Chemistry Reference Tables
Name
Value
Standard temperature
6.022  10 23 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
g°C
g°C
for steam,
4.18 J 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
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
NCDPI Reference Tables for Chemistry (2012)
Stock No. 14155
11.3437
1.74
13.5939
660
328
649
–39
420
Page 1
Organic Substances
Name
Ethanol
(CH3CH2OH)
Glucose
(C 6H12O 6)
Density
0.7893 g/cm3
Melting Point (°C)
114
Boiling Point (°C)
79
1.56 g/cm3
146
Hexane
(C 6H14)
0.6603 g/cm3
95
69
Methane
(CH4)
0.716 g/L
182
161
98
65
Methanol (CH3OH)
Sucrose
(C12H22O11)
0.7914 g/cm3
1.58 g/cm3
86
Decomposes
Decomposes
Inorganic Substances
*Density @ STP
Melting 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/cm3
851
Decomposes
Sodium chloride
2.165 g/cm3
801
1413
Sulfur dioxide
2.92 g/L
73
10
*Water (at 4°C)
1.00 g/cm3
0
100
Name
NCDPI Reference Tables for Chemistry (2012)
Boiling Point (°C)
Page 2
Formulas
D  m
V
D = density
K  C  273
m = mass
P1V1
PV
 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
liter of solution
T = temperature
q  mC pT
M = molarity
q  mHv
n = number of moles
q  mH f
q = quantity of heat energy
pH  pOH  14
C p = 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 (2012)
Page 3
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
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
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)
Cerium
Praseodymium Neodymium
© 2011 North Carolina Department of Public Instruction
NCDPI Reference Tables for Chemistry (2012)
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
Helium
10
VIIIB
11
IB
12
IIB
Aluminum
Silicon
Phosphorus
Sulfur
Chlorine
Argon
26.98
28.09
30.97
32.07
35.45
39.95
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
207.20
208.98
(209)
(210)
(222)
110
Ds
111
Rg
112
Cn
Darmstadtium Roentgenium
Copernicium
(271)
(272)
(285)
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 (2012)
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 Reactions
Key: M = Metal
NM = Nonmetal
1.
2.
SYNTHESIS:
a. Formation of binary compound: A + B  AB
b. Metal oxide and water: MO + H2O  base
c. Nonmetal oxide and water: (NM)O + H2O  acid
DECOMPOSITION:
a. Binary compounds: AB  A + B
b. Metallic carbonates: MCO3  MO + CO2
c. Metallic hydrogen carbonates: MHCO3  MCO3 (s) + 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
5.
COMBUSTION REACTION
Hydrocarbon + oxygen  carbon dioxide + water
NCDPI Reference Tables for Chemistry (2012)
Page 6
ACTIVITY SERIES of Halogens:
NH
F2
Cl2
Br2
I2
BrO
Sb
Bi
Cu
Hg
Ag
Pt
Au
Ammonium

3

CN
C 2H3O2
(CH3COO )
ACTIVITY SERIES of Metals
Li
Rb
K
Ba
Sr
Ca
Na
Mg
Al
Mn
Zn
Cr
Fe
Cd
Co
Ni
Sn
Pb
[ H2 ]
Polyatomic Ions
+
4
Replace hydrogen
from cold water
Perchlorate
ClO3
Chlorate
ClO2
Chlorite
ClO 
IO3
Hypochlorite
MnO
Iodate

4
React with oxygen to form
oxides
NCDPI Reference Tables for Chemistry (2012)
Permanganate
NO

3
Nitrate
NO

2
Nitrite
SCN 
CO23 
Hydroxide
Hydrogen
carbonate
Hydrogen sulfate
Thiocyanate
Carbonate
Cr2O27 
Dichromate
HCO3
Replace hydrogen from
acids
Acetate
ClO 4
OH 
Replace hydrogen from
steam
Bromate
Cyanide
HSO 4
CrO
SO
2
4
2
4
Chromate
Sulfate
SO23 
Sulfite
PO34 
Phosphate
Page 7
Bohr Model for Hydrogen Atom
(measurement in nanometers)
n
n
n
n
n
=
=
=
=
=
6
5
4
3
2
n=1
UV = Ultraviolet
IR = Infrared
1282
656 434
1094
1875
IR
486
410
Visible
122 97
103
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 10–1010–1110–12 10–13
X rays
Microwaves
Infrared
Ultraviolet
Gamma
rays
Radio
waves
Shorter Wavelength
Longer Wavelength
Visible Light
Red
Orange
Yellow
Green
Blue
Violet
7.0 ´ 10 –7 6.5 ´ 10 –7 5.9 ´ 10 –7 5.7 ´ 10–7 4.9 ´ 10 –7 4.2 ´ 10 –7 4.0 ´ 10–7
NCDPI Reference Tables for Chemistry (2012)
Page 8