Unformatted text preview: Exam III Review Sheet: Chapter 4: • Know all the six types of reactions (be able to identify, predict products, and whether or not the reaction will go) ‐ Double replacement – solubility rules define precipitant o Acid/Base – produces water ‐ Redox Reactions o Single replacement – activity series o Combustion o Combination o Decomposition – happens with unstable compounds and/or in the presence of heat • Be able to identify oxidation numbers in complex compounds • Be able to identify and define oxidation/reduction and oxidizing/reducing agents in redox reactions • Be able to write the total ionic and net ionic equations for double replacement, acid/base, and single replacement reactions • Define and be able to identify and define strong, weak, and non‐electrolytes Chapter 3: Parts I & II • Conservation of Mass in chemical reactions • Avogadro’s number and the mole ‐ Need to know conversion ‐ Must know how to use o Ex. How many atoms in 1.4 mole of NaCl? o Ex. How many H atoms in 2 moles of CH4 • Molar Mass ‐ define ‐ Be able to calculate ‐ Be able to use in conversions and stoichiometry o Ex. How many moles of water in 2.6 g? o Ex. How many grams of C in 4.2 moles? o Ex. How many molecules in 4.6 g of CH4? • Solutions – Define solute, solvent, and solution ‐ Measure of concentration Molarity = (moles/L) ‐ Be able to calculate: o Ex. How many grams of NaCl is needed to make 100.0 ml of 1.0 M solution Dilutions: M1V1=M2V2 o Ex. How many milliliters of 12 M sulfuric acid is needed to make 150.0 ml of 1.2 M solution • Stoichiometry: ‐ Remember to balance reactions ‐ Be able to answer stoichiometry questions. o Given ‘X’ amount of reactant, how much product will form? o Given ‘X’ amount of reactant ‘A’ and ‘Y’ amount of reactant ‘B’, how much product will form? o Which is the limiting reactant? Be able to define limiting reactant o Be able to do stoichiometry with masses and solutions! ‐ Titrations o Define end point and equivalence point o Use in calculations (i.e. standardizations) ‐ Percent Yield – be able to calculate o Define Percent yield Theoretical yield Actual yield • Percent composition – define ‐ Empirical Formula – define and be able to calculate from given mass %’s ‐ Molecular Formula – define and be able to calculate from empirical if given molar mass ‐ ...
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- 1.0 M, 2 moles, 12 m, 1.2 m, 4.6 g, 2.6 g