1. 6 Basic Types of Reactions
Combination (Synthesis)
Decomposition
Single replacement
Double replacement
Neutralisation
Combustion

2. Combination Reactions
reactants join together to form a single product

3. Magnesium burns in Oxygen

4. Decomposition Reactions
Products split to form 2 or more reactants

5. Electrolysis of water

6. Decomposition of Hydrogen Peroxide

7. Single Replacement Reaction
A single compound replaces one element for another
(ie. Metals swap positions)
AB + C  AC + B

8. Hydrochloric Acid with Mg metal

9. Double Replacement Reaction
When two ionic compounds swap ions with each other (eg. Cations swap places)
AB + CD  AD + CB

10. Precipitation Reactions

11. Potassium iodide + lead nitrate
 Lead nitrate + potassium iodide

12. Which one forms a precipitate?
Soluble = dissolves, no precipitate (aq)
Low solubility = forms a solid precipitate (s)

13. Solubility Table (pg. 152)

14. Writing the chemical equation:

15. ___NaOH + ____Pb(NO3) 2 ___ Pb(OH) 2 + ___ NaNO3
Balance the Equation
___NaOH + ____Pb(NO3) ___ Pb(OH) 2 + ___ NaNO3
Balance order:
1st metals
2nd any groups (in brackets)
3rd non-metals
4th oxygen or hydrogen last

16. Neutralisation Reaction
A special type of double replacement reaction involving an acid and base to form an ionic salt and water
Eg. HBr + LiOH 

17. Combustion Reaction

18. Gasoline vs Diesel

19. Balance the reaction:
hexane + oxygen  carbon dioxide + water C6H14 (l) + O2 (g)  CO2 (g) + H20 (g)