Chemistry Reference Tables Name Value Avogadro s number 6.0 10 particles/mole 0.081 L atm mole K Gas constant (R) 6. L mmhg mole K 8.1 L kpa mole K Standard pressure Standard temperature Volume of 1 mole of any gas at STP 1.00 atm = 101. kpa = 760. mmhg = 760. torr 0 C or 7K. L Thermodynamic Constants Heat of fusion of water Heat of vaporization of water Specific heat of water Symbol H f (water) H v (water) C p (water) J/g,60 J/g Value J.05 for ice, g C J.0 for steam, g C J.18 for liquid g C NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page 1
Metal Specific Heat J g C Density (g/cm ) Melting Point ( C) Aluminum 0.897.70 660 Copper 0.85 8.9 108 Gold 0.19 19.1 106 Iron 0.9 7.86 155 Lead 0.19 11.7 8 Magnesium 1.0 1.7 69 Mercury 0.10 1.599 9 Nickel 0. 8.90 155 Titanium 0.5.5 1660 Zinc 0.88 7.1 0 NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page
Name Ethanol Organic Substances Density Melting Point ( C) (CH CH OH) 0.789 g/cm 119 Boiling Point ( C) 79 Glucose (C H O ) 6 1 6 Hexane (C H ) 6 1 1.5 g/cm 86 Decompose 0.660 g/cm 95 69 Methane (CH ) 0.716 g/l 18 16 Methanol (CH OH) Sucrose (C H O ) 1 11 0.791 g/cm 9 65 1.7 g/cm 86 Decompose NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page
NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page
D Formulas = m D = density V K = C + 7 m = mass PV T PV 1 1= V = volume 1 T P = P + P + P + K = Kelvin t MV PV 1... 1 1= MV P = pressure = nrt R = gas constant M = moles of solute T = temperature liters of solution q = mc p Δ T M = molarity q = mh v q = mh f ph + poh = 1 n = number of moles q = quantity of heat energy C p = specific heat H ph = log[ H + ] v = heat of vaporization H poh = log[ OH ] f = heat of fusion + 1 K = [ H ][ OH ] = 1 10 w + ph [H ] = 10 [OH ] = 10 poh K w = equilibrium constant for the ionization of water NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page 5
NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page 6 56 Ba Barium 17.8 55 Cs Cesium 1.91 57 La Lanthanum 18.91 7 Hf Hafnium 178.9 7 Ta Tantalum 180.95 7 W Tungsten 18.8 75 Re Rhenium 186.1 76 Os Osmium 190. 77 Ir Iridium 19. 88 Ra Radium (6) 87 Fr Francium () 89 Ac Actinium (7) 10 Rf Rutherfordium (61) 105 Db Dubnium (6) 106 Sg Seaborgium (6) 107 Bh Bohrium (6) 108 Hs Hassium (69) 109 Mt Meitnerium (68) 7 Rb Rubidium 85.7 5 Rh Rhodium 10.91 Ru Ruthenium 101.07 Tc Technetium (98) Mo Molybdenum 95.9 1 Nb Niobium 9.91 0 Zr Zirconium 91. 9 Y Yttrium 88.91 8 Sr Strontium 87.6 0 Ca Calcium 0.08 19 K Potassium 9.10 1 Sc Scandium.96 Ti Titanium 7.88 V Vanadium 50.9 Cr Chromium 51.99 5 Mn Manganese 5.9 6 Fe Iron 55.85 7 Co Cobalt 58.9 1 Mg Magnesium.1 11 Na Sodium.99 IVB 5 VB 6 VIB 7 VIIB 8 VIIIB 9 VIIIB IIIB Be Beryllium 9.01 Li Lithium 6.91 1 H Hydrogen 1.008 IIA 1 IA 91 Pa Protactinium 1.0 90 Th Thorium.0 9 U Uranium 8.0 9 Np Neptunium (7) 9 Pu Plutonium () 95 Am Americium () 96 Cm Curium (7) 59 Pr Praseodymium 10.91 58 Ce Cerium 10.1 60 Nd Neodymium 1. 61 Pm Promethium (15) 6 Sm Samarium 150.6 6 Eu Europium 151.96 6 Gd Gadolinium 157.5 PERIODIC TABLE
NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page 7 78 Pt Platinum 195.08 79 Au Gold 196.97 80 Hg Mercury 00.59 81 Tl Thallium 0.8 8 Pb Lead 07. 8 Bi Bismuth 08.98 8 Po Polonium (09) 85 At Astatine (10) 86 Rn Radon () 110 Ds Darmstadtium (71) 111 Rg Roentgenium (7) 11 Uub Ununbium (77) 8 Cd Cadmium 11.1 7 Ag Silver 107.87 6 Pd Palladium 106. 5 Xe Xenon 11.9 5 I Iodine 16.90 5 Te Tellurium 17.60 51 Sb Antimony 11.76 50 Sn Tin 118.71 9 In Indium 11.8 8 Ni Nickel 58.69 9 Cu Copper 6.55 0 Zn Zinc 65.9 1 Ga Gallium 69.7 Ge Germanium 7.61 As Arsenic 7.9 Se Selenium 78.96 5 Br Bromine 79.90 6 Kr Krypton 8.80 18 Ar Argon 9.95 17 Cl Chlorine 5.5 16 S Sulfur.07 15 P Phosphorus 0.97 1 Si Silicon 8.09 1 Al Aluminum 6.98 10 VIIIB 11 IB 1 IIB 5 B Boron 10.81 6 C Carbon 1.01 7 N Nitrogen 1.01 8 O Oxygen 16.00 9 F Fluorine 19.00 10 Ne Neon 0.18 He Helium.00 17 VIIA 1 IIIA 1 IVA 15 VA 16 VIA 18 VIIIA 97 Bk Berkelium (7) 98 Cf Californium (51) 99 Es Einsteinium (5) 100 Fm Fermium (57) 101 Md Mendelevium (58) 10 No Nobelium (5) 10 Lr Lawrencium (6) 65 Tb Terbium 158.9 66 Dy Dysprosium 16.50 67 Ho Holmium 16.9 68 Er Erbium 167.6 69 Tm Thulium 168.9 70 Yb Ytterbium 17.0 71 Lu Lutetium 17.97 OF THE ELEMENTS
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 (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), (IIA), and Ammonium All Oxides except Group 1 (IA) NCDPI Reference Tables for Chemistry (October 006 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 + H O base c. Nonmetal oxide-water reactions: (NM)O + H O acid. DECOMPOSITION: a. Binary compounds: AB A + B b. Metallic carbonates: MCO MO + CO c. Metallic hydrogen carbonates: MHCO MO+ H O (l) + CO (g) d. Metallic hydroxides: MOH MO + H O e. Metallic chlorates: MClO MCl + O f. Oxyacids decompose to nonmetal oxides and water: acid (NM)O + H O. SINGLE REPLACEMENT: a. Metal-metal replacement: A + BC AC + B b. Active metal replaces H from water: M + H O MOH + H c. Active metal replaces H from acid: M + HX MX + H 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 5. COMBUSTION REACTION Hydrocarbon + oxygen carbon dioxide + water NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page 9
ACTIVITY SERIES of Halogens: F Cl Br I ACTIVITY SERIES of Metals Li Rb K Ba Sr Ca Na Mg Al Mn Zn Cr Fe Cd Co Ni Sn Pb [ Sb Bi Cu Hg Ag Pt Au H ] 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 006 form A-v1) Page 10
+ NH BrO CN CHO (CHCOO ) ClO ClO ClO ClO IO MnO NO NO OH HCO HSO SCN CO CrO 7 CrO SO SO PO Polyatomic Ions Ammonium Bromate Cyanide Acetate Perchlorate Chlorate Chlorite Hypochlorite Iodate Permanganate Nitrate Nitrite Hydroxide Hydrogen carbonate Hydrogen sulfate Thiocyanate Carbonate Dichromate Chromate Sulfate Sulfite Phosphate NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page 11
Bohr Model for Hydrogen Atom (measurement in nanometers) n = 6 n = 5 n = n = n = n = 1 UV = Ultraviolet IR = Infrared 18 656 1 97 1875 86 109 10 10 IR Visible UV NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page 1 Stock No. 107
NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page 1