Chemistry Reference Tables

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


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


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)


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)


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


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


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