NCDPI Chemistry Reference Tables (October 2006 form A-v1), Cheat Sheet of Chemistry

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NCDPI Reference Tables for Chemistry (October 2006 form A-v1) Page 1 Chemistry Reference Tables Name Value Avogadro’s number 236.022 10× particles/mole Gas constant (R) 0.0821 L atm mole K 62.4 L mmHg mole K 8.314 L kPa mole K Standard pressure 1.00 atm = 101.3 kPa = 760. mmHg = 760. torr Standard temperature 0 C or 273K° Volume of 1 mole of any gas at STP 22.4 L Thermodynamic Constants Symbol Value Heat of fusion of water fH (water) 334 J/g Heat of vaporization of water vH (water) 2,260 J/g Specific heat of water pC (water) J J2.05 for ice, 2.02 for steam, g°C g°C J4.18 for liquidg°C 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 11.3437 328 Magnesium 1.023 1.74 649 Mercury 0.140 13.5939 —39 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) Page 2 Organic Substances Name Density Melting Point (°C) Boiling Point (°C) Ethanol 3 2(CH CH OH) 30.7893 g/cm 119− 79 Glucose 6 12 6(C H O ) 31.54 g/cm 86 Decompose Hexane 6 14(C H ) 30.6603 g/cm 95− 69 Methane 4(CH ) 0.716 g/L 182− 164− Methanol 3(CH OH) 30.7914 g/cm 94− 65 Sucrose 12 22 11(C H O ) 31.27 g/cm 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 32.532 g/cm 851 Decomposes Sodium chloride 32.165 g/cm 801 1413 Sulfur dioxide 2.92 g/L 73− 10− *Water (at 4°C) 31.00 g/cm 0 100 NCDPI Reference Tables for Chemistry (October 2006 form A-v1) Page 5 78 Pt Platinum 195.08 79 Au Gold 196.97 80 Hg Mercury 200.59 81 Tl Thallium 204.38 82 Pb Lead 207.2 83 Bi Bismuth 208.98 84 Po Polonium (209) 85 At Astatine (210) 86 Rn Radon (222) 110 Ds Darmstadtium (271) 111 Rg Roentgenium (272) 112 Uub Ununbium (277) 48 Cd Cadmium 112.41 47 Ag Silver 107.87 46 Pd Palladium 106.42 54 Xe Xenon 131.29 53 I Iodine 126.90 52 Te Tellurium 127.60 51 Sb Antimony 121.76 50 Sn Tin 118.71 49 In Indium 114.82 28 Ni Nickel 58.69 29 Cu Copper 63.55 30 Zn Zinc 65.39 31 Ga Gallium 69.72 32 Ge Germanium 72.61 33 As Arsenic 74.92 34 Se Selenium 78.96 35 Br Bromine 79.90 36 Kr Krypton 83.80 18 Ar Argon 39.95 17 Cl Chlorine 35.45 16 S Sulfur 32.07 15 P Phosphorus 30.97 14 Si Silicon 28.09 13 Al Aluminum 26.98 10 VIIIB 11 IB 12 IIB 5 B Boron 10.81 6 C Carbon 12.01 7 N Nitrogen 14.01 8 O Oxygen 16.00 9 F Fluorine 19.00 10 Ne Neon 20.18 2 He Helium 4.003 17 VIIA 13 IIIA 14 IVA 15 VA 16 VIA 18 VIIIA 97 Bk Berkelium (247) 98 Cf Californium (251) 99 Es Einsteinium (252) 100 Fm Fermium (257) 101 Md Mendelevium (258) 102 No Nobelium (254) 103 Lr Lawrencium (262) 65 Tb Terbium 158.93 66 Dy Dysprosium 162.50 67 Ho Holmium 164.93 68 Er Erbium 167.26 69 Tm Thulium 168.93 70 Yb Ytterbium 173.04 71 Lu Lutetium 174.97 OF THE ELEMENTS NCDPI Reference Tables for Chemistry (October 2006 form A-v1) Page 6 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 NCDPI Reference Tables for Chemistry (October 2006 form A-v1) Page 7 ACTIVITY SERIES of Halogens: 2F 2Cl 2Br 2I ACTIVITY SERIES of Metals Li Rb K Ba Sr Ca Na Mg Al Mn Zn Cr Fe Cd Co Ni Sn Pb [ 2H ] Sb Bi Cu Hg Ag Pt Au Polyatomic Ions + 4NH Ammonium 3BrO− Bromate CN− Cyanide 2 3 2C H O− 3(CH COO )− Acetate 4ClO− Perchlorate 3ClO− Chlorate 2ClO − Chlorite ClO− Hypochlorite 3IO − Iodate 4MnO− Permanganate 3NO− Nitrate 2NO− Nitrite OH− Hydroxide 3HCO− Hydrogen carbonate 4HSO− Hydrogen sulfate SCN− Thiocyanate 2 3CO − Carbonate 2 2 7Cr O − Dichromate 2 4CrO − Chromate 2 4SO − Sulfate 2 3SO − Sulfite 3 4PO − Phosphate React with oxygen to form oxides Replace hydrogen from acids Replace hydrogen from steam Replace hydrogen from cold water