College-Test-Preparation-Princeton-Review-Cracking-the-SAT-Subject-Test-in-Chemistry-16th-Edition_-Everything-You-Need-to-Help-Score-a-Perfect-800-Princeton-Review-2017

FORMULA REFERENCE GUIDE • Heat • q = mcΔT q = Heat m = mass c = specific heat ΔT = Temperature change Spontaneity • ΔG = ΔH – TΔS ΔG < 0 means that a reaction is spontaneous at this temperature +ΔH, Low temp ΔG > 0 –ΔS, High temp –ΔH, +ΔS, Any temp ΔG < 0 –ΔH, +ΔS, Any temp +ΔS, High temp

• ΔH > 0 Endothermic • ΔH < 0 Exothermic • ΔT = kmi Freezing Point Depression & Boiling Point Depression i: whole number equaling the number of particles a substance dissolves into k: solvent constant m: molality (NOT molarity) molarity = molality = mole fraction = Ideal Gas Law • PV = nRT P = pressure in atm (or mmHg or torr) V = volume in liters n = number of moles of gas particles in the container R = the ideal gas constant T = temperature in Kelvin

To calculate the ideal gas constant, use the following formula: R = .08 Conversions • Pressure: 1 ATM = 760 torr = 760 mmHg • Energy (Heat): 1 Calorie = 1000 calories = 4000 joules • Temperature: 0°C = 273 Kelvin 25°C = 298 K Facts to Know • To find the mass of a mole of a substance, multiply the formula weight by the number of moles. • 1 mol of gas at STP occupies 22.4 L of volume. Solubility • All alkali and ammonium (NH4+) compounds are soluble. The alkali metals are included in group IA (Li+, NA+, K+, Rb+, Cs+). • All acetates (CH3COO–), chlorates (ClO3–), nitrates (NO3–), and

perchlorates (ClO4–) are soluble. • Pbn+, Hgn+, and Agn+ salts are insoluble, unless they are paired with one of the anions from the previous rule. Oxidation Rules 1. When oxygen is in a compound, its oxidation state is usually –2 (it has been reduced). One important exception is oxygen in a peroxide such as hydrogen peroxide (H2O2). In a peroxide, oxygen has an oxidation state of –1. 2. When an alkali metal (Li, Na, etc.) is involved in a compound, its oxidation state is always +1 (it’s been oxidized). 3. When an alkaline earth metal (Be, Mg, etc.) is involved in a compound, its oxidation state is +2. 4. When a halogen (F, Cl, etc.) is involved in a compound, its oxidation state is often –1. The oxidation state of fluorine in a compound is always –1. 5. When hydrogen is combined with a nonmetal, its oxidation state is +1. When hydrogen is combined with a metal, its oxidation state is –1. 6. In any compound, the sum of all oxidation states is zero. Constants • Avogadro’s number: 6 × 1023 molecules/mole Prefixes Prefixes for Organics

Meth- 1 Eth- 2 Prop- 3 But- 4 Pent- 5 Hex- 6 Hep- 7 Oct- 8 Non- 9 Dec- 10 Prefix Symbol Notation nano- n 10-9 micro- μ 10-6 milli- m 10-3 centi- c 10-2 kilo- k 10-3 mega- M 106 Electrochemistry OIL Oxidation Is Losing Electrons RIG Reduction Is Gaining Electrons AN OX

Oxidation Occurs at Anode RED CAT Reduction Occurs at Cathode • Galvanic Cell: E°cell > 0 means reaction is spontaneous and energy is released (battery). • Electrolytic Cell: E°cell < 0 means the reaction is NOT spontaneous and requires a voltage source (electro plating). Equilibrium •  Periodic Trends

Acid-Base pH = pKa + log pH = –log10[H+] pH > 7: Basic pH = 7: Neutral pH < 7: Acidic Strong Acids: HCI, HI, H2SO4, HBr, HClO4, HNO3 Strong Bases: All Group I Hydroxides

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