• Observable properties of objects include size, shape, color, weight, and texture.

• Properties of objects and materials.

• Volume and mass are distinct components of density.
  
• Appropriate tools and use of significant digits are needed to measure volume and mass.
  
• Mass is conserved in a closed system.

States of Matter, Kinetic Molecular Theory, and Thermochemistry

• Objects and materials are solid, liquid, or gas.  Solids have a definite shape; liquids and gases take the shape of their container.

• Solids, liquids, and gases have distinct properties.
• Water can be changed from one state to another by adding or taking away heat.

• A substance has a melting point and a boiling point, both indepen-dent of the amount of the sample.
  
• Physical changes and chemical changes.
• The effect of heat on particle motion during a change in phase.

• Physical and chemical properties and changes.
  
• The three normal states of matter in terms of energy, particle motion, and phase transitions.
  
• Kinetic molecular theory explains the behavior of gases and the relationships among pressure, volume, temperature, and the number of particles in a gas sample. The combined gas law determines changes in pressure, volume, and temperature.
  
• The ideal gas law and molar volume at 273K and 1 atmosphere.
  
• Properties of gases, liquids, and solids using kinetic molecular theory; molecular behavior of matter during phase transitions.

Forms of Energy

•  Basic forms of energy, which cause motion or create change.
• Energy can be transferred from one form to another.

•  Kinetic energy is transformed into potential energy & vice versa.
• Temperature change results from adding or taking away heat energy from a system.
• Heat moves in predictable ways, from warmer to cooler objects until reaching equilibrium.

•  The law of conservation of energy; endothermic and extothermic processes.
• There is a natural tendency for systems to move in a direction of disorder or randomness (entropy).

• Many elements combine in a multitude of ways to produce compounds that make up living and nonliving things.
• Differences between an atom and a molecule.
• Basic examples of elements and compounds.
• Differences between mixtures and pure substances.

• Pure substances and mixtures; heterogeneous and homogeneous mixtures.
• Discoveries of atomic theory, the electron, the nucleus, and the planetary model of atom led to modern theory.
• Rutherford’s “gold foil” experiment led to discovering the nuclear atom. Components of the nuclear atom and how they interact.
• The laws of conservation of mass, constant composition, and multiple proportions.
• Electron configurations for twenty elements.
• The three main types of radioactive decay and their properties.
• Process of radioactive decay using nuclear equations and the concept of half-life for an isotope.
• Nuclear fission and nuclear fusion.

Periodicity

•  An element’s position on the periodic table relates to its atomic number, family, and period.
• Metals, nonmetals, and metalloids on the periodic table.
• An element’s position on the periodic table relates to its electron configuration and reactivity.
  Trends on the periodic table.

• Atoms combine through ionic and covalent bonding. Valence electrons can predict chemical formulas.
• Lewis dot structures for simple molecules and ionic compounds.
• Electronegativtiy explains polar and nonpolar covalent bonds.
• Valence-shell electron-pair repulsion theory predicts molecular geometry of simple molecules.
• Hydrogen bonding in water affects a variety of physical, chemical, and biological phenomena.
• Chemical formulas for simple ionic and molecular compounds.  

• Conservation laws are used to balance chemical equations.
• Classifications of chemical reactions.
• The number of particles and molar mass can be determined using the mole concept.
• Percent compositions; empirical and molecular formulas.
• Mass-to-mass stoichiometry for a chemical reaction.
• Percent yield in a chemical reaction 

•  Process by which solutes dissolve in solvents.
• Concentration, solution dilution, and solution stoichiometry, using molarity.
• Factors that affect the rate of dissolving.
• The properties of solutions and pure solvents.
• Factors affecting the rate of a chemical reaction.
• The factors and processes that can cause a shift in equilibrium of a system.

• Theories of acids and bases in terms of the presence of hydronium and hydroxide ions in water, and proton donors and acceptors.
• The pH scale and acidic, basic, and neutral solutions are related to hydrogen ion concentrations.
• How a buffer works.
• Oxidation and reduction reactions and everyday examples; oxidation numbers in a reaction.