1. Chemical Reactions
   1. Simple
      1. Synthesis
         1. A + B -> AB
      2. Decomposition
         1. AB -> A + B
      3. Combustion
         1. Fuel + Oxygen + Energy -> Carbon byproducts + More energy
         2. Contributes to greenhouse effect and acid rain
   2. Displacement
      1. Single
         1. AB + C -> AC + B
         2. More reactive replaces less reactive
      2. Double
         1. AB + CD -> AD + CB
         2. Occurs between two ionic compounds
         3. Topic
            1. High solubility means that much of the product will stay within the solution
            2. Low solubility means that either a solid precipitate or gas will form
            3. Different compounds have different solubilities in different solvents
         4. Neutralization reactions fall under this
2. Nomenclature
   1. Binary ionic
      1. Metal name
      2. Non-metal(ide)
   2. Covalent
      1. (amount prefix)non-metal
      2. (amount prefix)non-metal(ide)
   3. Oxyanions
      1. Number of O2 molecules
         1. 1
            1. (hypo)non-metal(ite)
         2. 2
            1. non-metal(ite)
         3. 3
            1. non-metal(ate)
         4. 4
            1. (per)non-metal(ate)
   4. Hydrates
      1. Molecule name (amount prefix)hydrate
   5. Acids
      1. Binary
         1. (hydro)non-metal(ic) acid
         2. (aqueous) compound name
      2. Oxyacids
         1. Number of O2 molecules
            1. 1
            2. (hypo)non-metal(ous) acid
            3. 2
            4. non-metal(ous) acid
            5. 3
            6. non-metal(ic) acid
            7. 4
            8. (per)non-metal(ic) acid
3. Periodic Trends
   1. Electronegativity
      1. The tendency for an element to attract electrons
      2. Combines the scales of ionization energy and atomic radius into a simple package
      3. On the periodic table, the trend travels from
         1. Bottom left
            1. Large atomic radius, few electrons
         2. Top right
            1. Small atomic radius, many electrons
   2. Atomic Radius
      1. The distance between two nuclei of atoms of the same element bonded together
      2. Two determining factors
         1. Shielding
            1. Electrons in lower energy levels provide a shield from nuclear attraction for the valence electrons, increasing radius
         2. Number of protons
            1. Protons attract electrons towards the nucleus, decreasing radius
      3. On the periodic table, the trend travels from
         1. Top right
            1. Little shielding, high nuclear attraction
         2. Bottom left
            1. Lots of shielding, little nuclear attraction
   3. Ionization Energy
      1. The amount of energy required to remove an electron from an atom or ion in a gaseous state
      2. Element in gaseous state + energy -> Element with a positive charge in a gaseous state + an electron
      3. The more electrons in the valence shell, the more energy will be required to remove them
         1. This is because elements with a high number of valence electrons are close to becoming stable
         2. Less energy shells, harder to remove e-
            1. Reduced shielding
            2. Increased nuclear attraction
   4. Electron Affinity
      1. A measurement of the energy change when an atom gains an electron.
         1. Either a
            1. Release of energy due to higher attraction to nucleus than repulsion by electrons
            2. Absorbtion of energy due to lower attraction to nucleus than repulsion by electrons
      2. On the periodic table, the trend travels from left to right, within a period.
4. Types of Chemical Bonds
   1. Covalent
      1. The sharing of electrons between two or more atoms
         1. Polar
            1. Unequal sharing resulting in partial charges
         2. Non-polar
            1. Equal sharing due to equal electronegativity
      2. Create molecules
   2. Ionic
      1. Non-metal takes electron from metal
         1. One atom becomes positive, the other negative
      2. Binary
         1. Occur between metals and non-metals
      3. Tertiary
         1. Occur between metals and polyatomic ions
            1. Polyatomics are a group of atoms that behave as one
5. Chemical Bonding
   1. Intramolecular forces
      1. The attractive force between atoms within a compound
   2. Intermolecular forces
      1. Van der Waals forces
         1. dipole-dipole
            1. Forces of attraction between oppositely charged ends of polar molecules
         2. London dispersion forces
            1. Exist between all molecules
            2. Temporary displacements in the electron cloud
            3. Short-lived dipoles
      2. Hydrogen bonding
         1. Occur between either N, O, F, and H
         2. Similar to dipole-dipole, but much stronger