1. The Periodic Table displays the elements in increasing atomic number and shows how periodicity of the physical and chemical properties of the elements relates to atomic structure. As a basis for understanding this concept, students know

• how to relate the position of an element in the Periodic Table to its atomic number and atomic mass
  
• how to use the Periodic Table to identify metals, semimetals, nonmetals, and halogens
  
• how to use the Periodic Table to identify alkali metals, alkaline earth metals and transition metals, and trends in ionization energy, electronegativity, and the relative sizes of ions and atoms
  
• how to use the Periodic Table to determine the number of electrons available for bonding
  
• the nucleus is much smaller in size than the atom yet contains most of its mass
  
• * how to use the Periodic Table to identify the lanthanides and actinides, and transactinide elements, and know that the transuranium elements were man-made
  
• * how to relate the position of an element in the periodic table to its quantum electron configuration, and reactivity with other elements in the table
  
• * the experimental basis for the development of the quantum theory of atomic structure and the historical importance of the Bohr model of the atom
  
• * spectral lines are a result of transitions of electrons between energy levels. Their frequency is related to the energy spacing between levels using Planck's relationship (E=hv).

2. Biological, chemical, and physical properties of matter result from the ability of atoms to form bonds based on electrostatic forces between electrons and protons, and between atoms and molecules. As a basis for understanding this concept, students know

• atoms combine to form molecules by sharing electrons to form covalent or metallic bonds, or by exchanging electrons to form ionic bonds
  
• chemical bonds between atoms in molecules such as H2, CH4, NH3, H2CCH2, N2, Cl2, and many large biological molecules are covalent
  
• salt crystals such as NaCl are repeating patterns of positive and negative ions held together by electrostatic attraction
  
• in a liquid the inter-molecular forces are weaker than in a solid, so that the molecules can move in a random pattern relative to one-another
  
• how to draw Lewis dot structures
  
• * how to predict the shape of simple molecules and their polarity from Lewis dot structures
  
• * how electronegativity and ionization energy relate to bond formation.

3. The conservation of atoms in chemical reactions leads to the principle of conservation of matter and the ability to calculate the mass of products and reactants. As a basis for understanding this concept, students know

• how to describe chemical reactions by writing balanced equations
  
• the quantity one mole is defined so that one mole of carbon 12 atoms has a mass of exactly 12 grams
  
• one mole equals 6.02x1023 particles (atoms or molecules)
  
• how to determine molar mass of a molecule from its chemical formula and a table of atomic masses, and how to convert the mass of a molecular substance to moles, number of particle or volume of gas at standard temperature and pressure
  
• how to calculate the masses of reactants and products in a chemical reaction from the mass of one of the reactants or products, and the relevant atomic masses
  
• * how to identify reactions that involve oxidation and reduction and how to balance oxidation-reduction reactions.

4. The Kinetic Molecular theory describes the motion of atoms and molecules and explains the properties of gases. As a basis for understanding this concept, students know

• the random motion of molecules and their collisions with a surface create the observable pressure on that surface
  
• the random motion of molecules explains the diffusion of gases
  
• how to apply the gas laws to relations between the pressure, temperature, and volume of any amount of an ideal gas or any mixture of ideal gases
  
• the values and meanings of standard temperature and pressure (STP)
  
• how to convert between Celsius and Kelvin temperature scales
  
• there is no temperature lower than 0 Kelvin
  
• the kinetic theory of gases relates the absolute temperature of a gas to the average kinetic energy of its molecules or atoms
  
• how to solve problems using the ideal gas law in the form PV=nRT.

5. Acids, bases, and salts are three classes of compounds that form ions in water solutions. As a basis for understanding this concept, students know

• the observable properties of acids, bases and salt solutions
  
• acids are hydrogen-ion-donating and bases are hydrogen-ion-accepting substances
  
• strong acids and bases fully dissociate and weak acids and bases partially dissociate
  
• how to use the pH scale to characterize acid and base solutions
  
• how to calculate pH from the hydrogen ion concentration.

6. Solutions are homogenous mixtures of two or more substances. As a basis for understanding this concept, students know

• definitions of solute and solvent
  
• how to describe the dissolving process as a result of random molecular motion
  
• temperature, pressure, and surface area affect the dissolving process
  
• how to calculate the concentration of a solute in terms of grams per liter, molarity, parts per million and percent composition.

7. Energy is exchanged or transformed in all chemical reactions and physical changes of matter. As a basis for understanding this concept, students know

• how to describe temperature and heat flow in terms of the motion of molecules (or atoms)
  
• chemical processes can either release (exothermic) or absorb (endothermic) thermal energy
  
• energy is released when a material condenses or freezes and absorbed when a material evaporates or melts.

8. Chemical reaction rates depend on factors that influence the frequency of collision of reactant molecules. As a basis for understanding this concept, students know

• the rate of reaction is the decrease in concentration of reactants or the increase in concentration of products with time
  
• how reaction rates depend on such factors as concentration, temperature, and pressure.
  
• the role a catalyst plays in increasing the reaction rate
  
• * the definition and role of activation energy in a chemical reaction.

9. Chemical equilibrium is a dynamic process at the molecular level. As a basis for understanding this concept, students know

• equilibrium is established when forward and reverse reaction rates are equal
  
• how to use LeChatelier's Principle to predict the effect of changes in concentration, temperature and pressure.

10. The bonding characteristics of carbon lead to many different molecules with varied sizes, shapes, and chemical properties, providing the biochemical basis of life. As a basis for understanding this concept, students know

• the bonding characteristics of carbon lead to a large variety of structures ranging from simple hydrocarbons to complex polymers and biological molecules.

11. Nuclear processes are those in which an atomic nucleus changes, including radioactive decay of naturally occurring and man-made isotopes, nuclear fission, and nuclear fusion. As a basis for understanding this concept, students know

• protons and neutrons in the nucleus are held together by strong nuclear forces which are stronger than the electromagnetic repulsion between the protons
  
• the energy release per gram of material is much larger in nuclear fusion or fission reactions than in chemical reactions: change in mass (calculated by E=mc) is small but significant in nuclear reactions
  
• many naturally occurring isotopes of elements are radioactive, as are isotopes formed in nuclear reactions
  
• the three most common forms of radioactive decay (alpha, beta, gamma) and how the nucleus changes in each type of decay
  
• alpha, beta, and gamma radiation produce different amounts and kinds of damage in matter and have different penetration
  
• * how to calculate the amount of a radioactive substance remaining after an integral number of half lives have passed