Chemistry Reference Tables - Dpi

Chemistry Reference Tables

Name Value
Avogadro’s number
6.022 × 1023 particles/mole
Gas constant (R) 0.0821 L atm

Standard pressure mole K
Standard temperature 62.4 L mmHg
Volume of 1 mole of any gas at STP
mole K
8.314 L kPa

mole K
1.00 atm = 101.3 kPa =
760. mmHg = 760. torr
0°C or 273K

22.4 L

Thermodynamic Constants Symbol Value
Heat of fusion of water
Heat of vaporization of water Hf (water) 334 J/g

Specific heat of water Hv (water) 2,260 J/g
Cp (water)
2.05 J for ice, 2.02 J for steam,
g°C g°C

4.18 J for liquid
g°C

Metal Specific Heat J Density Melting Point (°C)
g°C (g/cm3)
Aluminum 2.702 660
Copper 0.897 8.92 1083
Gold 19.31 1064
Iron 0.385 7.86 1535
Lead 11.3437
Magnesium 0.129 1.74 328
Mercury 13.5939 649
Nickel 0.449 8.90 —39
Titanium 4.5 1455
Zinc 0.129 7.14 1660
420
1.023

0.140

0.444

0.523

0.388

NCDPI Reference Tables for Chemistry (October 2006 form A-v1) Page 1

Organic Substances

Name Density Melting Point (°C) Boiling Point (°C)
79
Ethanol 0.7893 g/cm3 −119
(CH3CH2OH) Decompose
1.54 g/cm3 86 69
Glucose
(C6H12O6) 0.6603 g/cm3 −95 −164
Hexane 65
0.716 g/L −182
(C6H14) Decompose
Methane 0.7914 g/cm3 −94

(CH4) 1.27 g/cm3 86
Methanol
(CH3OH)
Sucrose
(C12H22O11)

Inorganic Substances

Name *Density @ STP Melting Point (°C) Boiling Point (°C)
−35
Chlorine 3.21 g/L −101
−253
Hydrogen 0.0899 g/L −259 −85
−61
Hydrogen chloride 1.640 g/L −115
−196
Hydrogen sulfide 1.54 g/L −85 −152
−183
Nitrogen 1.25 g/L −210 Decomposes
1413
Nitrogen monoxide 1.34 g/L −164
−10
Oxygen 1.43 g/L −218 100
Sodium carbonate 2.532 g/cm3 851

Sodium chloride 2.165 g/cm3 801

Sulfur dioxide 2.92 g/L −73

*Water (at 4°C) 1.00 g/cm3 0

NCDPI Reference Tables for Chemistry (October 2006 form A-v1) Page 2

Formulas

D = m D = density
V m = mass

K = °C + 273 V = volume

P1V1 = P2V2 K = Kelvin
T1 T2 P = pressure
R = gas constant
Pt = P1 + P2 + P3 + ... T = temperature
M = molarity
M1V1 = M2V2 n = number of moles
q = quantity of heat energy
PV = nRT Cp = specific heat
Hv = heat of vaporization
M = moles of solute Hf = heat of fusion
liters of solution Kw = equilibrium constant for

q = mCpΔT the ionization of water

q = mHv

q = mHf

pH + pOH = 14

pH = − log[H +]

pOH = − log[OH −]

Kw = [H +][OH −] = 1 × 10−14

[H+] = 10−pH
[OH−] = 10−pOH

NCDPI Reference Tables for Chemistry (October 2006 form A-v1) Page 3

PERIODIC TABLE

1 2 34 5 67 8 9
IA IIA IIIB IVB VB VIB VIIB VIIIB VIIIB

1 4 21 22 23 24 25 26 27
H Be Sc Ti V Cr Mn Fe Co

Hydrogen Beryllium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt

1.008 9.012 44.96 47.88 50.94 51.99 54.94 55.85 58.93

3 12 39 40 41 42 43 44 45
Li Mg Y Zr Nb Mo Tc Ru Rh

Lithium Magnesium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium

6.941 24.31 88.91 91.22 92.91 95.94 (98) 101.07 102.91

11 20 57 72 73 74 75 76 77
Na Ca La Hf Ta W Re Os Ir

Sodium Calcium Lanthanum Hafnium Tantalum Tungsten Rhenium Osmium Iridium

22.99 40.08 138.91 178.49 180.95 183.84 186.21 190.23 192.22

19 38 89 104 105 106 107 108 109
K Sr Ac Rf Db Sg Bh Hs Mt

Potassium Strontium Actinium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium

39.10 87.62 (227) (261) (262) (263) (264) (269) (268)

37 56
Rb Ba

Rubidium Barium

85.47 137.38

55 88
Cs Ra

Cesium Radium

132.91 (226)

87
Fr

Francium

(223)

58 59 60 61 62 63 64
Ce Pr Nd Pm Sm Eu Gd

Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium

140.12 140.91 144.24 (145) 150.36 151.96 157.25

90 91 92 93 94 95 96
Th Pa U Np Pu Am 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

10 11 12 13 14 15 16 17 18
VIIIB IB IIB IIIA IVA VA VIA VIIA VIIIA

28 29 30 5 6 7 8 9 2
Ni Cu Zn B C N O F He

Nickel Copper Zinc Boron Carbon Nitrogen Oxygen Fluorine Helium

58.69 63.55 65.39 10.81 12.01 14.01 16.00 19.00 4.003

46 47 48 13 14 15 16 17 10
Pd Ag Cd Al Si P S Cl Ne

Palladium Silver Cadmium Aluminum Silicon Phosphorus Sulfur Chlorine Neon

106.42 107.87 112.41 26.98 28.09 30.97 32.07 35.45 20.18

78 79 80 31 32 33 34 35 18
Pt Au Hg Ga Ge As Se Br Ar

Platinum Gold Mercury Gallium Germanium Arsenic Selenium Bromine Argon

195.08 196.97 200.59 69.72 72.61 74.92 78.96 79.90 39.95

112 49 50 51 52 53 36
Uub In Sn Sb Te I Kr

Ununbium Indium Tin Antimony Tellurium Iodine Krypton

(277) 114.82 118.71 121.76 127.60 126.90 83.80

81 82 83 84 85 54
Tl Pb Bi Po At Xe

Thallium Lead Bismuth Polonium Astatine Xenon

204.38 207.2 208.98 (209) (210) 131.29

86
Rn

Radon

(222)

110 111
Ds Rg

Darmstadtium Roentgenium

(271) (272)

65 66 67 68 69 70 71
Tb Dy Ho Er Tm Yb Lu

Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium

158.93 162.50 164.93 167.26 168.93 173.04 174.97

97 98 99 100 101 102 103
Bk Cf Es Fm Md No 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 Insoluble (0.10 M or greater):
• All Carbonates and Phosphates
Soluble:
• All Nitrates, Acetates, Ammonium, except Group 1 (IA) and Ammonium
and Group 1 (IA) salts • All Hydroxides except Group 1 (IA),
• All Chlorides, Bromides, and Iodides,
except Silver, Lead, and Mercury(I) Strontium, Barium, and
• All Fluorides except Group 2 (IIA), Ammonium
Lead(II), and Iron(III) • All Sulfides except Group 1 (IA),
• All Sulfates except Calcium, 2 (IIA), and Ammonium
Strontium, Barium, Mercury, • All Oxides except Group 1 (IA)
Lead(II), and Silver

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

F2 NH+4 Ammonium
Cl2 BrO3− Bromate
Br2 CN− Cyanide
I2
C2H3O2− Acetate
ACTIVITY SERIES of Metals (CH3COO−)
ClO4− Perchlorate
Li ClO3− Chlorate
Rb ClO2− Chlorite
K
Ba ClO− Hypochlorite
Sr
Ca Replace hydrogen IO3− Iodate
Na from cold water MnO4− Permanganate
Mg NO3− Nitrate
Al Replace hydrogen from steam NO2− Nitrite
Mn
Zn Replace hydrogen from acids OH− Hydroxide
Cr React with oxygen to form oxides
Fe HCO3− Hydrogen carbonate
Cd HSO4− Hydrogen sulfate
Co SCN− Thiocyanate
Ni
Sn CO32− Carbonate
Pb Cr2O72 − Dichromate
[ H2 ] CrO24− Chromate
SO42− Sulfate
Sb SO32− Sulfite
Bi PO34− Phosphate
Cu
Hg
Ag
Pt
Au

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 656 434 122 97

1875 1094 486 103
IR 410 UV

Visible

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

Microwaves X rays
Ultraviolet
Infrared

Radio Gamma
waves rays

Longer Wavelength Shorter 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 (October 2006 form A-v1) Page 8
Stock No. 10569