Model expected behavior in the classroom.
Discuss school and classroom rules.
Review laboratory procedures and classroom rules.
Explain and show comprehension of science process skills and the scientific method.
Make use of the metric system and the scientific measurement.

September

Define chemistry.
Classify the three states of matter.
Differentiate between mass and weight.
Recognize the difference between physical and chemical properties and changes.
Define and calculate density.
Classify matter as pure substances (elements, compounds) or mixtures (homogeneous, heterogeneous).
Explain the role of energy in chemical changes.
Distinguish between heat and temperature.
Convert between Celsius and Kelvin temperature scales.
Demonstrate understanding of measurements and calculations in chemistry (accuracy, precision, significant figures, scientific notation).

October

Explain the development of the atomic theory.
Outline the laws supporting the existence of atoms.
Demonstrate understanding of the structure of the atom.
Differentiate between atomic mass and atomic number.
Define isotopes and be able to identify them.
Construct electron configurations of atoms.
Count atoms using atomic mass units, the mole, and Avogadro's  number.
Discuss the history of the periodic table.
Define periodicity.
Examine the organization of the periodic table in relation to groups (families), periods, metals, metalloids, nonmetals, lanthanide series, actinide series.
Identify group names and their properties.
Examine trends in the periodic table (ionization energy, atomic radius, electronegativity, ionic size, electron affinity, melting and boiling points).Explain the formation of elements (natural and synthetic)

November

Explain the dependency of chemical reactivity upon electron configuration.
Demonstrate knowledge of the formation of ions.
Discuss the stability of ions in relation to noble gas configuration.
Describe the formation of ionic bonds.
State the properties of ionic compounds.
Name and write ionic compounds.
Demonstrate the formation of compounds by the sharing of electrons.
Explain how energy and electronegativity are involved in covalent bonding.
Draw molecules using Lewis electron-dot structures.
Name molecular compounds.
Relate how molecular shapes effects a substance's properties.

December

Use Avogadro's number to convert from number of moles to number of particles and visa versa.
Use molar mass to convert between moles and mass and visa versa.
Knowing the isotopic composition of a compound, calculate the average atomic mass.
Calculate the molar mass of a compound.
Determine a compound's empirical formula from its percent composition.
Determine the molecular formula or formula unit of a compound from its empirical formula and its formula mass.
Calculate percent composition of a compound from its molecular formula or formula unit.

January

Review naming and writing ionic and covalent compounds.
Identify evidence that a chemical reaction has taken place.
Construct chemical equations using word or formula equations.
List information included in an equation.
Balance equations using coefficients.
Identify and classify the five types of equations (combustion, synthesis, decomposition, single replacement, double replacement).
Write net ionic equations.
Identify atoms that are oxidized or reduced through electron transfer.
Assign oxidation numbers to atoms in compounds and ions.
Identify redox reactions by analyzing changes in oxidations numbers for different atom in the reaction.
Balance equations for oxidation-reduction reactions through the half-reaction method.
Describe the relationship between voltage and the movement of electrons.
Identify the parts of an electrochemical cell and their functions.
Write electrode reactions for cathodes and anodes.
Describe the operation of galvanic cells, including dry cells, lead-acid batteries, and fuel cells.
Identify conditions that lead to corrosion and ways to prevent it.
Calculate cell voltage from a table of standard electrode potentials.
Describe how  electrolytic cells work.
Describe the process of electrolysis in the decomposition of water and in the production of metals.
Describe the process of electroplating. 

February

Explain the steps used in solving stoichiometry problems.
Determine mole ratios to convert between amount of moles.
Use mole ratios to solve mass-mass stoichiometry problems.
Use mole ratios to solve volume-volume stoichiometry problems.
Use mole ratios to solve particle stoichiometry problems.
Identify the limiting reactant for a reaction and use it to calculate theoretical yield.
Perform calculations involving percent yield.
Apply stoichiometry problems to cars.
Describe general properties of gases.
Define pressure and convert between standard units of pressure.
Relate the kinetic-molecular theory to the properties of the ideal gas.
Use Boyle's law to solve problems involving pressure and volume.
Use Charles's law to solve problems involving volume and temperature.
Use Gay-Lussac's law to solve problems involving pressure and temperature.
Use Avogadro's law to determine the molecular mass of a gas.
Solve problems using the ideal gas law.
Describe the relationships between gas behavior and chemical formulas using Graham's law of diffusion, Gay-Lussac's law of combining volumes, and Dalton's law of partial pressures.
Solve gas stoichiometry problems using reaction stoichiometry. 

March

Distinguish among solutions, suspensions, and colloids.
Describe techniques to separate mixtures.
Calculate concentrations using common units.
Define and calculate molarity.
Use molarity in stoichiometric calculations.
Identify solubility principles and relate them to polarity and intermolecular forces.
Predict the solubility of an ionic compound using a solubility table.
Describe solutions in terms of degree of saturation.
Describe factors involved in the solubility of gases in liquids.
Distinguish between nonelectrolytes and weak and strong electrolytes.
Describe how a solute affects the freezing point and boiling point of a solution.
Explain how a surfactant stabilizes oil in a water emulsion.
Define chemical equilibrium and give examples.
Write Keq expressions for reactions in equilibrium and perform calculations with them.
Write Ksp expressions for the the solubility of slightly soluble salts and perform calculations with them.
State Le Chatelier's principle.
Apply Le Chatelier's principle to determine whether the forward or reverse reaction is formed when stress such as concentration, temperature, or pressure is applied to an equilibrium system.
Explain the common-ion effect in the context of Le Chatelier's principle.
Discuss practical uses of Le Chatelier's principle. 

April

Describe the distinctive properties of strong and weak acids, and relate their properties to the Arrhenius definition of an acid.
Describe the distinctive properties of strong and weak bases, and relate their properties to the Arrhenius definition of a base.
Compare the Bronsted-Lowry definitions of acids and bases with the Arrhenius definitions of acids and bases.
Identify conjugate acid-base pairs.
Write chemical equations that show how an amphoteric species can behave as either an acid or a base.
Use Kw in calculations.
Explain the relationship between pH and H3O concentration.
Perform calculations using pH, [H3O], [OH], and Kw.
Describe two methods of measuring pH.
Predict the product of an acid-base reaction.
Describe the conditions at the equivalence point in a titration.
Explain how you would select an indicator for an acid-base titration.
Describe the procedure for carrying out a titration to determine the concentration of an acid or base solution.
Write an equilibrium equation that shows how a weak acid is in equilibrium with its conjugate base.
Calculate Ka from the hydronium ion concentration of a weak acid solution.
Describe the components of a buffer solution, and explain how a buffer solution resists changes in pH.
Describe how the strong force attracts nucleons.
Relate binding energy and mass defect.
Predict the stability of a nucleus by considering factors such as nuclear size, binding energy, and the ratio of neutrons to protons in the nucleus.
Predict the particles and electromagnetic waves produced by different types of radioactive decay and write equations for nuclear decays.
Identify examples of nuclear fission and describe potential benefits and hazards of its use.
Describe nuclear fusion and its potential as an energy source.
Define the half-life of a radioactive nuclide, and explain how it can be used to determine an object's age.
Describe some of the uses of nuclear chemistry.
Compare acute and chronic exposures to radiation. 

May

Explain the unique properties of carbon that make the formation of organic molecules possible.
Relate the structures of diamond, graphite, and other allotropes of carbon to their properties.
Describe the nature of the bonds formed by carbon in alkanes, alkenes, alkynes, aromatic hydrocarbons, and cyclic hydrocarbons.
Classify organic compounds such as alcohols, esters, and ketones by their functional groups.
Explain how the structural difference between isomers is related to the difference in their properties.
Name simple hydrocarbons from their structural formulas.
Name branched hydrocarbons from their structural formulas.
Identify functional groups from a structural formula and assign names to compounds containing functional groups.
Draw and interpret structural formulas and skeletal structures for common organic compounds.
Describe and distinguish between substitution and addition reactions.
Describe and distinguish between condensation and elimination reactions.