Cheat Sheet for AP Chemistry Reference Table, Cheat Sheet of Chemistry

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NCDPI Reference Tables for Chemistry (2012) 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 g°C g°C for steam, J4.18 for liquid g°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 (2012) Page 2 Organic Substances Name Density Melting Point (°C) Boiling Point (°C) Ethanol 3 2 (CH CH OH) 30.7893 g/cm 114 79 Glucose 6 12 6 (C H O ) 31.56 g/cm 146 Decomposes Hexane 6 14 (C H ) 30.6603 g/cm 95 69 Methane 4 (CH ) 0.716 g/L 182 161 Methanol 3 (CH OH) 30.7914 g/cm 98 65 Sucrose 12 22 11 (C H O ) 31.58 g/cm 86 Decomposes 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 OF THE ELEMENTS 18 VITTA 2 13 14 15 16 17 | He ITIA IVA VA VIA VITA 4.003 5 6 7 8 9 10 B c N °o F Ne Boron Carbon Nitrogen Oxygen Fluorine Neon 10.81 12.01 14.01 16.00 19.00 20.18 13 14 15 16 17 18 Al Si P s cl Ar 1 0 1 1 1 2 Aluminum Phosphorus Sulfur Chlorine Argon VITIB. IB IIB 26.98 30.97 35.45 39.95 28 29 30 32 34 35 36 Ni Cu Zn Ga Ge Se Br Kr Nickel Copper Zinc Gallium Germanium Selenium Bromine Krypton 58.69 63.55 65.39 69.72 72.61 78.96 79.90 83.80 46 47 48 49 50 51 52 53 54 Pd Ag cd In Sn Sb Te I Xe Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon 106.42 || 107.87 || 112.41 || 114.82 |} 118.71 || 121.76 J 127.60 || 126.90 || 131.29 78 79 80 81 82 83 84 85 86 Pt Au Hg Ti Pb Bi Po At Rn Platinum Gold Mercury Thallium Lead Bismuth Polonium Astatine Radon 195.08 |} 196.97 || 200.59 |} 204.38 |] 207.20 |] 208.98 || (209) (210) (222) 110 111 112 Ds Rg Cn [Darmstadtium|| Roentgenium || Copernicium (271) || (272) |) (285) 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 (2012) Page 5 NCDPI Reference Tables for Chemistry (2012) 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 Reactions Key: M = Metal NM = Nonmetal 1. SYNTHESIS: a. Formation of binary compound: A + B  AB b. Metal oxide and water: MO + H2O  base c. Nonmetal oxide and water: (NM)O + H2O  acid 2. DECOMPOSITION: a. Binary compounds: AB  A + B b. Metallic carbonates: MCO3  MO + CO2 c. Metallic hydrogen carbonates: MHCO3  MCO3 (s) + 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 5. COMBUSTION REACTION Hydrocarbon + oxygen  carbon dioxide + water NCDPI Reference Tables for Chemistry (2012) Page 7 ACTIVITY SERIES of Halogens: 2 F 2 Cl 2 Br 2 I ACTIVITY SERIES of Metals Li Rb K Ba Sr Ca Na Mg Al Mn Zn Cr Fe Cd Co Ni Sn Pb [ 2 H ] Sb Bi Cu Hg Ag Pt Au Polyatomic Ions + 4 NH Ammonium 3 BrO Bromate CN Cyanide 2 3 2 C H O Acetate 3 (CH COO ) 4 ClO Perchlorate 3 ClO Chlorate 2 ClO Chlorite ClO Hypochlorite 3 IO Iodate 4 MnO Permanganate 3 NO Nitrate 2 NO Nitrite OH Hydroxide 3 HCO Hydrogen carbonate 4 HSO Hydrogen sulfate SCN Thiocyanate 2 3 CO  Carbonate 2 2 7 Cr O  Dichromate 2 4 CrO  Chromate 2 4 SO  Sulfate 2 3 SO  Sulfite 3 4 PO  Phosphate React with oxygen to form oxides Replace hydrogen from acids Replace hydrogen from steam Replace hydrogen from cold water