PHYSICAL CONSTANTS AND CONVERSION FACTORS
NAME
SYMBOL
VALUE (with units)
Length
Meter
m
Nanometer
nm
o
Angstrom
A
−9
1 × 10
m
−10
1 × 10
m
Mass (m)
Kilogram
kg
Atomic Mass Units
amu or u
1.66 ´ 10
—24
g
Chemistry Reference Tables
Volume (V)
Liter
L
1 mL = 1 cm3
Pressure (P)
Standard Pressure
1 atm
1 atm = 101.3 kPa = 760. Torr
= 760. mmHg = 14.7 lb/ in2
Temperature (T)
Standard Temperature
°C
32.0°F = 0.0°C = 273.15K
Q
1 cal = 4.184 J
Energy
Heat
1 Cal = 4.184 kJ
Activation Energy
Ea
kJ/mol
Specific Heat of water (l)
Cp
4.18 J/g•°C
Specific Heat of water (g)
Cp
2.02 J/g•°C
Specific Heat of water (s)
Cp
2.05 J/g•°C
Heat of fusion of water
∆Hfus
6.01 kJ/mol or
334 J/g
Heat of vaporization
∆Hvap
of water
40.7 kJ/mol or
2260 J/g
Constants
Speed of light
c
3.00 × 108 m/s
Avogadro’s number
NA
6.022 × 10
Charge of an electron
e
1.60 × 10
Equilibrium constant
K
Rate constant
k
Reaction quotient
Q
Universal gas constant
R
23
–19
particles/mol
C
0.08206 L-atm/mol K
62.4 L mmHg/mol K
8.314 J/K mol
8.314 L kPa/mol K
1.99 cal/K mol
NCDPI Reference Tables for Chemistry (adopted 2000)
i
NAME
SYMBOL
DENSITY
BOILING MELTING
POINT (K)POINT (K)
Ammonia
Carbon Dioxide
Carbon Monoxide
Chlorine
Ethanol
Glucose
Gold
Hexane
Hydrogen
Hydrogen Chloride
Hydrogen Sulfide
Iron
Lead
Magnesium
Methane
Methanol
Nitrogen
Nitrogen(II) Oxide
Oxygen
Silver
Sodium Bicarbonate
Sodium Carbonate
Sodium Chloride
Sucrose
Sulfur Dioxide
Tin
Water
NH3
CO2
CO
Cl2
CH3CH2OH
C6H12O6
Au
C6H14
H2
HCl
H2S
Fe
Pb
Mg
CH4
CH3OH
N2
NO
O2
Ag
NaHCO3
Na2CO3
NaCl
C12H22O11
SO2
Sn
H2O
0.771 g/L@STP
1.98 g/L@STP
1.25 g/L@STP
3.21 g/L@STP
0.7893 g/cm3
1.54 g/cm3
19.31 g/cm3
0.6603 g/cm3
0.0899 g/L@STP
1.64 g/L@STP
1.54 g/L@STP
7.86 g/cm3
11.3437 g/cm3
1.74 g/cm3
0.716 g/cm3
0.7914 g/cm3
1.25 g/L@STP
1.34 g/L@STP
1.43 g/L@STP
10.5 g/cm3
2.159 g/cm3
2.532 g/cm3
2.165 g/cm3
1.27 g/cm3
2.92 g/L@STP
5.75 g/cm3
1.00 g/cm3
240
195 subl
82
238
351.5
decompose
3353
342
20
188
212
3023
2013
1380
109
338
77
121
90
2485
decompose
decompose
1686
decompose
263
2543
373
195.3
216.4
74
172.02
155.7
359
1337.43
178
13.86
158.2
187.5
1808
600.502
921.8
91
179.1
63.14
109.4
54.6
1234.93
543
1124
1074
359
200.3
504.96
273
STANDARD UNITS
Symbol
m
kg
Pa
K
mol
J
s
C
V
L
ii
Name
meter
kilogram
pascal
Kelvin
mole
joule
second
coulomb
volt
liter
Quantity
length
mass
pressure
temperature
amount of a substance
energy, work, quantity of heat
time
electric charge
electric potential
volume
NCDPI Reference Tables for Chemistry (adopted 2000)
WRITING CHEMICAL EQUATIONS
Writing correct chemical equations requires that you know how to predict products of reactions. Even with
limited experience, one can use a few guidelines to accomplish this. Seven frequently used elements naturally
occur as diatomic molecules: H2, O2, N2, F2, Cl2, Br2, I2. This is how they should always be written in a chemical
equation. States of matter should be indicated by (s), (l), or (g) and ions in aqueous solution as (aq).
General Classification of Reactions
(A, B, C, D represent elements and M represents a metal)
1. Synthesis: A + B → AB
3. Single Replacement: A + BC → AC + B
a. Reaction between hydrogen and a nonmetal
H2 ( g) + Cl2 ( g) → 2HCl ( g)
a. Metal-metal replacement
2Al (s) + 3Fe(NO3)2 (aq) → 2Al(NO3)3 (aq) + 3Fe (s)
b. Metal-Nonmetal reactions
2Na (s) + Cl2 ( g) → 2NaCl (s)
b. Active metal + water reactions
2Na (s) + 2H2O (l) → 2NaOH (aq) + H2 ( g)
c. Metal oxide-water reactions
CaO (s) + H2O (l) → Ca(OH)2 (s)
c. Metal-Acid reactions
2HCl (aq) + Mg (s) → MgCl2 (aq) + H2 ( g)
d. Nonmetal oxide-water reactions
SO2 ( g) + H2O (l) → H2SO3 (aq)
d. Halide-Halide replacement
Cl2 ( g) + 2HBr (aq) → 2HCl (aq) + Br2 (l)
2. Decomposition
4. Double Replacement:
a. Binary compounds AB-heat /electricity → A + B
2HgO (s) + heat → 2Hg (l) + O2 ( g)
a. Formation of a precipitate from solution
Pb(NO3)2 (aq) + 2KI (aq) → PbI2 (s) + 2KNO3 (aq)
b. Metallic carbonates MCO3 → MO + CO2
CaCO3 (s) + heat → CaO (s) + CO2 ( g)
b. Formation of a gas
CaCO3 (s) + 2HCl (aq) → CaCl2 (aq) + H2O (l) + CO2 ( g)
AB + CD → AD + BC
c. Metallic hydrogen carbonates MHCO3 → MO + H2O + CO2 c. Acid-Base Neutralization Reaction
2NaHCO3 (s) + heat → Na2O (s) + H2O ( g) + 2CO2 ( g)
HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)
d. Metallic hydroxides MOH → MO + H2O
2NaOH (s) + heat → Na2O (s) + H2O ( g)
e. Metallic chlorates decompose MClO3 → MCl + O2
2KClO3 (s) + heat → 2KCl (s) + 3O2 ( g)
5. Combustion Reaction
Hydrocarbon + oxygen → Carbon dioxide and water
CH4 ( g) + 2O2 ( g) → CO2 ( g) + 2H2O (l)
f. Some acids decompose to nonmetal oxides and water
H2CO3 (aq) + heat → H2O (l) + CO2 ( g)
g. Hydrate decomposition AB • xH2O → AB + xH2O
CuSO4 • 5H2O (s) + heat → CuSO4 (s) + 5H2O (l)
h. Peroxide
2H2O2 (l) + heat or catalyst → 2H2O (l) + O2 ( g)
NCDPI Reference Tables for Chemistry (adopted 2000)
iii
Bohr Model
for Hydrogen Atom
n=6
n=5
n=4
n=3
n=2
n=1
-12
10
Gamma ray
-10
10
-9
10
-8
-7
10
10
1875
1282
-6
10
-5
10
-4
10
-3
-2
10
X ray
10
-1
10
0
10
1
10
2
10
3
10
4
10
100,000
10,000
1,000
100
10
1.0
0.1
0.01
0.001
0.0001
0.00001
0.000001
0.0000001
0.00000001
0.000000001
0.0000000001
-11
10
IR
5
10
Microwaves
UV
Visible
-13
10
Visible
Electromagnetic Spectrum
0.00000000001
0.000000000001
(m)
0.0000000000001
UV
(nm)
1094
103
410 434
486
656
97
122
UV = Ultraviolet
IR = Infrared
IR
Radio waves
iv
Orange
5.9´10
Red
7.0´10 -7
Yellow
-7
Green
5.7´10 -7
Blue
4.9´10 -7
4.2´10 -7
4.0´10 -7
Violet
(m)
Longer Wavelength
Visible Light
6.5´10 -7
Shorter Wavelength
NCDPI Reference Tables for Chemistry (adopted 2000)
150
Solubility (grams of solute per 100 grams of water)
NCDPI Reference Tables for Chemistry (adopted 2000)
Solubility Curve
140
URANIUM DISINTEGRATION SERIES
gases
KI
solids
130
100
88
90
92
60
230
226
NH4Cl
NH3
Mass
222 Number
KCl
218
Na2SO4
NaCl
214
KClO3
210
20
10
0
238
234
HCl
70
30
86
KNO3
80
40
84
NaNO3
90
50
82
Pb Bi Po At Rn Fr Ra Ac Th Pa U
120
110
Atomic Number and Chemical Symbol
206
SO2
10 20 30 40 50 60 70 80 90 100
Temperature (°C)
4
2 He
0e
–1
(a particle) Helium nucleus emission
(b particle) electron emission
v
vi
D = density
m = mass
m
D =
V
V = volume
K =°C + 273
K = Kelvin
V1P1
VP
= 2 2
T1
T2
T = temperature
Pt = P1 + P2 + P3 + . . .
V = volume
PV = nRT
R = universal gas constant
v = rate of effusion
mw2
v1
=
v2
M =
P = pressure
mw = molecular mass
mw1
moles of solute
liters of solution
M = molarity
n = number of moles of ions
nM1V1 = nM2V2
Q = quantity of heat
∆T = change in temperature
Q = mCp∆T
Cp = specific heat
Q = mHf
Hf = heat of fusion
Hv = heat of vaporization
m = mass
Q = mHv
c = λυ
NCDPI Reference Tables for Chemistry (adopted 2000)
c = speed of light
λ = wavelength
υ = frequency
E = energy
E = hυ
h = Planck’s constant
[ ]
K
pOH = − log[OH ]
K = [ H ][OH ] = 1 × 10
pH = − log H
+
−
+
−
w
= equilibrium constant for
the ionization of water
−14
w
0
0
Error =
Accepted value – Experimental value
× 100
Accepted value
SOLUBILITY RULES:
SOLUBLE:
All Nitrates, Acetates, Ammonium and Group I salts
All Chlorides, Bromides, and Iodides, except Silver, Lead, and Mercury(I)
All Fluorides except Group II, Lead(II), and Iron(III)
All Sulfates except Calcium, Strontium, Barium, Mercury, Lead(II), and Silver
INSOLUBLE:
All Carbonates and Phosphates except Group I and Ammonium
All Hydroxides except Group I, Strontium, and Barium
All Sulfides except Group I, II, and Ammonium
All Oxides except Group I
INSOLUBLE means a precipitate forms when equal volumes of 0.10 M solutions or
greater are mixed
ACTIVITY SERIES of METALS:
Li
Rb
K
Ba
Sr
Ca
Replace hydrogen from cold water
Na
Activity
of Halogens
Mg
F2
Al
Cl2
Mn
Br2
Zn
I2
Cr
Fe
Replace hydrogen from steam
Cd
Co
Ni
Sn
Pb
Replace hydrogen from acids
[H2]
Sb
Bi
Cu
React with oxygen to form oxides
Hg
Ag
Pt
Au
1. Any metal higher in the activity series will displace another metal in a single
displacement reaction.
2. Metals above water may react with water rather than a metal compound.
Half-Reaction
H 2 O 2 +2H +2e → 2H 2 O
+
–
PbO 2 +4H + +SO 4
2–
+ 2e – → PbSO 4 +2H 2 O
E° (V)
1.78
1.69
M nO +4H +3e → M nO 2 +2H 2 O
1.68
M nO +8H +5e → M n +4H 2 O
1.51
PbO 2 + 4H + 2e → Pb +2H 2 O
1.46
Cl 2 +2e → 2Cl
1.36
–
4
+
–
4
–
+
–
+
2+
–
–
2+
–
O 2 +4H + +4e – → 2H 2 O
1.23
Br 2 +2e → 2Br
1.09
–
–
NO 3– +4H + +3e – → NO +2H 2 O
0.96
Ag + +e – → Ag
0.80
I 2 +2e → 2I
0.54
–
–
Cu +e → Cu
+
–
0.52
O 2 +2H 2 O+4e → 4OH
–
–
Hg 2 Cl 2 +2e → 2Hg+2Cl
–
0.40
–
0.34
Cu 2+ +2e – → Cu
0.34
SO +4H +2e → H 2SO 3 +H 2 O
0.20
Cu 2+ +e – → Cu +
0.16
2H +2e → H 2
0.00
Fe +3e → Fe
–0.036
Pb +2e → Pb
–0.13
Sn +2e → Sn
–0.14
2–
4
+
+
–
–
3+
–
2+
–
–
2+
Ni 2+ +2e – → Ni
PbSO 4 +2e → Pb+SO
–
–0.23
2–
4
–0.35
Cd 2+ +2e – → Cd
–0.40
Fe +2e → Fe
–0.44
Cr 3+ +3e – → Cr
–0.73
2+
–
Zn +2e → Zn
2+
–
2H 2 O+2e → H 2 +2OH
–
M n +2e → M n
2+
Al
3+
–
+ 3e → Al
–
–0.76
–
–0.83
–1.18
–1.66
M g 2+ +2e – → M g
–2.37
Na +e → Na
–2.71
Ca 2+ +2e – → Ca
–2.76
K +e → K
–2.92
Li + +e – → Li
–3.05
+
+
–
–
NCDPI Reference Tables for Chemistry (adopted 2000)
Increasing strength as reducing agent
Standard Reduction Table
25°C
vii
viii
Rf
(261)
La
138.
89
Ac
Actinium
227.0
58
Ce
88
87
232.0
Thorium
90
Th
140.1
Cerium
104
Lanthanum
Ba
Barium
137.
Cs
Cesium
132.
Ra
Fr
Francium Radium
226.0
(223)
76
75
74
73
72
57
56
55
Sg
(263)
61
Pm
60
Nd
59
Pr
231.0
Protactnium
91
Pa
140.9
238.0
Uranium
92
U
144.2
237.0
Neptunium
93
Np
(145)
Neodymium Promethium
Seaborgium
Db
Dubnium
(262)
Rutherfordium
Praseodymium
106
105
108
(244)
Plutonium
94
Pu
150.4
Samarium
62
Sm
(243)
Americium
95
Am
152.0
Europium
63
Eu
Hs
Bh
Bohrium Hassium
(265)
(262)
107
Os
Re
W
Ta
Hf
Hafnium Tantalum Tungsten Rhenium Osmium
190.2
186.
183.8
181.0
178.
78
(247)
Curium
96
Cm
157.3
(247)
Berkelium
97
Bk
158.9
Terbium
99
Es
(252)
98
Cf
(251)
164.9
Californium Einsteinium
162.5
Holmium
67
Ho
(277)
Uub
Ununbium
112
(257)
Fermium
100
Fm
167.3
Erbium
68
Er
Tl
Hg
Mercury Thallium
204.38
200.59
Dysprosium
66
Dy
65
Tb
64
Gd
Gadolinium
(272)
Uuu
(269)
Uun
111
(266)
Mt
110
Meitnerium Ununnilium Unununium
109
Pt
Ir
Iridium Platinum
195.08
192.22
77
Au
Gold
196.96
(258)
Mendelevium
101
Md
168.9
Thulium
69
Tm
Pb
Lead
207.2
82
81
80
79
101.1
(98)
52
84
Xe
Xenon
131.3
86
I
Iodine
126.9
85
(259)
Nobelium
102
No
173.0
Ytterbium
70
Yb
(262)
Lawrencium
103
Lr
175.0
71
Lu
Lutetium
Rn
Radon
(222)
54
Kr
Krypton
83.80
53
At
Po
Bi
Bismuth Polonium Astatine
(210)
(209)
208.98
83
Te
Sb
Antimony Tellurium
127.6
121.8
Sn
Tin
118.7
In
Indium
114.8
Cd
Cadmium
112.4
95.94
Zr
Pd
Rh
Rhodium Palladium
106.4
102.9
Ag
Silver
107.9
Ru
Tc
Mo
51
50
49
48
47
46
45
44
Molybdenum Technetium Ruthenium
43
42
41
72.61
91.22
40
Ge
Nb
Niobium
92.91
39
As
Arsenic
74.92
Germanium
Ga
Gallium
69.72
Zn
Zinc
65.39
Cu
Copper
63.55
Ni
Nickel
58.69
Co
Cobalt
58.93
Fe
Iron
55.85
Zirconium
38
54.94
Mn
Manganese
Y
Sr
Rb
Rubidium Strontium Yttrium
88.91
87.62
85.47
37
Cr
V
Ti
Sc
Ca
K
Potassium Calcium Scandium Titanium Vanadium Chromium
52.00
50.94
47.88
44.96
40.08
39.10
32
31
30
29
28
27
26
Br
Se
Selenium Bromine
79.90
78.96
36
35
25
24
23
22
21
34
20
19
26.98
12
2B
11
1B
10
8B
9
8B
8
8B
30.97
33
24.31
7
7B
P
Al
Mg
6
6B
Ar
Argon
39.95
Cl
Chlorine
35.45
S
Sulfur
32.07
Phosphorus
Si
Silicon
28.09
Aluminum
Magnesium
Na
Sodium
22.99
5
5B
18
17
16
15
14
13
12
11
4
4B
Ne
Neon
20.18
F
Fluorine
19.00
O
Oxygen
16.00
N
Nitrogen
14.01
C
Carbon
12.01
B
Boron
10.81
3
3B
10
9
8
7
6
5
4
Be
Li
Lithium Beryllium
9.012
6.941
3
17
7A
16
6A
15
5A
14
4A
13
3A
2
2A
He
Helium
4.003
18
8A
H
Hydrogen
1.008
PERIODIC TABLE OF THE ELEMENTS
2
1
1A
1
Stock No. 7952
NCDPI Reference Tables for Chemistry (adopted 2000)