Chemistry 311 Final Exam Topic/Objective List

Chemistry 311 – Final Exam Topic/Objective List 2013

Chapter 7 and 9: Ionic and Metallic Bonding (pg 187 – 202) and Chemical Names and Formulas (pg 252-278)

Chapter 7:  Use the periodic table to determine the number of valence electrons for the representative elements  Describe the formation of cations and anions using the octet rule  Describe the formation of ionic bonds through electron transfer  Interpret the chemical formula of a formula unit  Describe the structure and properties of ionic compounds  Describe the nature of a metallic bond  Explain the composition and utility of alloys Chapter 9:  Determine the charges of ions created from the representative elements  Determine the name of transition metal ions from the number of electrons lost  Recognize and name several polyatomic anions  Name and write the formulas for binary ionic compounds and those containing polyatomic ions  Name and write the formulas for binary molecular compounds  Name and write the formulas for binary acids and oxyacids

Chapter 10: Chemical Quantities (pg 287 – 312)  Define the mole as a chemical quantity  Perform mole to particle, mole to mass and mole to volume conversions  Determine the percent composition of a compound using molar mass  Determine the empirical formula of a compound given either mass or percent by mass data  Determine the molecular formula of a compound

Chapter 11: Chemical Reactions (pg 320-344)  Identify the reactants, products and the appropriate symbols in reactions.  Write balanced equations from the given names or formulas of all reactants and products in the reaction including phase symbols.  Identify and write reactions from the pattern of 5 types: combustion (complete and incomplete), synthesis, decomposition, single replacement, and double replacement.  Predict the products of any one of the 5 types of reaction.

Chapter 12: Stoichiometry (pg 353 – 375)  Interpret balanced chemical equations in terms of interacting moles, representative particles, masses and volumes of gas.  Construct mole ratios from balanced chemical equations and  Calculate stoichiometric quantities from balanced chemical equations using units of moles, mass, particles and volume.  Identify the limiting reagent in a reaction and use it to calculate stoichiometric quantities and the amount of excess reagent.  Calculate percent yield from actual and theoretical yields. Chapter 13: State of Matter (pg 385-404)  Describe the motion of particles of a gas according to the kinetic theory  Describe how air pressure is measured with a barometer  Interpret gas pressure in terms of the kinetic theory.  Describe the relationship between kinetic energy and temperature  Describe the nature of liquids in terms of kinetic theory and intermolecular attractive forces  Explain how boiling point is related to vapor pressure and temperature  Distinguish solids from gases and liquids by organization and attractive forces.  Describe changes of state (sublimation, deposition, melting, freezing, condensation, vaporization) in terms of states of matter and whether they are endothermic or exothermic processes  Explain and identify different parts of a phase diagram

Chapter 14: The Behavior of Gases (pg 413-436)

 Explain how the kinetic theory describes the relationship between gas pressure, volume and temperature.  Demonstrate the use of Dalton’s Law  Explain Avogadro’s principle  Explain the difference between real gases and ideal gases  Perform calculations using the combined gas law and the ideal gas law (and derivatives there of), including stoichiometric calculations

Chapter 15, 16 and 19: Water and Aqueous Systems (pg 450-462), Solutions (pg 471-486) and Acids, Bases, and Salts (pg 587-590, 594-604, 605, 612-616)

Section 15.2-15.3  Define aqueous solutions in terms of solutes and solvents.  Distinguish suspensions and colloids from solutions.

Section 16.1-16.3:  Relate several factors to rate and extent of dissolving.  Describe solubility and how it is impacted by changing conditions.  Describe Henry’s Law describe  Define, and work problems involving molarity.  Solve dilutions problems.  Solve percent solution problems (m/m and m/v).

Section 19.1 (Arrhenius only), 19.2, 19.3 (no calculations) and 19.4  Note properties, names and formulas of some acids and bases.

 How does Kw help solve for pH or pOH?  Calculate pH, pOH, [H+], and [OH-]  Define and give common examples of Arrhenius acids and bases.  Write neutralization reactions.  Perform titration stoichiometry.

Chapter 17: Thermochemistry (pg 505-532)  Be able to convert between units of energy.  Be able to use the specific heat algorithm C = q / (m x T)  Perform calorimetry problem.  Interpret thermochemical equations.  Understand and solve for molar heat of combustion, fusion, etc.  Demonstrate how a heating curve show energy changes for a pure substance  Use Hess’s Law to calculate complex heats of reaction.  Calculate heat of reaction from standard heats of formation.