Chemistry Reference Tables
Name
6.022 ×
Avogadro’s number
Value
23
10 particles/mole
0.0821 L atm
mole K
62.4
Gas constant (R)
L mmHg
mole K
8.314 L kPa
mole K
Standard pressure
1.00 atm = 101.3 kPa =
760. mmHg = 760. torr
Standard temperature
0°C or 273K
Volume of 1 mole of
any gas at STP
22.4 L
Thermodynamic
Constants
Heat of fusion of
water
Heat of
vaporization of
water
Symbol
Value
Hf
(water)
334 J/g
Hv
(water)
2,260 J/g
J for ice,
g°C
2.02 J for steam,
g°C
4.18 J for liquid
g°C
2.05
Specific heat of
water
C p (water)
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
Page 1
Metal
Specific
Heat J
g°C
Density
3
(g/cm )
Melting Point (°C)
Aluminum
0.897
2.702
Copper
0.385
8.92
1083
Gold
0.129
19.31
1064
Iron
0.449
7.86
1535
Lead
0.129
11.3437
328
Magnesium
1.023
1.74
649
Mercury
0.140
13.5939
–39
Nickel
0.444
8.90
1455
Titanium
0.523
4.5
1660
Zinc
0.388
7.14
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
660
420
Page 2
Organic Substances
Name
Melting
Point
(°C)
Density
Boiling
Point
(°C)
Ethanol
(CH3CH2OH) 0.7893 g/cm3
Glucose
(C 6H12O 6)
Hexane
(C 6H14)
1.54 g/cm
3
−119
86
0.6603 g/cm3
79
Decompose
−95
69
−182
−164
−94
65
Methane
(CH4)
Methanol
(CH3OH)
Sucrose
(C12H22O11)
0.716 g/L
0.7914 g/cm
1.27 g/cm
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
3
3
86
Decompose
Page 3
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
Page 4
Formulas
D = m
V
D = density
K = °C + 273
m = mass
P1V1
P2V2
=
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 = mC pΔT
M = molarity
n = number of
moles
q = quantity of
heat energy
q = mHv
q = mH f
C p = specific heat
pH + pOH = 14
Hv = heat of
+
pH = − log[H ]
vaporization
−
pOH = − log[OH ]
K w = [H +][OH −] = 1 × 10
H f = heat of
fusion
K
= equilibrium
w
−14
constant for
the ionization
of water
[H +] = 10 −pH
[OH −] = 10 −pOH
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
Page 5
PERIODIC TABLE
1
IA
1
H
1.008
2
IIA
3
Li
4
Be
Hydrogen
Lithium
Beryllium
6.941
9.012
11
Na
12
Mg
24.31
3
IIIB
4
IVB
5
VB
6
VIB
7
VIIB
8
VIIIB
9
VIIIB
20
Ca
21
Sc
22
Ti
23
V
24
Cr
25
Mn
26
Fe
27
Co
Sodium
Magnesium
22.99
19
K
Potassium
Calcium
39.10
40.08
37
Rb
38
Sr
Scandium
Titanium
Vanadium
Chromium
Manganese
Iron
Cobalt
44.96
47.88
50.94
51.99
54.94
55.85
58.93
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
140.12
140.91
90
Th
91
Pa
Cerium
Praseodymium Neodymium
Promethium
Samarium
Europium
Gadolinium
144.24
(145)
150.36
151.96
157.25
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 6
OF THE ELEMENTS
18
VIIIA
10
VIIIB
11
IB
12
IIB
28
Ni
29
Cu
30
Zn
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
Helium
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
31
Ga
32
Ge
33
As
34
Se
35
Br
36
Kr
Gallium
Germanium
Arsenic
Selenium
Bromine
Krypton
65.39
69.72
72.61
74.92
78.96
79.90
83.80
48
Cd
49
In
50
Sn
Tin
51
Sb
Antimony
52
Te
Tellurium
53
I
Iodine
54
Xe
Xenon
Nickel
Copper
Zinc
58.69
63.55
46
Pd
47
Ag
Palladium
Silver
Cadmium
Indium
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
195.08
196.97
200.59
110
Ds
111
Rg
112
Uub
(271)
(272)
(277)
65
Tb
66
Dy
67
Ho
Darmstadtium Roentgenium
Thallium
Lead
Bismuth
Polonium
Astatine
Radon
204.38
207.2
208.98
(209)
(210)
(222)
68
Er
69
Tm
70
Yb
71
Lu
Ununbium
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 7
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)
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
Page 8
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
c. Metallic hydrogen carbonates:
→ MO + CO2
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 9
ACTIVITY SERIES of Halogens:
F2
Cl2
Br2
I2
ACTIVITY SERIES of Metals
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
Replace hydrogen from cold water
Replace hydrogen from steam
Replace hydrogen from acids
React with oxygen to form oxides
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
Page 10
NH+4
−
BrO3
Polyatomic Ions
CN−
C 2H3O2−
−
(CH3COO )
ClO 4−
−
ClO3
−
ClO2
ClO−
−
IO3
−
MnO 4
NO3−
−
NO2
OH−
HCO3−
−
HSO 4
SCN−
CO23 −
2−
Cr2O7
2−
CrO 4
SO24 −
2−
SO3
3−
PO 4
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
Ammonium
Bromate
Cyanide
Acetate
Perchlorate
Chlorate
Chlorite
Hypochlorite
Iodate
Permanganate
Nitrate
Nitrite
Hydroxide
Hydrogen carbonate
Hydrogen sulfate
Thiocyanate
Carbonate
Dichromate
Chromate
Sulfate
Sulfite
Phosphate
Page 11
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
1094
IR
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
Stock No. 10732
656 434
486
410
Visible
122 97
103
UV
Page 12
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
Page 13