FINAL EXAM STUDY GUIDE

Topic Text Reference
CHAPTER 9
- Know the types of bonds and their general characteristics 9.2
- Draw Lewis structures for all main group elements 9.3
- Draw Lewis structures for ionic compounds 9.4
- Use Lewis symbols to predict the formula for an ionic compound 9.4
- Know the definition of lattice energy and how it affects the energetics of formation of ionic bonds 9.4
- Construct a Born-Haber cycle for formation of crystalline solids from their elements 9.4
- Calculate the lattice energy of an ionic bond from given data 9.4
- Know factors affecting lattice energy and rank lattice energies for various formulas based on these factors 9.4
- Draw Lewis structures for covalent compounds and ions with single and multiple bonds 9.5, 9.7
- Know the concept of electronegativity (EN) and its effect on the polarity of bonds 9.6
- Rank polarity of bonds based on 9.6
- Classify bond types based on 9.6
- Determine approximate value for % ionic character of a bond from and Figure 9.10 9.6
- Know the concept of resonance and draw resonance hybrids for structures requiring them 9.8
- Assign formal charges to atoms in a structure and determine the more favored resonance 9.8
- Know the exceptions to the octet rule 9.9
- Know the relationship of bond length, bond energy and bond order 9.10, Notes
- Calculate the enthalpy of reaction from bond energies 9.10
CHAPTER 10
- Use VSEPR model to assign electron-pair geometry for molecules with 2-6 electrons 10.2
- Predict and explain the effect of lone pairs on the geometry of the molecule 10.3
- Distinguish between electron pair geometry and molecular geometry for molecules with nonbonding electrons pairs 10.3
- Know the bond angles of various shapes predicted by VSEPR 10.3
- Predict the shape of larger molecules along the interior atoms 10.4
- Distinguish between bond polarity and molecular polarity 10.5
- Predict the polarity of molecules based on their geometry 10.5
- Explain chemical bonding based on valence bond theory 10.6
- Use electron configuration and valence bond theory to explain bonding in simple 10.6
- Explain the general principles in hybridization of orbitals and characterize the differences 10.7
- Identify bonding orbitals (hybridized and standard) involved in bonding of molecules 10.7
- Distinguish between sigma and pi bonds in molecules 10.7
- Predict formation of pi bonds in molecules with hybridized orbitals 10.7
- Assign hybridization for each geometry predicted by VSEPR model 10.7
CHAPTER 11
- Distinguish between intermolecular forces and bonding forces present in molecules
- Explain why intermolecular forces are smaller in magnitude compared to bonding forces
- Classify the four types of intermolecular force and identify which substances contain each
- Predict the effect of different type of intermolecular force on the properties of substances
- Know the definition of vapor pressure and its relationship to the boiling point and volatility of a substance.
- Rank substances according to boiling point, and other properties based on their intermolecular forces.
- Explain why different molecules contain different intermolecular forces.
11.3 11.3 11.3 11.3 Notes 11.3 11.3
CHAPTER 13
- Know concentration units of molarity, molality, mass percent and mole fraction.
- Convert between mass %, molarity, molality and mole fraction.
- Know colligative properties and factors they depend on.
- Calculate boiling point elevation and freezing point depression of a solvent by addition of solute.
- Use Raoult's law to determine the vapor pressure of a solution containing a nonelectrolytes and nonvolatile solute.
- Use Raoult's law to determine the vapor pressure of a solution containing 2 volatile components.
- Use Law of partial pressures to determine the pressure and composition of vapor over an ideal solution.
- Differentiate between effects of nonelectrolyte and electrolyte solutes on properties of solutions.
- Calculate vapor pressure lowering, b.p. elevation and f.p. depression of a solution containing a strong electrolyte.
- Calculate van't Hoff factor for solutions containing strong electrolytes from given data.
13.5 13.5 13.6 13.6 13.6 12.6 13.6 13.7 13.7 13.7

SUMMARY OF EQUATIONS

The equations listed below will be provided for your use on the test.