Honors ChemistryFinal Test Prep

General Guidelines for Study1. Be familiar with common polyatomic ions.2. Remember solubility rules (Table 6.2).3. Understand Periodic Table basics (groups, families, trends)4. Study vocabulary terms from each chapter (8-17, plus organic outline)5. Memorize key items (Ideal Gas Constant, standard molar volume, etc.).6. Rework homework, worksheet, or practice test problems as necessary.

Chapter 8 - Chemical Equations and Reactions1.Translate chemical equations into word and formula equations.2. Write balanced chemical equations from word or formula equations.3. Define and write general equations for synthesis, decomposition, single

replacement, double replacement and combustion reactions.4. Given any reaction, classify it as one of the five types of reactions.

Chapter 9 - Stoichiometry1. Distinguish between composition stoichiometry and readion stoichiometry.2. Define mole ratio and identify the mole ratio for any two substances in a chemical

reaction.3. Calculate masses/moles of products and/or reactants in mass-mass,

mole-mole, mole-mass and mass-mole reaction-stoichiometry problems.4. Define and utilize a method for calculating limiting reactant.5. Calculate the mass or moles of products, given moles/masses of reactants.6. Define theoretical yield, actual yield and percent yield.

Chapter 10 - Representative Gases - Review the general characteristics of thecommon gases (production, reactivity, uses, etc).

Chapter 11 - Physical Characteristics of Gases1. List the five assumptions of the kinetic theory of gases.2. Describe the characteristic properties of gases: fluidity, expansion, low density

and compressibility.3. Define dfffusion and effusion.

4. Describe the differences between an ideal gas and a real gas5. Know the four variables that describe the state of a gas6. Describe the relationships between these variables under various conditions (i.e.,

if pressure and number of moles are constant, what is the relationship betweentemperclture and volume?)

7. Use all gas laws in calculations with temperature and pressure conversions.

Chapter 12 - Molecular Composition of Gases1. Calculate density and molar mass of a gas at STP2. Calculate molar mass or density from the Ideal Gas Law.3. Balance chemical equations and use Gay-Lussac's law, Avagadro's principle and

the Ideal Gas Law to solve problems involving gases (stoichiometry of gases).4. Memorize the equation for kinetic energy: KE = ~ mv2.5. Define and differentiate between diffusion and effusion.6. Use Graham's Law to solve "rate of effusion" problems.

Honors ChemistryFinal Test Prep

Chapter 13 - Liquids and Solids1. Describe both liquids and solids according to the kinetic theory.2. Explain the properties of liquids and solids according to the particle model.3. Name, describe and give examples of the five changes of state.4. Explain changes of equilibrium according to Le Chatelier's Principle.5. Interpret phase diagrams.6. Explain how the molecular structure of water accounts its physical properties.

Chapter 14 - Types of Mixtures! The Solution Process1. Explain the factors that influence the rate of dissolving of a solid in a liquid.2. Define and distinguish between unsaturated, saturated and supersarturated.3. Explain the phrase "like dissolves like:4. Describe the three interactions involved in heat of solution and what causes heat to

. be absorbed or released.5. Explain how temperature and pressure affect solubility of solids in liquids and gases

in liquids (Henry's Law)..6. Define and calculate percent by mass, molarity, mo/ality and mole fraction.7. List three colligative properties and describe how each is caused.8. Solve "freezing-point depression- and "boiling-point elevation" problems.

Chapter 15 - Ions in Aqueous Solutions1. Write simple equations representing the dissociation of an ionic compound (p.442-3).2. Know molar relationships of ions dissociated from ionic compounds (443).3. Write a simple net ionic equation excluding appropriate (spectator) ions (445).4. Distinguish between strong and weak electrolytes (p.449).5. Solve "freezing-point" and "boiling-point- equations for ionic solutions (453-4).

-6. Explain why colligative property measurement prevented scientists from completelyunderstanding the ionization of particular ionic compounds (454-6).

Chapter 16 - Acids/Bases1. Explain the differences between strong and weak acids; strong and weak bases.2. Define and recognize traditional (Arrhenius), Brl7t\sted and Lewis acids and bases.3. Write the formula for conjugate base of an acid and conjugate acid of a base.4. Explain why strong acids have weak conjugate bases and strong bases have weak

conjugate acids.5. Define an amphoteric substance and give an example.7. Define acid anhydride and basic anhydride, give examples and general location of

elements that form such compounds on the Periodic Table.

Chapter 17 - Acid-Base Titration and pH1. Calculate equivalents and equivalent masses of acids and bases (17.1).2. Define and calculate normality for given solutions of acid or base (17.1).3. Describe the self-ionization (auto-ionization) of water (17.2).4. Define pH and describe the use of the pH scale (17.2).5. Perform calculations using pH values (17.2).6. Describe how an acid-base indicator functions (17.3).7. Calculate normality and molarity from titration data (17.3)