1. Unit: Chemical Reactions Types of Chemical Reactions: Synthesis and Decomposition

2. Types of Chemical Reactions 1.Synthesis 2.Decomposition 3.Single Replacement 4.Double Replacement 5.Combustion

3. Predicting Products 1.Synthesis: Two elements combine to form a compound Common form: Element + Element  Compound A + B  AB

4. Examples of synthesis: sodium + chlorine  magnesium + phosphorus  sulfur + aluminum  sodium chloride magnesium phosphide aluminum sulfide (Metal) (Non-metal) (Metal) (Non-metal)

5. Predicting Products 2. Decomposition: A compound breaks down into elements and/or smaller compounds Common form: Compound  Element + Element AB  A + B

6. Examples of decomposition: potassium nitride  potassium + nitrogen Go back to the non-metal’s original ending.

7. Examples of “special” decompositions: 1. Example of a metal chlorate decomposition: barium chlorate  barium chloride + oxygen metal chlorate  metal chloride + oxygen Always apart of the product! (ClO 3 ) -1

8. Examples of “special” decompositions: 2. Example of a metal carbonate decomposition: potassium carbonate  potassium oxide + carbon dioxide metal carbonate  metal oxide + carbon dioxide Always apart of the product! (CO 3 ) -2

9. Examples of “special” decompositions: 3. Example of a metal hydroxide decomposition: tin (IV) hydroxide  tin(IV) oxide + water metal hydroxide  metal oxide + water Always apart of the product! (OH) -1 Don’t forget the Roman numeral!