Table 3.1 Densities of Some Common Substances Substance Color Melting Point (°C) Boiling Point (°C) Bromine red-brown -7 59 Chlorine yellow-green -101 -34 Gold yellow 1064 2856 Iron silver 1538 2862 Mercury silvery-white -117 78 Nitrogen colorless -210 -196 Oxygen colorless -219 -183 Sodium chloride white 801 1413 Water colorless 0 100 Table 3.2 Symbols and Latin Names for Various Elements Chemical Symbol Name Latin Name Na Sodium Natrium K Potassium Kalium Fe Iron Ferrum Cu Copper Cuprum Ag Silver Argentum Sn Tin Stannum Sb Antimony Stibium Au Gold Aurum Pb Lead Plumbum Table 4.1 SI Base Units of Measurement Quantity SI Base Unit Symbol Length meter m Mass kilogram kg Time second s Temperature Kelvin K Amount of a Substance mole mol Electric Current ampere A Luminous Intensity candela cd Table 4.2 Relationships Between English and Metric Units Measurement English/Metric Relationship Length 1.00 inch = 2.54 cm Mass 1.00 slug = 14.59 kg Volume 1.00 gallon = 3.78 L Table 4.3 Common Prefixes Used in the Metric System Prefix Numerical Meaning Micro (µ) 0.000,001 Milli (m) 0.001 Centi (c) 0.01 Deci (d) 0.1 Deca or Deka (da) 10 Hecta (H) 100 Kilo (k) 1000 Mega (M) 1,000,000 Table 4.4 Derived SI Units Quantity Symbol Unit Unit Abbreviation Derivation Area A square meter m2 length × width Volume V cubic meter m3 length × width × height Density D kilograms per cubic meter kg/m3 mass / volume Concentration c moles per liter mol/L amount / volume Speed (velocity) v meters per second m/s length / time Acceleration a meters per second per second m/s2 speed / time Force F newton N mass × acceleration Energy E joule J force × length Table 4.5 Relationships Between English and Metric Units Measurement English/Metric Relationship Length 1.00 inch = 2.54 cm Mass 1.00 slug = 14.59 kg Volume 1.00 gallon = 3.78 L Table 4.6 Densities of Some Common Substances Liquids and Solids Density at 20°C (g/mL) Gases Density at 20°C (g/L) Ethanol 0.79 Hydrogen 0.084 Ice (0°C) 0.917 Helium 0.166 Water 0.998 Air 1.20 Water (4°C) 1.000 Oxygen 1.33 Aluminum 2.70 Carbon dioxide 1.83 Copper 8.92 Radon 9.23 Lead 11.35 Mercury 13.6 Gold 19.3 Table 4.7 Examples of Significant Figure Rules Number Example Number of Significant Figures 9,341 4 0.0000564 3 Zero between 2 significant figures 120.043 6 Zero at end of number of to right of decimal point 510.0 510 4 2 Nonzero Digits Zeros in front of first 1-9 digit Table 7.1 Principal Energy Levels and Sublevels Principal Energy Level Number of Possible Sublevels Possible Angular Momentum Quantum Numbers Orbital Designation by Principal Energy Level and Sublevel n=1 1 I=0 1s n=2 2 I=0 I=1 2s 2p 3 I=0 I=1 I=2 3s 3p 3d 4 I=0 I=1 I=2 I=3 4s 4p 4d 4f n=3 n=4 Table 7.2 Electron Arrangement Within Energy Levels Principal Quantum Number (n) Allowable Sublevels Number of Orbitals per Sublevel Number of Orbitals per Principal Energy Level Number of Electrons per Sublevel Number of Electrons per Principal Energy Level 1 s 1 1 2 2 s 1 2 3 2 4 8 p 3 6 s 1 2 p 3 d 5 10 s 1 2 p 3 4 9 6 18 6 16 32 d 5 10 f 7 14 Table 8.1 Element Names and Symbols (in order as they appear in the periodic table) (Homonuclear diatomic elements are in blue highlight) Name Symbol Name Symbol Name Symbol Hydrogen H Yttrium Y Iridium Ir Helium He Zirconium Zr Platinum Pt Lithium Li Niobium Nb Gold Au Beryllium Be Molybdenum Mo Mercury Hg Boron B Technetium Tc Thallium Tl Carbon C Ruthenium Ru Lead Pb Nitrogen N Rhodium Rh Bismuth Bi Oxygen O Palladium Pd Polonium Po Fluorine F Silver Ag Astatine At Neon Ne Cadmium Cd Radon Rn Sodium Na Indium In Francium Fr Magnesium Mg Tin Sn Radium Ra Aluminum Al Antimony Sb Actinium Ac Siicon Si Tellurium Te Thorium Th Phosphorus P Iodine I Protactinium Pa Sulfur S Xenon Xe Uranium U Chlorine Cl Cesium Cs Neptunium Np Argon Ar Barium Ba Putonium Pu Potassium K Lanthanum La Americium Am Calcium Ca Cerium Ce Curium Cm Scandium Sc Praseodymium Pr Berkelium Bk Titanium Ti Neodymium Nd Californium Cf Vanadium V Promethium Pm Einsteinium Es Chromium Cr Samarium Sm Fermium Fm Manganese Mn Europium Eu Mendelevium Md Iron Fe Gadolium Gd Nobelium No Cobalt Co Terbium Tb Lawrencium Lr Nickel Ni Dysprosium Dy Rutherfordium Rf Copper Cu Holmium Ho Dubnium Db Zinc Zn Erbium Er Seaborgium Sg Gallium Ga Thulium Tm Bohrium Bh Germanium Ge Ytterbium Yb Hassium Hs Arsenic As Lutetium Lu Meitnerium Mt Selenium Se Hafnium Hf Darmstadium Ds Bromine Br Tantalum Ta Roentgenium Rg Krypton Kr Tungsten W Copernicum Cn Rubiduim Rb Rhenium Re Flerovium Fl Strontium Sr Osmium Os Livrmorium Lv Table 10.1 The -ide Atom Names of Nonmentals Atom -ide Name Atom -ide Name H hydride P phosphide C carbide S sulfide N nitride Cl chloride O oxide Br bromide F fluoride I iodide Table 10.2 Examples of Molecular Compounds Formula Name Formula Name NO nitrogen monoxide N2O dinitrogen monoxide S2Cl2 disulfur dichloride Cl2O7 dichlorine heptoxide CH3OH methanol C2H5OH ethanol Table 10.3 Prefixes for Naming Covalent Compounds Prefix Meaning Prefix Meaning mono 1 hexa 6 di 2 hepta 7 tri 3 octa 8 tetra 4 nona 9 penta 5 deca 10 Table 10.4 Common Ions and Their Charges for Groups IA-8A Nonmetals Gain Valence Electrons Metals Lose Valence Electrons 1A 2A 3A 4A 5A 6A Noble Gases 7A Li+ 8A He Na+ Mg2+ K+ Ca2+ Rb+ Sr2+ Cs+ Ba2+ Al3+ C4- N3- O2- F- Ne Si4- P3- S2- Cl - Ar As3- Se2- Br - Kr I- Xe Table 10.5 Common Transition Metals That Form More Than One Positive Ion Element Possible Ions Name of Ions Chromium Cr2+, Cr3+ chromium(II), chromium(III) Iron Fe2+, Fe3+ iron(II), iron(III) Copper Cu+, Cu2+ copper(I), copper(II) Gold Au+, Au2+ gold(I), gold(II) Tin Sn2+, Sn4+ tin(II), tin(IV) Lead Pb2+, Pb4+ lead(II), lead(IV) Table 10.6 Important Polyatomic Ions Ion Name Formula Ion Name Formula ammonium NH4+ cyanide CN- hydroxide OH- carbonate CO32- chlorate ClO3- chromate CrO42- chlorite ClO2- dichromate Cr2O72- nitrate NO3- sulfate SO42- nitrite NO2- sulfite SO32- acetate C2H3O2- phosphate PO43- arsenite AsO33- arsenate AsO43- bromate BrO3- bismuthate BiO3- phosphite PO33- hydrogen phosphate HPO42- permanganate MnO4- peroxide O22- Table 10.7 Common Acids Formula Name Formula Name HCl Hydrochloric acid H2SO4 Sulfuric acid HBr Hydrobromic acid H3PO4 Phosphoric acid HF Hydrofluoric acid H2CO3 Carbonic acid HNO3 Nitric acid C2H4O2 Acetic acid Table 10.8 Naming System For Acids Anion Suffix Example Name of Acid Example -ide Chloride (Cl-) Hydro__ic acid Hydrochloric acid (HCl) -ate Sulfate (SO42-) ___ic acid Sulfuric acid (H2SO4) -ite Nitrite (NO2-) ___ous acid Nitrous acid (HNO2) Table 12.1 Intermolecular Forces and Boiling Points Substance Strongest Intermolecular Force Boiling Point (°C) H2 dispersion -253 Ne dispersion -246 O2 dispersion -183 Cl2 dispersion -34 HCl dipole-dipole -85 HBr dipole-dipole -66 H2S dipole-dipole -61 NH3 hydrogen bonding -33 HF hydrogen bonding 20 H2O hydrogen bonding 100 Table 15.1 Activity Series Activities of Metals Activities of Halogens Li K F2 Ba Cl2 Sr React with cold water, replacing hydrogen Ca I2 Na Mg Al Zn Cr React with steam, but not cold water, replacing hydrogen Fe Cd Co Ni Sn Do not react with water. React with acids, replacing hydrogen Pb H2 Cu Hg Ag Pt Au Br2 Unreactive with water or acids Scientific Laws Boyle’s Law: PV = constant or P1V1 = P2V2 Charles’s Law 𝑉 = constant or 𝑇 𝑉1 𝑉2 𝑇1 = 𝑇2 Combined Gas Law: 𝑃𝑉 = constant or 𝑇 𝑃1𝑉1 𝑃2𝑉2 𝑇1 = 𝑇2 Dalton’s Law of Partial Pressures: 𝑃𝑇 = 𝑃1 + 𝑃2 + 𝑃3 + … or 𝑃1 = 𝑋1𝑃𝑇 Ideal Gas Law: 𝐿•𝑎𝑡𝑚 PV = nRT, where R = 0.08206 𝑚𝑜𝑙•𝐾 or 8.314 J/K•mol Equations Density (𝜌) 𝑚 𝑉 𝜌= °C = Temperature Conversions 5 9 (°F - 32) K = °C + 273.15 Heat (q) q = mc∆T Frequency (f) 𝑐 λ f= Energy (E) E = h ×f # 𝑚𝑜𝑙 #𝐿 Molarity (M) M= Dilution Equation M1V1 = M2V2 Molality (m) m= # 𝑚𝑜𝑙 𝑠𝑜𝑙𝑢𝑡𝑒 # 𝑘𝑔 𝑠𝑜𝑙𝑣𝑒𝑛𝑡 Freezing-Point Depression ∆T = -i ×Kf ×m Boiling-Point Elevation ∆T = i ×Kb ×m Pressure (P) Mole Fraction (X) 𝐹 𝐴 P= X= # 𝑚𝑜𝑙 𝑜𝑓 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑 𝑡𝑜𝑡𝑎𝑙 # 𝑚𝑜𝑙 𝑖𝑛 𝑚𝑖𝑥𝑡𝑢𝑟𝑒 Change in Enthalpy (∆H) ∆H° = ∑∆Hf°(products) - ∑∆Hf°(reactants) Change in Entropy (∆S) ∆S° = ∑∆S°(products) - ∑∆S°(reactants) Gibbs Free Energy (∆G) ∆G = ∆H - T∆S or ∆G° = ∑∆Gf°(products) - ∑∆Gf°(reactants) Reaction Rate Rate Equation Equilibrium Constant (K) De Broglie Wave Equation R= ∆ [𝑝𝑟𝑜𝑑𝑢𝑐𝑡] ∆𝑡 =- ∆ [𝑟𝑒𝑎𝑐𝑡𝑎𝑛𝑡] ∆𝑡 R = k[A]x[B]y K= 𝑐 𝑑 𝑎 𝑏 [𝐶]𝑒𝑞[𝐷]𝑒𝑞 [𝐴]𝑒𝑞[𝐵]𝑒𝑞 λ= ℎ 𝑚𝑣 Physical Constants Planck’s Constant h = 6.626 × 10-34 𝐽 𝐻𝑧 Joule 1 J = 1kg•m2/s2 Speed of Light c = 3.0 × 108 Avogadro’s Number Freezing Point Depression Constant (water) Boiling Point Elevation Constant (water) Standard Temperature and Pressure (STP) 𝑚 𝑠 6.02 × 1023 Kf = 1.86 °C/m Kb = 0.512 °C/m T = 273 K, P = 1.00 atm