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| Text Book Contents in Brief | Text Book Objectives - Ch. 1-10 |
| Text Book Objectives - Ch. 11-20 | Text Book Objectives - Ch. 21-26 |
TEXT BOOK OBJECTIVES
| Chapter 11 | Chapter 12 | Chapter 13 | Chapter 14 | Chapter 15 |
| Chapter 16 | Chapter 17 | Chapter 18 | Chapter 19 | Chapter 20 |
11.1 Measuring Matter
Describe how a mole is used in chemistry.
Relate a mole to common counting units.
Convert moles to number of representative particles and representative particles to moles.
11.2 Mass and the Mole
Relate the mass of an atom to the mass of a mole of atoms.
Calculate the number of moles in a given mass of an element and the mass of a given number of moles of an element.
Calculate the number of moles of an element when given the number of atoms of the element.
Calculate the number of atoms of an element when given the number of moles of the element.
11.3 Moles of Compounds
Recognize the mole relationships shown by a chemical formula.
Calculate the molar mass of a compound.
Calculate the number of moles of a compound from a given mass of the compound, and the mass of a compound from a given number of moles of the compound.
Determine the number of atoms or ions in a mass of a compound.
11.4 Empirical and Molecular Formulas
Explain what is meant by the percent composition of a compound.
Determine the empirical and molecular formulas for a compound from mass percent and actual mass data.
11.5 The Formula for a Hydrate
Explain what a hydrate is and how its name reflects its composition.
Determine the formula for a hydrate from laboratory data.
12.1 What is Stoichiometry
Identify the quantitative relationships in a balanced chemical equation.
Determine the mole ratios from a balanced chemical equation.
12.2 Stoichiometric Calculations
Explain the sequence of steps used in solving stoichiometric problems
Use the steps to solve stoichiometric problems.
12.3 Limiting Reactions
Identify the limiting reactant in a chemical equation.
Identify the excess reactant in a chemical equation.
Calculate the mass of a product when the amounts of more than one reactant are given.
12.4 Percent Yield
Calculate the theoretical yield of a chemical reaction from data.
Determine the percent yield for a chemical reaction.
13.1 Gases
Use the kinetic-molecular theory to explain the behavior of gases.
Describe how mass affects the rates of diffusion and effusion.
Explain how gas pressure is measured and calculate the partial pressure of a gas.
13.2 Forces of Attraction
Describe and compare intramolecular and intermolecular forces.
Distinguish among intermolecular forces.
13.3 Liquids and solids
Apply kinetic-molecular theory to the behavior of liquids and solids
Relate properties such as viscosity, surface tension, and capillary action to intermolecular forces.
Compare the structures and properties of different types of solids.
13.4 Phase Changes
Explain how the addition and removal of energy can cause a phase change.
Interpret a phase diagram.
14.1 The Gas Laws
State Boyle’s law, Charles’s law and Gay-Lussac’s law.
Apply the three gas laws to problems involving the pressure, temperature, and volume of a gas.
14.2 The Combined Gas Laws and Avogadro’s Principle
State the relationship among temperature, volume, and pressure as the combined gas law.
Apply the combined gas law to problems involving the pressure, temperature, and volume of a gas.
Relate numbers of particles and volumes using Avogadro’s principle.
14.3 The Ideal Gas Law
Relate the amount of gas present to its pressure, temperature, and volume by using the ideal gas law.
Compare the properties of real and ideal gases.
14.4 Gas Stoichiometry
Determine volume ratios for gaseous reactants and products by using coefficients from a chemical equation.
Calculate amounts of gaseous reactants and products in a chemical reaction using the gas laws.
15.1 What are solutions?
Describe the characteristics of solutions and identify the various types.
Relate intermolecular forces and the process of solvation.
Define solubility and identify factors affecting it.
15.2 Solution Concentration
State the concentrations of solutions in different ways.
Calculate the concentrations of solutions.
15.3 Colligative Properties of Solutions
Explain the nature of colligative properties.
Describe four colligative properties of solutions.
Calculate the boiling point elevation and the freezing point depression of a solution.
15.4 Heterogeneous Mixtures
Identify the properties of suspensions and colloids.
Describe different types of colloids
Explain the electrostatic forces in colloids.
Chapter 16 Energy and Chemical Change
16.1 Energy
Explain what energy is and distinguish between potential and kinetic energy.
Relate chemical potential energy to the heat lost or gained in chemical reactions.
Calculate the amount of heat absorbed or released by a substance as its temperature changes.
16.2 Heat in Chemical Reactions and Processes
Describe how a calorimeter is used to measure energy absorbed or released.
Explain the meaning of enthalpy and enthalpy change in chemical reactions and processes.
16.3 Thermochemical Equations
Write thermochemical equations for chemical reactions and other processes.
Describe how energy is lost or gained during changes of state.
Calculate the heat absorbed or released in a chemical reaction.
16.4 Calculating Enthalpy Change
Use Hess’s law of summation of enthalpies of reaction to calculate the enthalpy change for a reaction.
Explain the basis for the table of standard enthalpies of formation.
Calculate ∆Hrxn using thermochemical equations.
Determine the enthalpy change for a reaction using standard enthalpies of formation data.
16.5 Reaction Spontaneity
Differentiate between spontaneous and nonspontaneous processes.
Explain how changes in entropy and free energy determine the spontaneity of chemical reactions and other processes.
17.1 A Model for Reaction Rates
Calculate average fates of chemical reactions from experimental data.
Relate rates of chemical reactions to collisions between reacting particles.
17.2 Factors Affecting Reaction Rates
Identify factors that affect the rates of chemical reactions.
Explain the role of a catalyst.
17.3 Reaction Rate Laws
Express the relationship between rate and concentration.
Determine reaction orders using the method of initial rates.
17.4 Instantaneous Reaction Rates and Reaction Mechanisms
Calculate instantaneous rates of chemical reactions.
Understanding that many chemical reactions occur in steps.
Relate the instantaneous rate of a complex reaction to its reaction mechanism.
Chapter 18 Chemical Equilibrium
18.1 Equilibrium: A State of Dynamic Balance
Recognize the characteristics of chemical equilibrium.
Write equilibrium expressions for systems that are at equilibrium.
Calculate equilibrium constants from concentration data.
18.2 Factors Affecting Chemical Equilibrium
Describe how various factors affect chemical equilibrium.
Explain how Le Chatelier’s principle applies to equilibrium systems.
18.3 Using Equilibrium Constants
Determine equilibrium concentrations of reactants and products.
Calculate the solubility of a compound from its solubility product constant.
Explain the common ion effect.
19.1 Acids and Bases: An Introduction
Identify the physical and chemical properties of acids and bases.
Classify solutions as acidic, basic, or neutral.
Compare the Arrhenius and Bronsted-Lowery models of acids and bases.
19.2 Strengths of Acids and Bases
Relate the strength of an acid or base to its degree of ionization.
Compare the strength of a weak acid with the strength of its conjugate base and the strength of a weak base with the strength of its conjugate acid.
Explain the relationship between the strengths of acids and bases and the values of their ionization constants.
19.3 What is pH?
Explain the meaning of pH and pOH to the ion product constant for water.
Relate pH and pOH to the ion constant for water.
Calculate the pH and pOH of aqueous solutions.
19.4 Neutralization
Write chemical equations for neutralization reactions.
Explain now neutralization reactions are used in acid-base titrations.
Compare the properties of buffered and unbuffered solutions.
20.1 Oxidation and Reduction
Describe the processes of oxidation and reduction.
Identify oxidizing and reducing agents.
Determine the oxidation number of an element in a compound.
Interpret redox reactions in terms of change in oxidation state.
20.2 Balancing Redox Equations
Relate changes in oxidation numbers to the transfer of electrons.
Use changes in oxidation number to balance redox equations.
Balance net ionic redox equations by the oxidation number method.
20.3 Half-Reactions
Recognize the interdependence of oxidation and reduction processes.
Derive oxidation and reduction half-reactions from a redox equation.
Balance redox equations by the half-reaction method.