Name Avogadro’s number Value 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 22.4 L Symbol Value
Gas constant (R)
Standard pressure Standard temperature Volume of 1 mole of any gas at STP Thermodynamic Constants
Heat of fusion of water Heat of vaporization of water
H f (water) Hv (water)
334 J/g 2,260 J/g
J for ice, 2.02 J for steam, g°C g°C J for liquid 4.18 g°C 2.05
Specific heat of water
C p (water)
Metal
Specific Heat
J g°C
Density (g/cm3)
Melting Point (°C)
Aluminum Copper Gold Iron Lead Magnesium Mercury Nickel Titanium Zinc
0.897 0.385 0.129 0.449 0.129 1.023 0.140 0.444 0.523 0.388
2.702 8.92 19.31 7.86 11.3437 1.74 13.5939 8.90 4.5 7.14
660 1083 1064 1535 328 649 —39 1455 1660 420
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
Page 1
Organic Substances
Name Density Melting Point (°C) Boiling Point (°C)
Ethanol (CH3CH2OH) Glucose (C6H12O6) Hexane (C6H14) Methane (CH4) Methanol (CH3OH)
Sucrose (C12H22O11)
0.7893 g/cm 3 1.54 g/cm 3 0.6603 g/cm 3 0.716 g/L
0.7914 g/cm 3 1.27 g/cm 3
−119
79 Decompose 69
86
−95
−182
−94 86
−164
65 Decompose
Inorganic Substances
Name
*Density @ STP
Melting Point (°C)
Boiling Point (°C)
Chlorine Hydrogen Hydrogen chloride Hydrogen sulfide Nitrogen
Nitrogen monoxide
3.21 g/L 0.0899 g/L 1.640 g/L 1.54 g/L 1.25 g/L 1.34 g/L 1.43 g/L 2.532 g/cm 3 2.165 g/cm 3 2.92 g/L 1.00 g/cm 3
−101
−35
−259
−115 −85
−253
−85 −61
−210
−164 −218 851 801
−73
−196
−152 −183 Decomposes 1413 −10 100
Oxygen Sodium carbonate Sodium chloride Sulfur dioxide
*Water (at 4°C)
0
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
Page 2
Formulas
D= m V
D = density
K = °C + 273
PV1 PV 1 = 2 2 T1 T2 Pt = P1 + P2 + P3 + ... M1V1 = M2V2
PV = nRT
m = mass
V = volume
K = Kelvin
P = pressure R = gas constant T = temperature
M = moles of solute liters of solution
q = mCpΔT q = mHv q = mH f
M = molarity n = number of moles q = quantity of heat energy Cp = specific heat Hv = heat of vaporization H f = heat of fusion K w = equilibrium constant for the ionization of water
pH + pOH = 14 pH = − log[H +] pOH = − log[OH −] K w = [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 IA
1 H
Hydrogen
1.008 3 Li
Lithium
2 IIA
4 Be
Beryllium
6.941 11 Na
Sodium
9.012 12 Mg
Magnesium
22.99 19 K
Potassium
24.31 20 Ca
Calcium
3 IIIB
21 Sc
Scandium
4 IVB
22 Ti
Titanium
5 VB
23 V
Vanadium
6 VIB
24 Cr
Chromium
7 VIIB
25 Mn
Manganese
8 VIIIB
26 Fe
Iron
9 VIIIB
27 Co
Cobalt
39.10 37 Rb
Rubidium
40.08 38 Sr
Strontium
44.96 39 Y
Yttrium
47.88 40 Zr
Zirconium
50.94 41 Nb
Niobium
51.99 42 Mo
Molybdenum
54.94 43 Tc
Technetium
55.85 44 Ru
Ruthenium
58.93 45 Rh
Rhodium
85.47 55 Cs
Cesium
87.62 56 Ba
Barium
88.91 57 La
Lanthanum
91.22 72 Hf
Hafnium
92.91 73 Ta
Tantalum
95.94 74 W
Tungsten
(98) 75 Re
Rhenium
101.07 76 Os
Osmium
102.91 77 Ir
Iridium
132.91 87 Fr
Francium
137.38 88 Ra
Radium
138.91 89 Ac
Actinium
178.49 104 Rf
Rutherfordium
180.95 105 Db
Dubnium
183.84 106 Sg
Seaborgium
186.21 107 Bh
Bohrium
190.23 108 Hs
Hassium
192.22 109 Mt
Meitnerium
(223)
(226)
(227)
(261)
(262)
(263)
(264)
(269)
(268)
58 Ce
Cerium
59 Pr
Praseodymium
60 Nd
Neodymium
61 Pm
Promethium
62 Sm
Samarium
63 Eu
Europium
64 Gd
Gadolinium
140.12 90 Th
Thorium
140.91 91 Pa
Protactinium
144.24 92 U
Uranium
(145) 93 Np
Neptunium
150.36 94 Pu
Plutonium
151.96 95 Am
Americium
157.25 96 Cm
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 13 IIIA
5 B
Boron
14 IVA
6 C
Carbon
15 VA
7 N
Nitrogen
16 VIA
8 O
Oxygen
17 VIIA
9 F
Fluorine
2 He
Helium
4.003 10 Ne
Neon
10.81 13 Al
Aluminum
12.01 14 Si
Silicon
14.01 15 P
Phosphorus
16.00 16 S
Sulfur
19.00 17 Cl
Chlorine
20.18 18 Ar
Argon
10 VIIIB
28 Ni
Nickel
11 IB
29 Cu
Copper
12 IIB
30 Zn
Zinc
26.98 31 Ga
Gallium
28.09 32 Ge
Germanium
30.97 33 As
Arsenic
32.07 34 Se
Selenium
35.45 35 Br
Bromine
39.95 36 Kr
Krypton
58.69 46 Pd
Palladium
63.55 47 Ag
Silver
65.39 48 Cd
Cadmium
69.72 49 In
Indium
72.61 50 Sn
Tin
74.92 51 Sb
Antimony
78.96 52 Te
Tellurium
79.90 53 I
Iodine
83.80 54 Xe
Xenon
106.42 78 Pt
Platinum
107.87 79 Au
Gold
112.41 80 Hg
Mercury
114.82 81 Tl
Thallium
118.71 82 Pb
Lead
121.76 83 Bi
Bismuth
127.60 84 Po
Polonium
126.90 85 At
Astatine
131.29 86 Rn
Radon
195.08 110 Ds
Darmstadtium
196.97 111 Rg
Roentgenium
200.59 112 Uub
Ununbium
204.38
207.2
208.98
(209)
(210)
(222)
(271)
(272)
(277)
65 Tb
Terbium
66 Dy
Dysprosium
67 Ho
Holmium
68 Er
Erbium
69 Tm
Thulium
70 Yb
Ytterbium
71 Lu
Lutetium
158.93 97 Bk
Berkelium
162.50 98 Cf
Californium
164.93 99 Es
Einsteinium
167.26 100 Fm
Fermium
168.93 101 Md
Mendelevium
173.04 102 No
Nobelium
174.97 103 Lr
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 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 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 DOUBLE REPLACEMENT: AB + CD → AD + CB a. Formation of a precipitate from solution b. Acid-Base neutralization reaction COMBUSTION REACTION Hydrocarbon + oxygen → carbon dioxide + water
2.
3.
4.
5.
NCDPI Reference Tables for Chemistry (October 2006 form A-v1)
Page 6
ACTIVITY SERIES of Halogens: F2 Cl2 Br2 I2 NH
+ 4 − 3
Polyatomic Ions Ammonium Bromate Cyanide Acetate Perchlorate Chlorate Chlorite Hypochlorite Iodate
− 4
BrO
−
CN − C2H3O2 (CH3COO−)
− ClO4 − ClO3
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
ClO2 − ClO− IO3 −
Replace hydrogen from cold water
MnO NO
− 3 − NO2
Permanganate Nitrate Nitrite Hydroxide Hydrogen carbonate Hydrogen sulfate Thiocyanate Carbonate Dichromate Chromate Sulfate Sulfite Phosphate
OH −
− HCO3 − HSO4
Replace hydrogen from steam
SCN − 2 CO3 −
2 Cr2O7 −
CrO
Replace hydrogen from acids
2− 4
SO SO
2− 4 2− 3 3− 4
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 IR 1094
656 434 486 410 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 —10 10 —11 10 —12 10 —13 Microwaves Infrared Radio waves X rays Ultraviolet Gamma rays
Longer Wavelength Visible Light Red Orange Yellow Green Blue
Shorter Wavelength
Violet 4.2×10—7 4.0×10—7
7.0×10—7 6.5×10—7
5.9×10—7 5.7×10—7
4.9×10—7
NCDPI Reference Tables for Chemistry (October 2006 form A-v1) Stock No. 10569
Page 8
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