2. Coefficient- In a chemical equation, the number written in front of a reactant or product; gives the smallest number of particles of the substance involved in the reaction. Reactants- starting substances. Products- substances formed during the reaction. Synthesis Reactions- chemical reaction in which two or more substances react to produce a single product.

3. Combustion Reaction- oxygen combines with a substance and release energy in the form of heat and light. Decomposition Reaction- a single compound breaks down into two or more elements or new compounds. Single Replacement- A reaction in which the atoms of one element replace the atoms of another element in a compound. Double Replacement- Involves an exchange of ions between two compounds.

4. When two elements react, the reaction is always a synthesis reaction. Example: 2 Na (s) + Cl 2 → 2 NaCl

5. Example: C (s) + O 2 → CO 2 In a combustion a substance is always combined with a oxygen. Note: Oxygen is on the reactants side. Example 2: 2 H 2 (g) + O 2 (g) → 2 H 2 O (l)

6. Single compound breaks down into two or more substances. Example: 2NaN 3 (s) → 2 Na (s) + 3 N 2

7. Atoms of one element replace the atoms of another element in a compound. Example: Cu (s) + 2 AgNO 3 (aq) → 2 Ag (s) + Cu(NO 3 ) 2 (aq)

8. Exchange of ions between two compounds Example: KCN(aq) + HBr (aq) → KBr(aq) + HCN (g)

9. 1.) Zn + Cu(NO 3 ) 2 → Cu + Zn(NO 3 ) 2 Double- Replacement Rxn Answer: Single- Replacement Rxn 2.) Magnesium Chloride + Silver Nitrate → Combustion Rxn Answer: Double Replacement Rxn: Magnesium Chloride + Silver Nitrate → Magnesium Nitrate + Silver Chloride MgCl 2 + AgNO 3 → Mg(NO 3 ) 2 + AgCl

10. 4.) 4 Fe (s) + 3 O 2 (g) → 2 Fe 2 O 3 (s) Synthesis Rxn Answer: Synthesis Rxn/Combustion Rxn – These are the only type of reactions that can go together. 5.) 2Al (s) + 3S (s) → Al 2 S 3 (s)Combustion Rxn Answer: Synthesis Rxn 3.) NaClO 3 → NaCl + O 2 Synthesis Rxn Answer: Decomposition Rxn