Chemistry 111 Exam III
2/15/16
Study Guide for Exam III Spring 05: Things to Know and Be Able to Do
Chap 9: Chemical Quantities
Use balanced chemical equation to determine relationships between moles of reactants and moles of
products (ratios from the equation). section 9.1-9.2
Calculate masses of reactants and products in chemical reactions:
grams A → mol A → mol B → grams B
1. divide by molar mass A 2. multiply by mol ratio B/A 3. multiply by molar mass B
9.3
From given amounts of reactants (moles or grams) determine the limiting reactant and predict the
theoretical yield (in g or mols) of products. 9.4
Calculate % yield from theoretical and actual yields. 9.5
Chap 11: Chemical Bonding
Understand the types of chemical bonds and their characteristics. 11.1
Electronegativity, how differences lead to polar bonds, bond polarity and dipole moments. 11.2, 11.3
Determine valence electron configurations of atoms and predict which ions (if any) will form based on
the stable electron configurations of noble gases. 11.4
Draw Lewis structures of atoms and molecules, including those with multiple bonds. (multiple bond is
treated as single bond for VSEPR!). 11.6, 11.7
VSEPR ..Predict electron pair geometry and molecular geometry. Know when they are the same and
when they differ. 11.9
Chapter 14: Solutions
Understand the concept of solubility, why certain substances dissolve in water, "like dissolves like".
Ways of expressing solution concentration. Calculate "weight percent" and "molarity".
Dilution calculations M1V1 = M2V2. Calculate any of the unknown variables.
Stoichiometry of solution reactions. Use balanced chemical equation (as in Chap 9) to determine
relationships between moles of reactants and moles of products (ratios from the equation) in solution
reactions.
Chemistry 111 Exam III
2/15/16
From given amounts of reactants (moles or grams) determine the limiting reactant and predict the
theoretical yield (in g or mols) of products. Also, from given amounts of reactants (moles or grams)
determine the limiting reactant and predict the theoretical yield (in g or mols) of products. 14.6
Do stoichiometric calculations for neutralization reactions. 14.7
Chapter 15: Acids and Bases
Know the 2 models of acid/base chemistry Arrhenius and Bronsted-Lowry. Identify conjugate acid/base
pairs. 15.1
Understand the concept of acid and base strength and how it relates to conjugate strength. 15.2
Understand the ionization of water and the ion product Kw. 15.3
Understand pH and pOH, calculate concentrations from these, and vice versa. 15.4, 15.5
Understand buffer solutions. 15.6
Important things you needed to know from Exam II and still will find useful for Exam III
Naming & formulas of compounds containing polyatomic ions. Must know nitrate NO3- ammonium NH4+
sulfate SO42- hydroxide OH- CN- cyanide phosphate PO43- carbonate CO32- bicarbonate (or
hydrogen carbonate) HCO3- permanganate MnO4- perchlorate ClO4- chlorate ClO3- chlorite ClO2hypochlorite ClONaming Acids HNO3, HCl, H2SO4, HClO4.
Writing formulas from names.
Writing and balancing chemical equations. Don't forget states!
Describing aqueous reactions. Molecular, Complete Ionic, Net Ionic equations. 7.3
Acid Base Reactions, identify acids/bases, formation of water 7.4
Molar mass. Be able to convert in any way among atoms, moles, grams. Determine the molar mass of
molecules and ionic compounds. 8.4
Important things you needed to know from Exam I and still need to know for Exam II
Use of periodic table to make predictions about properties and ionic compound formation (charges)
Chemistry 111 Exam III
2/15/16
Significant figures in numbers and calculations
Metric system and prefixes for units milli-, kilo-, etc.
Scientific notation, converting numbers to and from
Conversion factors and their use, dimensional analysis
Naming of binary ionic (metal + nonmetal) compounds, Types I & II, molecular (nonmetal + nonmetal)
compounds (Type III) Sections 5.1-5.4