• designated laboratory techniques;

• safe use of chemicals and equipment;

• proper response to emergency situations;

• multiple variables are manipulated with repeated trials;

• accurate recording, organizing, and analysis of data through repeated trials;

• mathematical and procedural error analysis; and

• mathematical manipulations (SI units, scientific notation, linear equations, graphing, ratio and proportion, significant digits, dimensional analysis, use of scientific calculator).

• mass/atomic number;

• isotopes/half–lives/nuclear particles;

• particle/mass charge;

• families/groups;

• series/periods;

• trends/patterns: atomic/nuclear radii, electronegativity, shielding effect;

• electron configurations/oxidation numbers;

• chemical/physical properties; and

• historical/quantum models.

• nomenclature;

• balancing chemical equations;

• writing chemical formulas –– molecular, structural, empirical, and Lewis diagrams;

• bonding types –– ionic, covalent;

• reaction types –– synthesis, decomposition, single and double replacement, oxidation–reduction, neutralization, nuclear, exothermic and endothermic, spontaneous/non–spontaneous, dissociation ionization;

• physical and chemical equilibrium; and

• reaction rates and kinetics: activation energy, catalysis, degree of randomness.

• avogadro's principle, molar volume;

• stoichiometric relationships;

• partial pressure;

• gas laws;

• solution concentrations;

• chemical equilibrium; and

• acid/base theory: strong/weak electrolytes, dissociation/ionization (pH, pOH), and titration.

• pressure, temperature, and volume;

• vapor pressure;

• partial pressures;

• phase changes;

• molar heats of fusion and vaporization;

• specific heat capacity;

• solutions; and

• colligative properties.

• organic and biochemistry;

• nuclear chemistry; and

• environmental chemistry.