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Unit: Chemistry Introduction
70 Questions: 52 Multiple Choice, 2 Bimodal, 5 Numeric Response, 5 Matching, 6 Essay.
Topics:
Problem Solving in Chemistry
Scope of Chemistry
Thinking Like a Scientist
Learning Objectives:
Describe how Lavoisier transformed chemistry.
Describe the steps for solving nonnumeric problems.
Describe the steps for solving numeric problems.
Explain the role that collaboration and communication play in science.
Explain why the scope of chemistry is so vast.
Identify five traditional areas of study in chemistry.
Identify some outcomes of modern research in chemistry.
Identify the central themes of chemistry.
Identify the general approach to solving a problem.
Identify the methods involved in scientific inquiry.
Identify three general reasons to study chemistry.
Unit: Scientific Measurement
118 Questions: 86 Multiple Choice, 2 Numeric Response, 8 Matching, 14 Short Answer, 8 Essay.
Topics:
Conversion Problems
Measurements
Units of Measurement
Learning Objectives:
Evaluate accuracy and precision.
Explain what happens when a measurement is multiplied by a conversion factor.
Explain what makes metric units easy to use.
Explain why measurements must be reported to the correct number of significant figures.
Identify the kinds of problems you can solve using dimensional analysis.
Identify the temperature units scientists commonly use.
Identify what determine the density of a substance.
Write numbers in scientific notation.
Unit: Matter and Change
120 Questions: 90 Multiple Choice, 2 Bimodal, 6 Numeric Response, 12 Matching, 10 Essay.
Topics:
Chemical Reactions
Elements and Compounds
Mixtures
Properties of Matter
Learning Objectives:
Classify substances and mixtures.
Describe how the mass of the reactants and the mass of the products of a chemical reaction are related.
Describe what chemists use to represent elements and compounds.
Describe what happens during a chemical change.
Explain how elements and compounds are different.
Explain how mixtures can be classified.
Explain how mixtures can be separated.
Explain why a periodic table is useful.
Explain why all samples of a substance have the same intensive properties.
Identify four possible clues that a chemical change has taken place.
Identify physical changes.
Identify the three states of matter.
Unit: Structure of the Atom
113 Questions: 73 Multiple Choice, 4 Bimodal, 16 Numeric Response, 10 Matching, 5 Short Answer, 5 Essay.
Topics:
Defining the Atom
Distinguishing Between Atoms
Structure of the Nuclear Atom
Learning Objectives:
Calculate the atomic mass of an element.
Describe the structure of Rutherford's nuclear atom.
Explain how isotopes of an element differ.
Explain how the concept of the atom developed from Democritus to John Dalton.
Explain what makes one element different from another.
Identify instruments used to observe individual atoms.
Identify three types of subatomic particles.
Unit: Electrons
119 Questions: 82 Multiple Choice, 4 Bimodal, 6 Numeric Response, 12 Matching, 8 Short Answer, 7 Essay.
Topics:
Atomic Emission Spectra and the Quantum Mechanical Model
Electron Arrangement in Atoms
The Atomic Model
Learning Objectives:
Describe how Einstein explained the photoelectric effect.
Describe what Bohr proposed in his model of the atom.
Describe what the quantum mechanical model determines about the electrons in an atom.
Distinguish between quantum mechanics and classical mechanics.
Explain how the frequencies of light are related to changes in electron energies.
Explain how the sublevels of principal energy levels differ.
Explain what causes atomic emission spectra.
List the three rules for writing the electron configurations of elements.
Unit: The Periodic Table
109 Questions: 76 Multiple Choice, 3 Bimodal, 5 Numeric Response, 10 Matching, 10 Short Answer, 5 Essay.
Topics:
Classifying the Elements
Organizing the Elements
Periodic Trends
Learning Objectives:
Classify elements based on electron configuration.
Describe how Mendeleev organized his periodic table.
Describe how the modern periodic table is organized.
Describe periodic trends for first ionization energy, ionic radii, and electronegativity.
Describe trends among elements for atomic radii.
Explain how chemists began to organize the known elements.
Explain how ions form.
Identify three broad classes of elements.
List the types of information that can be displayed in a periodic table.
Unit: Ionic Compounds and Metals
114 Questions: 84 Multiple Choice, 2 Bimodal, 4 Numeric Response, 7 Matching, 11 Short Answer, 6 Essay.
Topics:
Bonding in Metals
Ionic Bonds and Ionic Compounds
Ions
Learning Objectives:
Describe how cations form.
Describe the nature of metallic bonding.
Describe three properties of ionic compounds.
Determine the number of valance electrons in an atom of a representative element.
Explain how anions form.
Explain how ions form.
Explain the electrical charge of an ionic compound.
Explain the importance of alloys.
Unit: Covalent Compounds
119 Questions: 84 Multiple Choice, 2 Bimodal, 10 Numeric Response, 13 Matching, 10 Essay.
Topics:
Bonding Theories
Covalent Bonding
Molecular Compounds
Polar Bonds and Molecules
Learning Objectives:
Describe how atomic and molecular orbitals are related.
Describe how coordinate covalent bonds are different from other covalent bonds.
Describe how electronegativity values determine the charge distribution in a polar molecule.
Describe how resonance structures are used.
Describe how to predict a molecule's shape.
Describe the representative units that define molecular compounds and ionic compounds.
Evaluate how the strengths of intermolecular attractions compare with the strengths of ionic and covalent bonds.
Explain how the strength of a covalent bond is related to its bond dissociation energy.
Explain the result of electron sharing in covalent bonds.
Explain why the properties of covalent compounds are so diverse.
Identify some exceptions to the octet rule.
Identify the information a molecular formula provides.
Identify the ways in which orbital hybridization is useful in describing molecules.
Unit: Chemical Names and Formulas
128 Questions: 109 Multiple Choice, 4 Numeric Response, 9 Matching, 1 Short Answer, 5 Essay.
Topics:
Names and Formulas of Acids and Bases
Names and Formulas of Ionic Compounds
Names and Formulas of Molecular Compounds
Naming Ions
The Laws Governing How Compounds Form
Learning Objectives:
Apply the rules for naming and writing formulas for binary ionic compounds.
Apply the rules for naming and writing formulas for compounds with polyatomic ions.
Describe the guidelines used to write the name and formula of a binary molecular compounds.
Determine the names and formulas of acids.
Determine the names and formulas of bases.
Explain how polyatomic ions differ from and are similar to monatomic ions.
Explain how the law of definite proportions is consistent with Dalton's atomic theory.
Explain how to determine the charges of monatomic ions.
List the general guidelines that can help you write the name and formula of a chemical compound.
Unit: The Mole
118 Questions: 92 Multiple Choice, 5 Bimodal, 9 Matching, 7 Short Answer, 5 Essay.
Topics:
Mole-Mass and Mole-Volume Relationships
Percent Composition and Chemical Formulas
The Mole: A Measurement of Matter
Learning Objectives:
Calculate the empirical formula of a compound.
Calculate the percent composition of a compound.
Compare the molecular formula of a compound with the empirical formula.
Convert among the count, mass, and volume of something.
Convert the volume of a gas at STP to the number of moles of the gas.
Describe how to convert the mass of a substance to the number of moles of a substance.
Explain how chemists count the number of atoms, molecules, or formula units in a substance.
Explain how you use the mole concept to determine the molar mass of an element and a compound.
Unit: Chemical Reactions
116 Questions: 85 Multiple Choice, 4 Bimodal, 9 Matching, 12 Short Answer, 6 Essay.
Topics:
Describing Chemical Reactions
Reactions in Aqueous Solution
Types of Chemical Reactions
Learning Objectives:
Describe how to write a skeleton equation.
Describe the five general types of reactions.
Describe the information found in a net ionic equation.
Describe the steps for writing and balancing a chemical equation.
Predict the formation of a precipitate in double-replacement reaction.
Unit: Stoichiometry
102 Questions: 69 Multiple Choice, 1 Bimodal, 4 Numeric Response, 8 Matching, 11 Short Answer, 9 Essay.
Topics:
Chemical Calculations
Limiting Reagent and Percent Yield
The Arithmetic of Equations
Learning Objectives:
Describe how chemists use balanced chemical equations.
Describe the quantities you can use to interpret a balanced chemical equation.
Explain how mole ratios are used in chemical calculations.
Explain how the amount of product in a reaction is affected by an insufficient quantity of any of the reactants.
Explain the general procedure for solving a stoichiometric problem.
Explain what the percent yield of a reaction measures.
Unit: States of Matter
97 Questions: 68 Multiple Choice, 1 Bimodal, 15 Matching, 6 Short Answer, 7 Essay.
Topics:
Changes of State
Gases
Liquids
Solids
Learning Objectives:
Define the conditions under which a dynamic equilibrium can exist between a liquid and its vapor.
Define the relationship between evaporation and kinetic energy.
Describe how kinetic theory explains gas pressure.
Describe how the conditions at which phases are in equilibrium are represented on a phase diagram.
Describe how the structure and properties of a solid are related.
Describe the postulates of kinetic theory as it applies to gases.
Explain the relationship between the temperature in kelvins and the average kinetic energy of particles.
Identify the conditions necessary for sublimation.
Identify the conditions under which boiling occurs.
Identify the factors that determine the physical properties of a liquid.
Identify the factors that determine the shape of a crystal.
Unit: Gases
111 Questions: 76 Multiple Choice, 3 Bimodal, 3 Numeric Response, 10 Matching, 13 Short Answer, 6 Essay.
Topics:
Gases: Mixtures and Movements
Ideal Gases
Properties of Gases
The Gas Laws
Learning Objectives:
Calculate the volume, pressure, number of moles, and temperature for an ideal gas.
Describe and calculate the relationship among the pressure, volume, and temperature of a gas.
Determine the conditions under which real gases are most likely to differ from ideal gases.
Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses.
Relate the total pressure of a mixture of gases to the partial pressures of the component gases.
Unit: Water and Aqueous Systems
99 Questions: 71 Multiple Choice, 1 Bimodal, 4 Numeric Response, 14 Matching, 2 Short Answer, 7 Essay.
Topics:
Heterogeneous Aqueous Systems
Homogeneous Aqueous Systems
Water and Its Properties
Learning Objectives:
Describe the structure of ice.
Distinguish between a suspension and a solution.
Explain why all ionic compounds are electrolytes.
Explain why hydrates easily lose and regain water.
Identify how to distinguish a colloid from a suspension and a solution.
Identify the factor that causes the high surface tension, low vapor pressure, and high boiling point of water.
Identify the types of substances that dissolve most readily in water.
Unit: Solutions
113 Questions: 74 Multiple Choice, 3 Bimodal, 6 Numeric Response, 10 Matching, 15 Short Answer, 5 Essay.
Topics:
Calculations Involving Colligative Properties
Colligative Properties of Solutions
Concentrations of Solutions
Properties of Solutions
Learning Objectives:
Calculate the molarity of a solution.
Describe how the freezing-point depression and boiling-point elevation are related to molarity.
Describe the effect of dilution on the amount of solute.
Describe the equilibrium in a saturated solution.
Describe the factors that influence the solubility of a substance.
Distinguish percent by volume and percent by mass.
Identify the factors that influence a substance's rate of dissolution.
Identify three colligative properties of solutions.
Identify two ways of expressing the ratio of solute to solvent in a solution.
Unit: Thermochemistry
102 Questions: 69 Multiple Choice, 1 Bimodal, 4 Numeric Response, 11 Matching, 12 Short Answer, 5 Essay.
Topics:
Calculating Heats of Reaction
Enthalpy Changes
Heat in Changes of State
The Flow of Energy
Learning Objectives:
Describe how to express the enthalpy change for a reaction in a chemical equation.
Describe how to measure the change in enthalpy of a reaction.
Describe the relationship between molar heat of fusion and molar heat of solidification.
Describe the relationship between molar heat of vaporization and molar heat of condensation.
Explain the ways in which energy changes can occur.
Explain what happens to the energy of the universe during a chemical or physical process.
Identify the factors on which the heat capacity of an object depends.
Identify the thermochemical changes that can occur when a solution forms.
Identify two ways to calculate the heat of reaction when it cannot be directly measured.
Unit: Reaction Rates and Equilibrium
95 Questions: 59 Multiple Choice, 5 Bimodal, 10 Matching, 15 Short Answer, 6 Essay.
Topics:
Free Energy and Entropy
Rates of Reaction
Reversible Reactions and Equilibrium
Solubility Equilibrium
The Progress of Chemical Reactions
Learning Objectives:
Describe how most reactions progress from start to finish.
Describe how the value [delta] G is related to the spontaneity of a reaction.
Describe how to express the rate of a chemical reaction.
Describe the relationship between the solubility product constant and the solubility of a compound.
Describe what happens at the molecular level in a chemical system at equilibrium.
Describe what the size of an equilibrium constant indicates about a system at equilibrium.
Identify four factors that influence the rate of a chemical reaction.
Identify the part entropy plays in a chemical reaction.
Identify the three stresses that can cause a change in the equilibrium position of a chemical system.
Identify the two characteristics of spontaneous reactions.
Identify the two factors that determine whether a reaction is spontaneous.
Identify what information a rate law provides about a reaction.
Predict whether a precipitation will occur when two solutions are mixed.
Unit: Acids Bases Salts
120 Questions: 91 Multiple Choice, 6 Numeric Response, 10 Matching, 7 Short Answer, 6 Essay.
Topics:
Acid-Base Theories
Hydrogen Ions and Acidity
Neutralization Reactions
Salts in Solution
Strengths of Acids and Bases
Learning Objectives:
Classify a solution as neutral, acidic, or basic using pH.
Define an acid and a base according to Lewis.
Describe how acids or bases are classified as either strong or weak.
Describe how [H+] and [OH-] are related in aqueous solution.
Describe when a solution of a salt is acidic or basic.
Distinguish an acid from a base according to Arrhenius.
Distinguish an acid from a base according to the Brønsted-Lowry theory.
Identify the components of a buffer.
Identify the point in a titration when neutralization will occur.
Identify the products that form when an acid and a base react.
Identify two methods that are used to measure pH.
Unit: Oxidation-Reduction Reactions
112 Questions: 80 Multiple Choice, 4 Bimodal, 9 Numeric Response, 8 Matching, 4 Short Answer, 7 Essay.
Topics:
Describing Redox Equations
Oxidation Numbers
The Meaning of Redox
Learning Objectives:
Define oxidation and reduction in terms of a change in oxidation number.
Describe how the presence of salts and acids accelerates the corrosion of metals.
Describe two different methods for balancing a redox equation.
Describe what happens to a substance that undergoes oxidation and a substance that undergoes reduction.
Identify the two classes of chemical reactions.
State the general rule for assigning oxidation numbers.
Unit: Electrochemistry
102 Questions: 64 Multiple Choice, 7 Bimodal, 10 Matching, 10 Short Answer, 11 Essay.
Topics:
Electrochemical Cells
Electrolytic Cells
Half-Cells and Cell Potentials
Learning Objectives:
Describe how a voltaic cell produces electrical energy.
Describe some applications that use electrolytic cells.
Determine if a redox reaction is spontaneous or nonspontaneous.
Determine the standard reduction potential of a half-cell.
Distinguish between electrolytic and voltaic cells.
Identify the current applications that use electrochemical processes to produce electrical energy.
Identify the type of chemical reaction involved in all electrochemical processes.
Identify what causes the electrical potential of an electrochemical cell.
Unit: Hydrocarbons
120 Questions: 87 Multiple Choice, 1 Bimodal, 2 Numeric Response, 17 Matching, 3 Short Answer, 10 Essay.
Topics:
Hydrocarbon Rings
Hydrocarbons
Hydrocarbons From Earth's Crust
Isomers
Unsaturated Hydrocarbons
Learning Objectives:
Classify coal.
Describe bonding in a benzene ring.
Describe some of the first steps in the refining of petroleum.
Describe the structural characteristics of alkenes.
Explain how the properties of constitutional isomers differ.
Explain why a carbon atom forms four covalent bonds.
Identify the general structure of a cyclic hydrocarbon.
Identify the hydrocarbons found in natural gas.
Identify the structural characteristics of alkynes.
Identify two possible arrangements of carbon atoms in an alkane.
Identify two types of sterioisomers.
Unit: Chemistry of Life
61 Questions: 27 Multiple Choice, 9 Bimodal, 3 Numeric Response, 8 Matching, 3 Short Answer, 11 Essay.
Topics:
A Basis for Life
Amino Acids and Their Polymers
Carbohydrates
Lipids
Metabolism
Nucleic Acids
Learning Objectives:
Construct the general formula for carbohydrates.
Define gene mutation.
Describe how enzymes affect the rates of reactions in living things.
Describe the function of ATP in the cell.
Describe two examples of DNA technology used today.
Describe what happens to biological molecules and energy during catabolism and anabolism.
Diagram the general structure of an amino acid.
Explain how nitrogen-fixing bacteria provide plants with a useable form of nitrogen.
Identify the compound that is reduced during photosynthesis and the compounds formed.
Identify the functions of DNA and RNA.
Identify the number of bases of DNA required to specify one amino acid in a peptide chain.
Identify the physical property that distinguishes lipids from other biological molecules.
Identify the two major cell types that occur in nature.
Identify what determines the differences in the chemical and physiological properties of peptides and proteins.
Unit: Nuclear Chemistry
112 Questions: 84 Multiple Choice, 1 Bimodal, 4 Numeric Response, 13 Matching, 7 Short Answer, 3 Essay.
Topics:
Fission and Fusion
Nuclear Radiation
Nuclear Transformations
Radiation in Your Life
Learning Objectives:
Compare fission reactions and fusion reactions.
Compare three devices that are used to detect radiation.
Describe some practical uses of radioisotopes.
Describe three main types of nuclear radiation.
Describe what happens in a nuclear chain reaction.
Explain how nuclear reactions differ from chemical reactions.
Identify factors that determine the type of decay a radioisotope undergoes.
Identify two ways transmutations can occur.
Solve problems that involve half-life.
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