1. Types of REACTIONS + solubility

2. Chemical Equations In a chemical equation the physical state can be represented by a letter; –Gas = g –Liquid = l –Solid = s –Vapour = v –Aqueous = aq A Catalyst is a substance that speeds up a reaction without being used up itself (they are shown by writing above the arrow)

3. Reaction Types Combination/ synthesisR + S  RS DecompositionRS  R + S Single-replacement T + RS  TS + R Double-replacement RS + TU  RU + TS CombustionC ? H ? + O 2  CO 2 + H 2 O

4. How to Write a Balanced Equation 1 Write a word equation that includes all reactants and products 2 Write the formulae for all substances involved (to make an unbalanced equation). 3 Balance the equation by putting numbers in front of symbols or formulae. Start with elements that occur in one place only on each side of the equation. 4 Add symbols for the physical states, (s), (l), (g), (aq).

6. 1.Identify which type of reaction each of the following are; a.SnF 4 + H 2 SO 4  Sn(SO 4 ) 2 + HF b.Li + + O 2  Li 2 O c.Al 2 O 3  Al 3+ + O 2 d.C 3 H 8 + O 2  CO 2 + H 2 O e.BeSiO 3 + Cl -  BeCl 2 + SiO 3 2- 2.Balance each of the equations above 3.Balance the following equations a.Li + + SO 4 2-  Li 2 SO 4 b.AlCl 3  Al 3+ + Cl 2 c.BeS + Cl -  BeCl 2 + S 2- d.FeF 3 + H 2 SO 4  Fe 2 (SO 4 ) 3 + HF e.C 3 H 6 + O 2  CO 2 + H 2 O 1.. a.Double replacement b.Combination c.Decomposition d.Combustion e.Single replacement 2.. a.SnF 4 + 2H 2 SO 4  Sn(SO 4 ) 2 + 4HF b.4Li + + O 2  2Li 2 O c.2Al 2 O 3  4Al 3+ + 3O 2 d.C 3 H 8 + 5O 2  3CO 2 + 4H 2 O e.BeSiO 3 + 2Cl -  BeCl 2 + SiO 3 2- 3.. a.2Li + + SO 4 2-  Li 2 SO 4 b.2AlCl 3  2Al 3+ + 3Cl 2 c.BeS + 2Cl -  BeCl 2 + S 2- d.2FeF 3 + 3H 2 SO 4  Fe 2 (SO 4 ) 3 + 6HF e.2C 3 H 6 + 9O 2  6CO 2 + 6H 2 O

7. Solublity Rules (insoluble = formation of precipitate in solution) All compounds containing either the Na +, NH 4 +, K +, or NO 3 - ion will dissolve in water Compounds containing the Cl -, Br - and I - ions are soluble (except when they contain Ag +, Pb 2+ or Hg 2+ ions) Compounds containing the SO 4 2- ions are soluble (except when they contain Ba 2+, Pb 2+ or Ca 2+ ions) Compounds containing CO 3 2- and PO 4 3- are insoluble except when they contain Na +, NH 4 + or K + ions) Compounds containing OH - are insoluble (except when they contain Na +, NH 4 +, or K + ions) Some compounds are slightly soluble; Ca(OH) 2, PbCl 2, PbBr 2, CaSO 4 and Ag 2 SO 4

8. Reactivity series of Metals A single replacement reaction will only happen if the free metal is more reactive than the bonded metal Li, K, Ba, Ca, Na, Mg, Al, Zn, Cr, Fe, Cd, Co, Ni, Sn, Pb, H 2, Cu, Hg, Ag, Au (most  least reactive) Eg. If T + RS  TS + R, then T must be more reactive than R

9. 1.Predict whether each of the following are soluble or not a.BaSO 4 b.PbCO 3 c.AgCl 2 d.Ca(OH) 2 e.AlPO 4 f.NaBr 2.Predict whether the following reactions will occur a.Li + H 2 SO 4  b.Cr 2+ + AlCl 3  c.BaS + Ag 2+  d.H 2 + AuCO 3  3.Complete and balance the equations in Q2 1.. a.Insoluble b.Insoluble c.Soluble d.Slightly Soluble e.Insoluble f.Soluble 2.. a.Yes b.No c.No d.Yes 3.. a.2Li + + H 2 SO 4  Li 2 SO 4 + H 2 b.3Cr 2+ + 2AlCl 3  No Reaction c.BaS + Ag 2+  No Reaction d.H 2 + AuCO 3  H 2 CO 3 + Au 2+