¨C1)

is

Atomic

Number

?

no N

C

tt E

o R

be T

re

pu

Actinium

Aluminium

Americium

Antimony

Argon

Arsenic

Astatine

Barium

Berkelium

Beryllium

Bismuth

Bohrium

Boron

Bromine

Cadmium

Caesium

Calcium

Californium

Carbon

Cerium

Chlorine

Chromium

Cobalt

Copper

Curium

Dubnium

Dysprosium

Einsteinium

Erbium

Europium

Fermium

Fluorine

Francium

Gadolinium

Gallium

Germanium

Gold

Hafnium

Hassium

Helium

Holmium

Hydrogen

Indium

Iodine

Iridium

Iron

Krypton

Lanthanum

Lawrencium

Lead

Lithium

Lutetium

Magnesium

Manganese

Meitneium

Mendelevium

Symbol

bl

Element

The value given in parenthesis is the molar mass of the isotope of largest known half-life.

261

Appendix

APPENDIX II

Some Useful Conversion Factors

Common Units of Length

1 inch = 2.54 centimetres (exactly)

1 pound = 453.59 grams = 0.45359 kilogram

1 kilogram = 1000 grams = 2.205 pounds

1 gram = 10 decigrams = 100 centigrams

= 1000 milligrams

1 gram = 6.022 ¡Á 1023 atomic mass units or u

1 atomic mass unit = 1.6606 ¡Á 10¨C24 gram

1 metric tonne = 1000 kilograms

= 2205 pounds

1 mile = 5280 feet = 1.609 kilometres

1 yard = 36 inches = 0.9144 metre

1 metre = 100 centimetres = 39.37 inches

= 3.281 feet

= 1.094 yards

1 kilometre = 1000 metres = 1094 yards

= 0.6215 mile

1 Angstrom = 1.0 ¡Á 10¨C8 centimetre

= 0.10 nanometre

= 1.0 ¡Á 10¨C10 metre

= 3.937 ¡Á 10¨C9 inch

he

is

Common Units of Force* and Pressure

1 atmosphere = 760 millimetres of mercury

= 1.013 ¡Á 105 pascals

= 14.70 pounds per square inch

1 bar = 105 pascals

1 torr = 1 millimetre of mercury

1 pascal = 1 kg/ms2 = 1 N/m2

?

no N

C

tt E

o R

be T

re

pu

1 litre = 1 cubic decimetre = 1000 cubic

centimetres = 0.001 cubic metre

1 millilitre = 1 cubic centimetre = 0.001 litre

= 1.056 ¡Á 10-3 quart

1 cubic foot = 28.316 litres = 29.902 quarts

= 7.475 gallons

bl

Common Unit of Volume

1 quart = 0.9463 litre

1 litre = 1.056 quarts

d

Common Unit of Mass and Weight

1 pound = 453.59 grams

Common Units of Energy

1 joule = 1 ¡Á 107 ergs

1 thermochemical calorie**

= 4.184 joules

= 4.184 ¡Á 107 ergs

= 4.129 ¡Á 10¨C2 litre-atmospheres

= 2.612 ¡Á 1019 electron volts

1 ergs = 1 ¡Á 10¨C7 joule = 2.3901 ¡Á 10¨C8 calorie

1 electron volt = 1.6022 ¡Á 10¨C19 joule

= 1.6022 ¡Á 10¨C12 erg

= 96.487 kJ/mol?

1 litre-atmosphere = 24.217 calories

= 101.32 joules

= 1.0132 ¡Á109 ergs

1 British thermal unit = 1055.06 joules

= 1.05506 ¡Á1010 ergs

= 252.2 calories

Temperature

SI Base Unit: Kelvin (K)

K = -273.15¡ãC

K = ¡ãC + 273.15

¡ãF = 1.8(¡ãC) + 32

¡ãC =

¡ãF ? 32

1.8

Force: 1 newton (N) = 1 kg m/s 2 , i.e.,the force that, when applied for 1 second, gives a

1-kilogram mass a velocity of 1 metre per second.

** The amount of heat required to raise the temperature of one gram of water from 14.50C to 15.50C.

? Note that the other units are per particle and must be multiplied by 6.022 ¡Á1023 to be strictly

comparable.

*

Chemistry 262

APPENDIX III

Standard potentials at 298 K in electrochemical order

E? /V

Reduction half-reaction

E? /V

H4XeO6 + 2H+ + 2e¨C ?¡ú XeO3 + 3H2O

F2 + 2e¨C ?¡ú 2F¨C

O3 + 2H+ + 2e¨C ?¡ú O2 + H2O

2¨C

2¨C

S2O8 + 2e¨C ?¡ú 2SO4

Ag+ + e¨C ?¡ú Ag+

Co3+ + e¨C ?¡ú Co2+

H2O2 + 2H+ + 2e¨C ?¡ú 2H2O

Au+ + e¨C ?¡ú Au

Pb4+ + 2e¨C ?¡ú Pb2+

2HClO + 2H+ + 2e¨C ?¡ú Cl2 + 2H2O

Ce4+ + e¨C ?¡ú Ce3+

2HBrO + 2H+ + 2e¨C ?¡ú Br2 + 2H2O

¨C

MnO4 + 8H+ + 5e¨C ?¡ú Mn2+ + 4H2O

Mn3+ + e¨C ?¡ú Mn2+

Au3+ + 3e¨C ?¡ú Au

Cl2 + 2e¨C ?¡ú 2Cl¨C

2¨C

Cr2O 7 + 14H+ + 6e¨C ?¡ú 2Cr3+ + 7H2O

O3 + H2O + 2e¨C ?¡ú O2 + 2OH¨C

O2 + 4H+ + 4e¨C ?¡ú 2H2O

ClO¨C4 + 2H+ +2e¨C ?¡ú ClO¨C3 + 2H2O

MnO2 + 4H+ + 2e¨C ?¡ú Mn2+ + 2H2O

Pt2+ + 2e¨C ?¡ú Pt

Br2 + 2e¨C ?¡ú 2Br¨C

Pu4+ + e¨C ?¡ú Pu3+

NO¨C3 + 4H+ + 3e¨C ?¡ú NO + 2H2O

2Hg2+ + 2e¨C ?¡ú Hg 2+

2

ClO¨C + H2O + 2e¨C ?¡ú Cl¨C + 2OH¨C

Hg2+ + 2e¨C ?¡ú Hg

NO¨C3 + 2H+ + e¨C ?¡ú NO2 + H2O

Ag+ + e¨C ?¡ú Ag

¨C

Hg 2+

2 +2e ?¡ú 2Hg

3+

¨C

Fe + e ?¡ú Fe2+

BrO¨C + H2O + 2e¨C ?¡ú Br¨C + 2OH¨C

Hg2SO4 +2e¨C ?¡ú 2Hg + SO42¨C

MnO42¨C + 2H2O + 2e¨C ?¡ú MnO2 + 4OH¨C

MnO¨C4 + e¨C ?¡ú MnO42¨C

I2 + 2e¨C ?¡ú 2I¨C

¨C

I3 + 2e¨C ?¡ú 3I¨C

+3.0

+2.87

+2.07

+2.05

+1.98

+1.81

+1.78

+1.69

+1.67

+1.63

+1.61

+1.60

+1.51

+1.51

+1.40

+1.36

+1.33

+1.24

+1.23

+1.23

+1.23

+1.20

+1.09

+0.97

+0.96

+0.92

+0.89

+0.86

+0.80

+0.80

+0.79

+0.77

+0.76

+0.62

+0.60

+0.56

+0.54

+0.53

Cu+ + e¨C ?¡ú Cu

NiOOH + H2O + e¨C ?¡ú Ni(OH)2 + OH¨C

Ag2CrO4 + 2e¨C ?¡ú 2Ag + CrO42¨C

O2 + 2H2O + 4e¨C ?¡ú 4OH¨C

ClO¨C4 + H2O + 2e¨C ?¡ú ClO¨C3 + 2OH¨C

[Fe(CN)6]3¨C + e¨C ?¡ú [Fe(CN)6]4¨C

Cu2+ + 2e¨C ?¡ú Cu

Hg2Cl2 + 2e¨C ?¡ú 2Hg + 2Cl¨C

AgCl + e¨C ?¡ú Ag + Cl¨C

Bi3+ + 3e¨C ?¡ú Bi

¨C

SO42 + 4H+ + 2e¨C ?¡ú H2SO3 + H2O

Cu2+ + e¨C ?¡ú Cu+

Sn4+ + 2e¨C ?¡ú Sn2+

AgBr + e¨C ?¡ú Ag + Br¨C

Ti4+ + e¨C ?¡ú Ti3+

2H+ + 2e¨C ?¡ú H2

+0.52

+0.49

+0.45

+0.40

+0.36

+0.36

+0.34

+0.27

+0.27

+0.20

+0.17

+0.16

+0.15

+0.07

0.00

0.0 by

definition

¨C0.04

¨C0.08

¨C0.13

¨C0.14

¨C0.14

¨C0.15

¨C0.23

¨C0.26

¨C0.28

¨C0.34

¨C0.34

¨C0.36

¨C0.37

¨C0.40

¨C0.40

¨C0.41

¨C0.44

¨C0.44

¨C0.48

¨C0.49

¨C0.61

¨C0.74

¨C0.76

?

no N

C

tt E

o R

be T

re

pu

bl

is

he

d

Reduction half-reaction

Fe3+ + 3e¨C ?¡ú Fe

O2 + H2O + 2e¨C ?¡ú HO¨C2 + OH¨C

Pb2+ + 2e¨C ?¡ú Pb

In+ + e¨C ?¡ú In

Sn2+ + 2e¨C ?¡ú Sn

AgI + e¨C ?¡ú Ag + I¨C

Ni2+ + 2e¨C ?¡ú Ni

V3+ + e¨C ?¡ú V2+

Co2+ + 2e¨C ?¡ú Co

In3+ + 3e¨C ?¡ú In

Tl+ + e¨C ?¡ú Tl

PbSO4 + 2e¨C ?¡ú Pb + SO2¨C

4

Ti3+ + e¨C ?¡ú Ti2+

Cd2+ + 2e¨C ?¡ú Cd

In2+ + e¨C ?¡ú In+

Cr3+ + e¨C ?¡ú Cr2+

Fe2+ + 2e¨C ?¡ú Fe

In3+ + 2e¨C ?¡ú In+

S + 2e¨C ?¡ú S2¨C

In3+ + e¨C ?¡ú In2+

U4+ + e¨C ?¡ú U3+

Cr3+ + 3e¨C ?¡ú Cr

Zn2+ + 2e¨C ?¡ú Zn

(continued)

263

Appendix

APPENDIX III CONTINUED

E? /V

Reduction half-reaction

E? /V

Cd(OH)2 + 2e¨C ?¡ú Cd + 2OH¨C

2H2O + 2e¨C ?¡ú H2 + 2OH¨C

Cr2+ + 2e¨C ?¡ú Cr

Mn2+ + 2e¨C ?¡ú Mn

V2+ + 2e¨C ?¡ú V

Ti2+ + 2e¨C ?¡ú Ti

Al3+ + 3e¨C ?¡ú Al

U3+ + 3e¨C ?¡ú U

Sc3+ + 3e¨C ?¡ú Sc

Mg2+ + 2e¨C ?¡ú Mg

Ce3+ + 3e¨C ?¡ú Ce

¨C0.81

¨C0.83

¨C0.91

¨C1.18

¨C1.19

¨C1.63

¨C1.66

¨C1.79

¨C2.09

¨C2.36

¨C2.48

La3+ + 3e¨C ?¡ú La

Na+ + e¨C ?¡ú Na

Ca2+ + 2e¨C ?¡ú Ca

Sr2+ + 2e¨C ?¡ú Sr

Ba2+ + 2e¨C ?¡ú Ba

Ra2+ + 2e¨C ?¡ú Ra

Cs+ + e¨C ?¡ú Cs

Rb+ + e¨C ?¡ú Rb

K+ +e¨C ?¡ú K

Li+ + e¨C ?¡ú Li

¨C2.52

¨C2.71

¨C2.87

¨C2.89

¨C2.91

¨C2.92

¨C2.92

¨C2.93

¨C2.93

¨C3.05

?

no N

C

tt E

o R

be T

re

pu

bl

is

he

d

Reduction half-reaction

Chemistry 264

APPENDIX IV

Logarithms

he

d

Sometimes, a numerical expression may involve multiplication, division or rational powers of large

numbers. For such calculations, logarithms are very useful. They help us in making difficult calculations

easy. In Chemistry, logarithm values are required in solving problems of chemical kinetics, thermodynamics,

electrochemistry, etc. We shall first introduce this concept, and discuss the laws, which will have to be

followed in working with logarithms, and then apply this technique to a number of problems to show

how it makes difficult calculations simple.

We know that

23 = 8, 32 = 9, 53 = 125, 70 = 1

the mth power of base a is b.

Another way of stating the same fact is

logarithm of b to base a is m.

If for a positive real number a, a ¡Ù 1

?

no N

C

tt E

o R

be T

re

pu

am = b,

bl

where b is a real number. In other words

is

In general, for a positive real number a, and a rational number m, let am = b,

we say that m is the logarithm of b to the base a.

b

We write this as lo g a = m ,

¡°log¡± being the abbreviation of the word ¡°logarithm¡±.

Thus, we have

log 2 8 = 3,

Since 2

log 3 9 = 2,

log

125

Since 3

= 3,

3

=8

2

= 9

3

= 125

0

=1

Since 5

5

log 7 1 = 0,

Since 7

Laws of Logarithms

In the following discussion, we shall take logarithms to any base a, (a > 0 and a ¡Ù 1)

First Law: loga (mn) = logam + logan

Proof: Suppose that logam = x and logan = y

Then ax= m, ay = n

Hence mn = ax.ay = ax+y

It now follows from the definition of logarithms that

loga (mn) = x + y = loga m ¨C loga n

?m?

? = loga m ¨C logan

?n?

Second Law: loga ?

Proof: Let logam = x, logan = y

265

Appendix

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