Chemistry Reference Tables
Name
Value
Standard temperature
6.022 × 1023 particles/mole
0.0821 L atm
mole K
L mmHg
62.4
mole K
8.314 L kPa
mole K
1.00 atm = 101.3 kPa =
760. mmHg = 760. torr
0°C or 273K
Volume of 1 mole of any gas at STP
22.4 L
Avogadro’s number
Gas constant (R)
Standard pressure
Thermodynamic Constants
Symbol
Value
Heat of fusion of water
H f (water)
334 J/g
Heat of vaporization of water
Hv (water)
2,260 J/g
J for ice, 2.02 J for steam,
g°C
g°C
J
4.18
for liquid
g°C
2.05
C p (water)
Specific heat of water
Metal
Specific Heat
J
g°C
Density
(g/cm3)
Melting Point (°C)
Aluminum
0.897
2.702
660
Copper
0.385
8.92
1083
Gold
0.129
19.31
1064
Iron
0.449
7.86
1535
Lead
0.129
Magnesium
1.023
Mercury
0.140
Nickel
0.444
8.90
1455
Titanium
0.523
4.5
1660
Zinc
0.388
7.14
420
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
11.3437
1.74
13.5939
328
649
—39
Page 1
Organic Substances
Name
Density
Melting Point (°C)
Ethanol
(CH3CH2OH)
0.7893 g/cm 3
−119
Glucose
(C6H12O6)
1.54 g/cm 3
Hexane
(C6H14)
0.6603 g/cm 3
Methane
(CH4)
0.716 g/L
Methanol
(CH3OH)
0.7914 g/cm 3
Sucrose
(C12H22O11)
1.27 g/cm 3
86
Boiling Point (°C)
79
Decompose
−95
69
−182
−164
−94
65
86
Decompose
Inorganic Substances
Name
*Density @ STP
Melting Point (°C)
Boiling Point (°C)
Chlorine
3.21 g/L
−101
−35
Hydrogen
0.0899 g/L
−259
−253
Hydrogen chloride
1.640 g/L
−115
−85
Hydrogen sulfide
1.54 g/L
−85
−61
Nitrogen
1.25 g/L
−210
−196
Nitrogen monoxide
1.34 g/L
−164
−152
Oxygen
1.43 g/L
−218
−183
Sodium carbonate
2.532 g/cm 3
851
Decomposes
Sodium chloride
2.165 g/cm 3
801
1413
Sulfur dioxide
2.92 g/L
−73
−10
*Water (at 4°C)
1.00 g/cm 3
0
100
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
Page 2
Formulas
D= m
V
D = density
K = °C + 273
m = mass
PV
PV
1 1
= 2 2
T1
T2
V = volume
Pt = P1 + P2 + P3 + ...
K = Kelvin
M1V1 = M2V2
P = pressure
PV = nRT
R = gas constant
M = moles of solute
liters of solution
T = temperature
q = mCpΔT
M = molarity
q = mHv
n = number of moles
q = mH f
q = quantity of heat energy
pH + pOH = 14
Cp = specific heat
pH = − log[H +]
Hv = heat of vaporization
pOH = − log[OH −]
H f = heat of fusion
K w = [H +][OH −] = 1 × 10−14
K w = equilibrium constant for
the ionization of water
[H +] = 10 −pH
[OH −] = 10−pOH
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
Page 3
PERIODIC TABLE
1
IA
1
H
1.008
2
IIA
3
Li
4
Be
Lithium
Beryllium
6.941
9.012
11
Na
12
Mg
Hydrogen
Sodium
Magnesium
22.99
24.31
3
IIIB
4
IVB
5
VB
6
VIB
7
VIIB
8
VIIIB
9
VIIIB
19
K
20
Ca
21
Sc
22
Ti
23
V
24
Cr
25
Mn
26
Fe
27
Co
Potassium
Calcium
Scandium
Titanium
Vanadium
Chromium
Manganese
Iron
Cobalt
39.10
40.08
44.96
47.88
50.94
51.99
54.94
55.85
58.93
37
Rb
38
Sr
39
Y
40
Zr
41
Nb
42
Mo
43
Tc
44
Ru
45
Rh
Rubidium
Strontium
Yttrium
Zirconium
Niobium
Molybdenum
Technetium
Ruthenium
Rhodium
85.47
87.62
88.91
91.22
92.91
95.94
(98)
101.07
102.91
55
Cs
56
Ba
57
La
72
Hf
73
Ta
74
W
75
Re
76
Os
77
Ir
Cesium
Barium
Lanthanum
Hafnium
Tantalum
Tungsten
Rhenium
Osmium
Iridium
132.91
137.38
138.91
178.49
180.95
183.84
186.21
190.23
192.22
87
Fr
88
Ra
89
Ac
104
Rf
105
Db
106
Sg
107
Bh
108
Hs
109
Mt
Francium
Radium
Actinium
Rutherfordium
Dubnium
Seaborgium
Bohrium
Hassium
Meitnerium
(223)
(226)
(227)
(261)
(262)
(263)
(264)
(269)
(268)
58
Ce
59
Pr
60
Nd
61
Pm
62
Sm
63
Eu
64
Gd
Cerium
Praseodymium
Neodymium
Promethium
Samarium
Europium
Gadolinium
140.12
140.91
144.24
(145)
150.36
151.96
157.25
90
Th
91
Pa
92
U
93
Np
94
Pu
95
Am
96
Cm
Thorium
Protactinium
Uranium
Neptunium
Plutonium
Americium
Curium
232.04
231.04
238.04
(237)
(244)
(243)
(247)
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
Page 4
OF THE ELEMENTS
18
VIIIA
2
He
13
IIIA
14
IVA
15
VA
16
VIA
17
VIIA
4.003
5
B
6
C
7
N
8
O
9
F
10
Ne
Boron
Carbon
Nitrogen
Oxygen
Fluorine
Neon
10.81
12.01
14.01
16.00
19.00
20.18
13
Al
14
Si
15
P
16
S
17
Cl
18
Ar
Aluminum
Silicon
Phosphorus
Sulfur
Chlorine
Argon
26.98
28.09
30.97
32.07
35.45
39.95
Helium
10
VIIIB
11
IB
12
IIB
28
Ni
29
Cu
30
Zn
31
Ga
32
Ge
33
As
34
Se
35
Br
36
Kr
Nickel
Copper
Zinc
Gallium
Germanium
Arsenic
Selenium
Bromine
Krypton
58.69
63.55
65.39
69.72
72.61
74.92
78.96
79.90
83.80
46
Pd
47
Ag
48
Cd
49
In
50
Sn
51
Sb
52
Te
53
I
54
Xe
Palladium
Silver
Cadmium
Indium
Tin
Antimony
Tellurium
Iodine
Xenon
106.42
107.87
112.41
114.82
118.71
121.76
127.60
126.90
131.29
78
Pt
79
Au
80
Hg
81
Tl
82
Pb
83
Bi
84
Po
85
At
86
Rn
Platinum
Gold
Mercury
Thallium
Lead
Bismuth
Polonium
Astatine
Radon
195.08
196.97
200.59
204.38
207.2
208.98
(209)
(210)
(222)
110
Ds
111
Rg
112
Uub
Darmstadtium
Roentgenium
Ununbium
(271)
(272)
(277)
65
Tb
66
Dy
67
Ho
68
Er
69
Tm
70
Yb
71
Lu
Terbium
Dysprosium
Holmium
Erbium
Thulium
Ytterbium
Lutetium
158.93
162.50
164.93
167.26
168.93
173.04
174.97
97
Bk
98
Cf
99
Es
100
Fm
101
Md
102
No
103
Lr
Berkelium
Californium
Einsteinium
Fermium
Mendelevium
Nobelium
Lawrencium
(247)
(251)
(252)
(257)
(258)
(254)
(262)
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
Page 5
SOLUBILITY RULES
Soluble:
• All Nitrates, Acetates, Ammonium,
and Group 1 (IA) salts
• All Chlorides, Bromides, and Iodides,
except Silver, Lead, and Mercury(I)
• All Fluorides except Group 2 (IIA),
Lead(II), and Iron(III)
• All Sulfates except Calcium,
Strontium, Barium, Mercury,
Lead(II), and Silver
Insoluble (0.10 M or greater):
• All Carbonates and Phosphates
except Group 1 (IA) and Ammonium
• All Hydroxides except Group 1 (IA),
Strontium, Barium, and
Ammonium
• All Sulfides except Group 1 (IA),
2 (IIA), and Ammonium
• All Oxides except Group 1 (IA)
Guidelines for Predicting the Products of Selected Types of Chemical Reaction
Key: M = Metal
NM = Nonmetal
1.
SYNTHESIS:
a. Formation of binary compound: A + B → AB
b. Metal oxide-water reactions: MO + H2O → base
c. Nonmetal oxide-water reactions: (NM)O + H2O → acid
2.
DECOMPOSITION:
a. Binary compounds: AB → A + B
b. Metallic carbonates: MCO3 → MO + CO2
c. Metallic hydrogen carbonates: MHCO3 → MO+ H2O(l) + CO2(g)
d. Metallic hydroxides: MOH → MO + H2O
e. Metallic chlorates: MClO3 → MCl + O2
f. Oxyacids decompose to nonmetal oxides and water: acid → (NM)O + H2O
3.
SINGLE REPLACEMENT:
a. Metal-metal replacement: A + BC → AC + B
b. Active metal replaces H from water: M + H2O → MOH + H2
c. Active metal replaces H from acid: M + HX → MX + H2
d. Halide-Halide replacement: D + BC → BD + C
4.
DOUBLE REPLACEMENT: AB + CD → AD + CB
a. Formation of a precipitate from solution
b. Acid-Base neutralization reaction
5.
COMBUSTION REACTION
Hydrocarbon + oxygen → carbon dioxide + water
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
Page 6
ACTIVITY SERIES of Halogens:
Polyatomic Ions
NH
F2
Cl2
Br2
I2
+
4
BrO
Ammonium
−
3
−
CN
C2H3O2−
Bromate
Cyanide
(CH3COO−)
Acetate
ClO4−
Perchlorate
ACTIVITY SERIES of Metals
ClO3−
Chlorate
Li
Rb
K
Ba
Sr
Ca
Na
Mg
Al
Mn
Zn
Cr
Fe
Cd
Co
Ni
Sn
Pb
[ H2 ]
Sb
Bi
Cu
Hg
Ag
Pt
Au
ClO2 −
Chlorite
ClO−
IO3 −
Hypochlorite
Replace hydrogen
from cold water
Replace hydrogen from steam
MnO
NO
−
3
Permanganate
Nitrate
NO2−
Nitrite
OH −
Hydroxide
HCO3−
Hydrogen carbonate
HSO4−
SCN −
CO32 −
Hydrogen sulfate
Thiocyanate
Carbonate
Cr2O72 −
Dichromate
CrO
Replace hydrogen from acids
Iodate
−
4
2−
4
Chromate
SO
2−
4
Sulfate
SO
2−
3
Sulfite
3−
4
Phosphate
PO
React with oxygen to form oxides
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
Page 7
Bohr Model for Hydrogen Atom
(measurement in nanometers)
n=6
n=5
n=4
n=3
n=2
n=1
UV = Ultraviolet
IR = Infrared
1282
1875
656 434
122 97
486
1094
103
410
Visible
IR
UV
Electromagnetic Spectrum
(measurement in meters)
104
103
102
101
100 10 —1 10 —2 10 —3 10 —4 10 —5 10 —6 10 —7 10 —8 10 —9 10 —10 10 —11 10 —12 10 —13
X rays
Microwaves
Infrared
Ultraviolet
Gamma
rays
Radio
waves
Shorter Wavelength
Longer Wavelength
Visible Light
Red
Orange
7.0×10—7 6.5×10—7
Yellow Green
5.9×10—7 5.7×10—7
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
Stock No. 10569
Blue
4.9×10—7
Violet
4.2×10—7
4.0×10—7
Page 8