1.         Chemical Reactions

2.         What is a Reaction

            a.         The recombination of elements to produce new substances

3.         Evidence for Reactions

            a.         Release of gas

            b.         Color change

            c.         Formation of precipitate

            d.         Change in energy (heat or light)

4.         Chemical Equation

            a.         A symbolic representation of a reaction

5.         Definitions

            a.         Reactants: What you start with

            b.         Products: What you end with

            c.         Skeleton: an equation showing only what happens, not how much

            d.         Catalyst: Speeds up a reaction, shown above line

6.         Symbols Used

            a.         Establish common meaning

            b.         See overhead transparency

7.         Information in an Equation

            a.         What substances are reacting

            b.         Condition of substances

            c.         Direction of reaction

8.         Energy in Reactions

            a.         Activation Energy: needed to start reaction, over the arrow

            b.         Exothermic: Releases energy, shown as a product

            c.         Endothermic: absorbs energy, not shown in equation

9.         Equations and Conservation of Mass

            a.         Conservation of Mass requires:

                        i.         Same elements present in reactants and products

                        ii.        Total atoms/moles of each element remain same

                        iii.       Elements may be rearranged

10.       Balancing an Equation

            a.         Write word equation

            b.         Determine chemical formulas of reactants and products

            c.         Write skeleton equation

            d.         Count the number of atoms and ions on both sides of the equation

11.       Balancing Equations

            a.         Use coefficients to balance the number of atoms and ions

            b.         Do not change subscripts to balance

            c.         Make sure coefficients are in simplest ratio

12.       Reactions: Synthesis

            a.         General form: A + B ----> AB

            b.         Reactants: elements or molecules

            c.         Product: a compound

                        i.         Ionic: metal with non-metal

                        ii.        Molecular: two non-metals

                        iii.       Acid: non-metal oxide with water

                        iv.       Base: metal oxide with water

13.       Reactions: Combustion

            a.         General form: A + O₂ ----> AO

            b.         Reactants: Substance and Oxygen

            c.         Products: Oxide, CO₂, H₂O, heat, light

            d.         Reaction is rapid synthesis with oxygen

14.       Reactions: Decomposition

            a.         General form: AB ----> A + B

            b.         Reactants: single compound

            c.         Products: two or more substances

            d.         Require added energy

            e.         Explosion: a rapid decomposition

15.       Reactions: Dissociation

            a.         General form: AB ----> A⁺ + B^-

            b.         Compound separates into ions in water solution

            c.         Physical vice chemical change

            d.         Produces acids and electrolytes

16.       Reactions: Single Replacement

            a.         General form: AB + C ----> AC + B

            b.         Reactants: compound and more reactive element

            c.         Products: compound and less reactive element

17.       Activity Series

            a.         Halogens only non-metal able to replace another

                        i.         Less active down the column

            b.         Metals:

                        i.         Experimentally determined

                        ii.        Use an activity series chart

18.       Reactions: Double Replacement

            a.         General form: AB + CD ---->AD + BC

            b.         Reactants: two ionic compounds in water solution

            c.         Positive ions are exchanged

19.       Reactions: Double Displacement

            a.         Products:

                        i.         Precipitate and ionic compound in solution

                        ii.        Gas and ionic compound in solution

                        iii.       Water and ionic compound in solution

            b.         Reaction will not occur if one of above not possible

20.       Predicting a Precipitate

            a.         Use solubility rules table

                        i.         Appendix A-7

            b.         Rules used to predict if a reaction will occur

21.       Oxidation-Reduction

            a.         May be any of the four types

            b.         Form between metal and non-metal or polyatomic ions

            c.         Produce ionic compounds

22.       Half Equations

            a.         Write normal equation

            b.         Write half equations to show movement of electrons

            c.         Combine to Redox Reaction

23.       Oxidation

            a.         (Old) O₂ added to substance

            b.         (New) Substance loses e^-

            c.         4Fe⁰ ---> 4Fe⁺³ + 12 e^-

24.       Reduction

            a.         (Old) O₂ is removed from substance

            b.         Substance gains e^-

            c.         3 O₂ + 12 e^- ---> 6 O^-2

25.       Effect on Metal

            a.         Metal loses electrons

            b.         Oxidation agent (oxidizer) accepts electrons

            c.         Oxidizers have higher electron affinity

26.       Effects on Non-Metal

            a.         Gains electrons

            b.         Reducing agent donates electrons

            c.         Reducing agent has lower electron affinity

27.       Bookkeeping Rules

            a.         Oxidation number of an element is zero

            b.         Oxidation number of monatomic ion is ionic charge

            c.         Group 1 elements always +1

            d.         Group 2 elements always +2

28.       Bookkeeping Rules

            a.         Al is always +3

            b.         F is always -1

            c.         H is +1 with non-metals and -1 with metals

            d.         O is -2 in compounds and ions

29.       Bookkeeping Rules

            a.         Oxidation numbers are per atoms in a compound

            b.         Sum in a polyatomic ion is ion charge

            c.         Sum in a compound is zero