Chapter 1 Matter and Change
1-1: Chemistry Is a Physical Science
1. Define chemistry.
2. List examples of the branches of chemistry.
3. Compare and contrast basic research, applied research, and technological development.
1-2: Matter and Its Properties
1. Distinguish between the physical properties and chemical properties of matter.
2. Classify changes of matter as physical or chemical.
3. Explain the gas, liquid, and solid states in terms of particles.
4. Explain how the law of conservation of energy applies to changes of matter.
5. Distinguish between a mixture and a pure substance.
1-3: Elements
1. Use a periodic table to name elements, given their symbols.
2. Use a periodic table to write the symbols of elements, given their names.
3. Describe the arrangement of the periodic table.
4. List the characteristics that distinguish metals, nonmetals, and metalloids.
Chapter 2 Measurements and Calculations
2-1: Scientific Method
1. Describe the purpose of the scientific method.
2. Distinguish between qualitative and quantitative observations.
3. Describe the differences between hypotheses, theories, and models.
2-2: Units of Measurement
1. Distinguish between a quantity, a unit, and a measurement standard.
2. Name and use SI units for length, mass, time, volume, and density.
3. Distinguish between mass and weight.
4. Perform density calculations.
5. Transform a statement of equality into a conversion factor.
2-3: Using Scientific Measurements
1. Distinguish between accuracy and precision.
2. Determine the number of significant figures in measurements.
3. Perform mathematical operations involving significant figures.
4. Convert measurements into scientific notation.
Ch. 3: Atoms: The Building Blocks of Matter
3-1: Atom: From Philosophical Idea to Scientific Theory
1. Explain the laws of conservation of mass, definite proportions, and multiple proportions.
2. Summarize the five essential points of Dalton's atomic theory.
3. Explain the relationship between Dalton's atomic theory and the law of conservation of mass, the law
of definite proportions, and the law of multiple proportions.
3-2: The Structure of the Atom
1. Summarize the observed properties of cathode rays that led to the discovery of the electron.
2. Summarize the experiment carried out by Rutherford and his coworkers that led to the discovery of the
nucleus.
3. List the properties of protons, neutrons, and electrons.
4. Define atom.
3-3: Counting Atoms
1. Explain what isotopes are.
2. Define atomic number and mass number, and describe how they apply to isotopes.
3. Determine the number of protons, neutrons, and electrons of a nuclide, given its identity.
4. Define mole, Avogadro's number, and molar mass, and state how all three are related.
5. Solve problems involving mass in grams, amount in moles, and number of atoms of an element.
Chapter 4 Arrangement of Electrons in Atoms
4-1: The Development of the New Atomic Model
1. Explain the mathematical relationship among the speed, wavelength, & frequency of electromagnetic
radiation.
2. Discuss the dual wave-particle nature of light.
3. Discuss the significance of the photoelectric effect and the line-emission spectrum of hydrogen to the
development of the atomic model.
4. Describe the Bohr model of the hydrogen atom.
4-2: The Quantum Model of the Atom
1. Discuss Louis de Broglie’s role in the development of the quantum model of the atom.
2. Compare and contrast the Bohr model and the quantum model of the atom.
3. Explain how the Heisenberg uncertainty principle & Schrödinger wave equation led to the idea of
atomic orbitals.
4. List the four quantum numbers, and describe their significance.
5. Relate the number of sublevels corresponding to each of an atom’s main energy levels, the number of
orbitals per sublevel, and the number of orbitals per main energy level.
4-3: Electron Configurations
1. List the total number of electrons needed to fully occupy each main energy level.
2. State the Aufbau principle, the Pauli exclusion principle, and Hund’s rule.
3. Describe the electron configurations for the atoms of any element using orbital notation, electronconfiguration notation, and when appropriate, noble-gas notation.
Chapter 5 The Periodic Law
5-1: History of the Periodic Table
1. Explain the roles of Mendeleev and Moseley in the development of the periodic table.
2. Describe the modern periodic table.
3. Explain how the periodic law can be used to predict the physical and chemical properties of elements.
4. Describe how the elements belonging to a group of the periodic table are interrelated in terms of
atomic number.
5-2: Electron Configurations and the Periodic Table
1. Describe the relationship between electrons in sublevels & the length of a period of the periodic table.
2. Locate and name the four blocks of the periodic table. Explain the reasons for these names.
3. Discuss the relationship between group configurations and group numbers.
4. Describe the locations in the periodic table and the general properties of the alkali metals, the alkalineearth metals, the halogens, and the noble gases.
5-3: Electron Configuration and Periodic Properties
1. Define atomic and ionic radii, ionization energy, electron affinity, and electronegativity.
2. Compare the periodic trends of atomic radii, ionization energy, and electronegativity, and state the
reasons for these variations.
3. Define valence electrons, & state how many are present in atoms of each main-group element.
4. Compare the atomic radii, ionization energies, and electronegativities of the d-block elements with
those of the main-group elements.
Chapter 6 Chemical Bonding
6-1: Introduction to Chemical Bonding
1. Define chemical bond and Explain why most atoms form chemical bonds.
2. Describe ionic and covalent bonding and Explain why most chemical bonding is neither purely ionic
nor purely covalent.
3. Classify bonding type according to electronegativity differences.
4. Compare and contrast a chemical formula for a molecular compound with one for an ionic compound.
5. Define valence electrons, and state how many are present in atoms of each main-group element.
6-2: Covalent Bonding and Molecular Compounds
1. Define molecule and molecular formula.
2. Explain the relationships among potential energy, distance between approaching atoms, bond length,
and bond energy.
4.List the six basic steps used in writing Lewis structures and Explain how to determine Lewis structures
for molecules containing single bonds, multiple bonds, or both.
5. Explain why scientists use resonance structures to represent some molecules.
6-3: Ionic Bonding and Ionic Compounds
1. Compare and contrast a chemical formula for a molecular compound with one for an ionic compound.
2. Discuss the arrangements of ions in crystals.
3. Define lattice energy and explain its significance.
4. List and compare the distinctive properties of ionic and molecular compounds.
5. Write the Lewis structure for a polyatomic ion given the identity of the atoms combined and other
appropriate information.
6-4: Metallic Bonding
1. Describe the electron-sea model of metallic bonding, & explain why metals are good conductors.
2. Explain why metal surfaces are shiny.
3. Explain why metals are malleable and ductile but ionic-crystalline compounds are not.
6-5: Molecular Geometry
1. Explain VSEPR theory and predict the shapes of molecules or polyatomic ions using VSEPR theory.
2. Explain how the shapes of molecules are accounted for by hybridization theory.
3. Describe dipole-dipole forces, hydrogen bonding, induced dipoles, and London dispersion forces and
their effects on properties such as boiling and melting points.
4. Explain what determines molecular polarity.
Chapter 7 Chemical Formulas and Chemical Compounds
7-1: Chemical Names and Formulas
1. Explain the significance of a chemical formula.
2. Determine the formula of an ionic compound formed between two given ions.
3. Name an ionic compound given its formula.
4. Name a binary molecular compound from its formula, using prefixes.
5. Write the formula of a binary molecular compound given its name.
7-2: Oxidation Numbers
1. List the rules for assigning oxidation numbers.
2. Give the oxidation number for each element in the formula of a chemical compound.
3. Name binary molecular compounds using oxidation numbers and the Stock system.
7-3: Using Chemical Formulas (Refresher)
1. Calculate the formula mass or molar mass of any given compound.
2. Convert between mass in grams and amount in moles of a chemical compound, using molar mass.
3. Calculate the number of molecules, formula units, or ions in a given molar amount of a chemical
compound.
4. Calculate the percentage composition of a given chemical compound.
7-4: Determining Chemical Formulas
1. Define empirical formula, and explain how the term applies to ionic and molecular compounds.
2. Determine an empirical formula from either a percentage or a mass composition.
3. Explain the relationship between the empirical formula & molecular formula of a given compound.
4. Determine a molecular formula from an empirical formula.
Chapter 8 Chemical Equations and Reactions
8-1: Describing Chemical Reactions
1. List three observations that suggest that a chemical reaction has taken place.
2. List three requirements for a correctly written chemical equation.
3. Write a word equation and a formula equation for a given chemical reaction.
4. Balance a formula equation by inspection.
8-2: Types of Chemical Reactions
1. Define and give general equations for synthesis, decomposition, single-displacement, and doubledisplacement reactions.
2. Classify combustion. incomplete
3. List four types of single-displacement reactions/ three types of double-displacement reactions.
4. Predict the products of simple reactions given the reactants.
5. Electrolysis
8-3: Activity Series of the Elements
1. Explain the significance of an activity series.
2. Predict whether a given reaction will occur and what the products will be, using an activity series.
Chapter 9 Stoichiometry
9-1: Introduction to Stoichiometry
1. Define stoichiometry.
2. Describe the importance of the mole ratio in stoichiometric calculations.
3. Write a mole ratio relating two substances in a chemical equation.
9-2: Ideal Stoichiometric Calculations
1. Calculate the moles of a reactant or product from the amount in moles of a different reactant or
product.
2. Calculate the mass of a reactant/product from moles of a different reactant/product.
3. Calculate the moles of a reactant or product from the mass of a different reactant or product.
4. Calculate the mass of a reactant or product from the mass of a different reactant or product.
9-3: Limiting Reactants and Percentage Yield
1. Describe a method for determining which of two reactants is a limiting reactant.
2. Calculate the moles or mass of a product, given the moles or masses of two reactants, one of which is in
excess.
3. Distinguish between theoretical yield, actual yield, and percentage yield.
4. Calculate percentage yield, given the actual yield and quantity of a reactant.
Chapter 10 States of Matter
10-1: The Kinetic-Molecular Theory of Matter
1. State the kinetic-molecular theory of matter, & describe how it explains certain properties of matter.
2. List the 5 assumptions of the kinetic-molecular theory of gases. Define ideal gas and real gas.
3. Describe each of the following characteristic properties of gases: expansion, density, fluidity,
compressibility, diffusion, and effusion.
4. Describe the conditions under which a real gas deviates from “ideal” behavior.
10-2: Liquids
1. Describe the motion of liquid particles & the properties of liquids according to the kinetic-molecular
theory.
2. Discuss the process by which liquids can change into gases. Define vaporization.
3. Discuss the process by which liquids can change into solids. Define freezing.
10-3: Solids
1. Describe the motion of solid particles & the properties of solids according to the kinetic-molecular
theory.
2. Distinguish between the two types of solids.
3. Describe the different types of crystal symmetry. Define crystal structure and unit cell.
10-4: Changes of State
1. Explain the relationship between equilibrium and changes of state.
2. Interpret phase diagrams.
3. Explain what is meant by equilibrium vapor pressure.
4. Describe the processes of boiling, freezing, melting, and sublimation.
10-5: Water
1. Describe the structure of a water molecule.
2. Discuss the physical properties of water. Explain how they are determined by the structure of water.
3. Calculate the amount of heat energy absorbed or released when a quantity of water changes state.
Chapter 11 Gases
11-1: Gases and Pressure
1. Define pressure, give units of pressure, and describe how pressure is measured.
2. State the standard conditions of temperature and pressure and convert units of pressure.
3. Calculate partial pressures and total pressures, using Dalton’s law of partial pressures.
11-2: The Gas Laws
1. Explain the relationships between gas volume, temperature, pressure, using the kinetic-molecular
theory.
2. Calculate volume-pressure changes at constant temperature, using Boyle’s law.
3. Calculate volume-temperature changes at constant pressure, using Charles’s law.
4. Calculate pressure-temperature changes at constant volume, using Gay-Lussac’s law.
5. Calculate volume-temperature-pressure changes, using the combined gas law.
11-3: Gas Volumes and the Ideal Gas Law
1. State the law of combining volumes.
2. State Avogadro’s law and explain its significance.
3. Define standard molar volume of a gas, and use it to calculate gas masses and volumes.
4. Calculate pressure, volume, temperature, or amount of gas when the other three quantities are known,
using the ideal gas law.
11-4 Diffusion and Effusion
1. Describe the process of diffusion.
2. State Graham’s law of effusion
3. State the relationship between the molecular velocities of two gases and their molar masses.
Chapter 12 Solutions
12-1 Types of Mixtures
1. Distinguish between heterogeneous and homogeneous mixtures.
2. List three different solute-solvent combinations.
3. Compare the properties of suspensions, colloids, and solutions.
4. Distinguish between electrolytes and nonelectrolytes.
12-2: The Solution Process
1. List and explain three factors that affect the rate at which a solid solute dissolves in a liquid solvent.
2. Explain solution equilibrium, and distinguish among saturated, unsaturated, and supersaturated
solutions.
3. Explain the meaning of like dissolves like in terms of polar and nonpolar substances.
4. List the three interactions that contribute to the enthalpy of solution, and explain how they combine to
cause dissolution to be exothermic or endothermic.
5. Compare the effects of temperature and pressure on solubility.
12-3: Concentration of Solutions
1. Calculate the concentration of a solution, given the mass of solute and volume of solvent.
2. Determine the amount of solute in a given amount of solution, given the concentration of the solution.
3. Determine the amount of solution that contains a given amount of solute, given the solution’s
concentration
Chapter 13 Ions in Aqueous Solutions & Colligative Properties
13-1: Compounds in Aqueous Solutions
1. Write equations for the dissolution of soluble ionic compounds in water.
2. Predict whether a precipitate will form when solutions of soluble ionic compounds are combined, and
write net ionic equations for precipitation reactions.
3. Compare dissociation of ionic compounds with ionization of molecular compounds.
4. Draw the structure of the hydronium ion, & explain why it is used to represent the hydrogen ion in
solution.
5. Distinguish between strong electrolytes and weak electrolytes.
13-2: Colligative Properties of Solutions
1. List four colligative properties, and explain why they are classified as colligative properties.
2. Calculate freezing-point depression, boiling-point elevation, & solution molality of nonelectrolyte
solutions.
3. Calculate the expected changes in freezing point and boiling point of an electrolyte solution.
4. Discuss causes of the differences between expected and experimentally observed colligative properties
of electrolyte solutions.
Chapter 14 Acids and Bases
14-1: Properties of Acids and Bases
1. List five general properties of aqueous acids and bases.
2. Name common binary acids and oxyacids, given their chemical formulas.
3. List five acids commonly used in industry and the laboratory, and give two properties of each.
4. Define acid and base according to Arrhenius's theory of ionization.
5. Explain the differences between strong and weak acids and bases.
14-2: Acid-Base Theories
1. Define and recognize Brønsted-Lowry acids and bases.
2. Define a Lewis acid and a Lewis base.
14-3: Acid-Base Reactions
1. Describe a conjugate acid, a conjugate base, and an amphoteric compound.
2. Explain the process of neutralization.
3. Explain how acid rain damages marble structures.
Chapter 15 Acid-Base Titration and pH
15-1: Aqueous Solutions & the Concept of pH- 45 MIN.
1. Describe the self-ionization of water.
2. Define pH, and give the pH of a neutral solution at 25°C.
3. Explain and use the pH scale.
4. Find pH, given [H3O+] or [OH–]. 5. Find [H3O+] or [OH–], given pH.
15-2: Determining pH and Titrations
1. Describe how an acid-base indicator functions.
2. Explain how to carry out an acid-base titration.
3. Calculate the molarity of a solution from titration data.
Chapter 16 Reaction Energy
16-1: Thermochemistry
1. Define temperature, and state the units in which it is measured.
2. Define heat and state its units.
3. Perform specific heat calculations.
4. Explain heat of reaction, heat of formation, heat of combustion, and enthalpy change.
5. Solve problems involving enthalpies of reaction, enthalpies of formation, & enthalpies of combustion.
16-2: Driving Force of Reactions
1. Explain the relationship between enthalpy change and the tendency of a reaction to occur.
2. Explain the relationship between entropy change and the tendency of a reaction to occur.
3. Discuss the concept of free energy, & explain how this quantity’s value is calculated & interpreted.
4. Describe the use of free energy change to determine the tendency of a reaction to occur.
Chapter 17 Reaction Kinetics
17-1: The Reaction Process
1. Explain the concept of reaction mechanism.
2. Interpret chemical reactions, using collision theory.
3. Define activated complex.
4. Relate activation energy to heat of reaction.
17-2: Reaction Rate
1. Define chemical kinetics, and explain the two conditions necessary for chemical reactions to occur.
2. Discuss the five factors that influence reaction rate.
3. Define catalyst, and discuss two different types.
4. Explain and write rate laws for chemical reactions.
Chapter 18 Chemical Equilibrium
18-1: The Nature of Chemical Equilibrium
1. Define chemical equilibrium.
2. Explain the nature of the equilibrium constant.
3. Write chemical equilibrium expressions and carry out calculations involving them.
18-2: Shifting Equilibrium
1. Discuss the factors that disturb equilibrium.
2. Discuss conditions under which reactions go to completion.
3. Describe the common-ion effect.
18-3: Equilibria of Acids, Bases, and Salts
1. Explain the concept of acid-ionization constants, and write acid-ionization equilibrium expressions.
2. Review the ionization constant of water.
3. Explain buffering.
4. Compare cation and anion hydrolysis.
18-4: Solubility Equilibrium
1. Explain what is meant by solubility product constants, and calculate their values.
2. Calculate solubilities using solubility product constants.
3. Carry out calculations to predict whether precipitates will form when solutions are combined.
Chapter 19 Oxidation-Reduction Reactions
19-1: Oxidation and Reduction
1. Assign oxidation numbers to reactant and product species.
2. Define oxidation and reduction.
3. Explain what an oxidation-reduction (redox reaction) is.
19-2: Balancing Redox Equations
1. Explain what must be conserved in redox equations.
2. Balance redox equations by using the half-reaction method.
19-3: Oxidizing and Reducing Agents
1. Relate chemical activity to oxidizing and reducing strength.
2. Explain the concept of disproportionation.
Chapter 20 Electrochemistry
20-1: Introduction to Electrochemistry
1. Identify parts of the electrochemical cell and their functions.
2. Write electrode half reactions for cathodes and anodes.
20-2: Voltaic Cells
1. Describe the operation of voltaic cells, including dry cells, lead-acid batteries, and fuel cells.
2. Identify conditions that lead to corrosion and ways to prevent it.
3. Describe the relationship between voltage and the movement of electrons.
4. Calculate cell voltage/potentials from a table of standard electrode potentials.
20-3: Electrolytic Cells
1. Describe the nature of electrolytic cells.
2. Describe the process of electrolysis in the decomposition of water and in the production of metals.
3. Explain the process of electroplating.
4. Describe the chemistry of a rechargeable cell.
Chapter 21 Nuclear Chemistry
21-1: The Nucleus
1. Explain what a nuclide is, and describe the different ways nuclides can be represented.
2. Define and relate the terms mass defect and nuclear binding energy.
3. Explain the relationship between nucleon number and stability of nuclei.
4. Explain why nuclear reactions occur and know how to balance a nuclear equation.
21-2: Radioactive Decay
1. Define and relate the terms radioactive decay and nuclear radiation.
2. Describe the different types of radioactive decay and their effects on the nucleus.
3. Define the term half-life, and explain how it relates to the stability of a nucleus.
4. Define and relate the terms decay series, parent nuclide, and daughter nuclide.
5. Explain how artificial radioactive nuclides are made, and discuss their significance.
21-3: Nuclear Radiation
1. Compare the penetrating ability and shielding requirements of - particles,  particles, &  rays.
2. Define the terms roentgen and rem, and distinguish between them.
3. Describe three devices used in radiation detection.
4. Discuss applications of radioactive nuclides.
21-4: Nuclear Fission and Nuclear Fusion
1. Define nuclear fission, chain reaction, and nuclear fusion, and distinguish between them.
2. Explain how a fission reaction is used to generate power.
3. Discuss the possible benefits and the current difficulty of controlling fusion reactions.
Chapter 22 Organic Chemistry
22-1: Organic Compounds
1. Explain how the structure & bonding of carbon lead to the diversity and number of organic compounds.
2. Compare the use of molecular and structural formulas to represent organic compounds.
3. Compare structural and geometric isomers of organic compounds.
22-2: Hydrocarbons
1. Distinguish among the structures of alkanes, alkenes, alkynes, and aromatic hydrocarbons.
2. Write structural formulas and names for alkanes, alkenes, and alkynes.
3. Relate properties of different types of hydrocarbons to their structures.
22-3: Functional Groups
1. Define functional group and explain why functional groups are important.
2. Identify alcohols, alkyl halides, ethers, aldehydes, ketones, carboxylic acids, esters, and amines based
on the functional group present in each.
3. Explain the relationships between the properties and structures of alcohols, alkyl halides, ethers,
aldehydes, ketones, carboxylic acids, esters, and amines.
This is a guide to help you study- NOT the end-all-be-all for what is on the exam. Please review all of
your notes from class.
Overview of certain objectives:
o Classify matter as pure substance or mixture
o Compare, contrast and identify elements and compounds, heterogeneous/ homogeneous
mixtures, and physical/chemical properties/changes
o Apply the law of conservation of matter/energy to physical/chemical change
o Trace the history of the atomic theory from Democritis, Dalton, Thomson, Rutherford, Bohr, and
modern theory
o Determine the number of protons, neutrons and electrons of an isotope
o Describe the relationship between emission spectra and position of electrons
o Trace the history of the organization of elements
o Use the concept of periodicity to predict chemical and physical properties of elements using the
Periodic Table (metals, nonmetals, metalloids, etc.)
o Identify substances as ionic or covalent and explain the role of electrons.
o Elements form chemical bonds in order to achieve stability according to the octet rule.
o Compare and contrast properties of ionic and covalent compounds.
o Describe how groups on the Periodic Table exhibit varying chemical reactivity.
o Write names and formulas for different types of compounds
o Balance chemical equations to satisfy the law of conservation of mass.
o Classify different types of chemical reactions
o Predict the products of chemical reactions (basic predictions)
o Why are different temperature scales used?
o Compare and contrast solutions, colloids, and suspensions.
o Explain the unique properties of water and why it is called the universal solvent
o Organic versus inorganic