 Single displacement reactions only occur when the displaced element is less reactive than the one replacing it.  We can predict if a reaction will occur by comparing the involved elements on the activity series.

Fe (s) + CuSO 4(aq)  FeSO 4(aq) + Cu (s) iron + copper (II) sulfate  iron (II) sulfate + copper This reaction occurs because iron donates its electrons more readily than copper (iron is more reactive). Fe (s) + AlCl 3(aq)  No Reaction Iron is less reactive than aluminum.

Cl 2(g) + 2NaBr (aq)  2NaCl (aq) + Br 2(g) Chlorine is more reactive than bromine, so this reaction occurs. Cl 2(g) + 2NaF (aq)  no reaction Chlorine is less reactive than fluorine, so no reaction occurs. We will show that no reaction occurs by simply writing “NR” on the products side of an equation.

 Cations exchange places in aqueous solutions.  General formula: AX + BY  AY + BX

 A reaction may form a solid (precipitate) Cu(NO 3 ) 2(aq) + AgCl (aq)  CuCl 2(aq) + AgNO 3(s)  We can predict if a precipitate will form by referring to a set of solubility guidelines that have been established based on experimental results

Anion+ Cation  Solubility of Compound 1MostAlkali metal ions (Li +, K +, Rb +, Cs +, Fr + )Soluble MostHydrogen ion (H + )Soluble MostAmmonium ion (NH 4 + )Soluble 2Nitrate (NO 3 - )MostSoluble Acetate (CH 3 COO - )Ag + Low solubility Most othersSoluble 3Chloride (Cl - ) Bromide (Br - ), Iodide (I - ) Ag +, Pb +, Hg 2 +, Cu +, Tl + Low solubility All othersSoluble 4.4. Flouride (F - )Mg 2+, Ca 2+, Ba 2+, Pb 2+ Low solubility Most othersSoluble 5.5. Sulfate (SO 4 2- )Ca 2+, Sr 2+,Ba 2+, Pb 2+ Low solubility Most othersSoluble 6.6. Sulfide (S 2 - )Alkali ions and H +, NH 4 +, Be 2+, Mg 2+, Ca 2+, Sr 2+, Ba 2+ Soluble All othersLow solubility 7Hydroxide (OH - )Alkali ions and H +, NH 4 +, Sr 2+, Ba 2+, Tl + Soluble All othersLow solubility 8Phosphate (PO 4 3- )Alkali ions and H +, NH 4 + Soluble All othersLow solubility

 Magnesium chloride and lead (II) acetate form a precipitate. Predict the products and write a balanced equation identifying the precipitate.

1. Identify the ions that make up each reactant. Magnesium chloride: Mg 2+, Cl - Lead acetate: Pb 2+, CH 3 COO - 2. Switch the pairs of ions to determine the products, and write the equation. MgCl 2(aq) + Pb(CH 3 COO) 2(aq)  Mg(CH 3 COO) 2 + PbCl 2

3. Use the solubility guidelines to determine the precipitate. Acetate is soluble with magnesium Lead (II) ions have low solubility with chloride ions. Therefore PbCl 2 is solid. MgCl 2(aq) + Pb(CH 3 COO) 2(aq)  Mg(CH 3 COO) 2(aq) + PbCl 2(s)

 A reaction may form a gas NaOH (aq) + NH 4 Cl (aq)  HOH (l) + NaCl (aq) + NH 3(g)  A reaction may form water H 2 SO 4(aq) + 2 NaOH (aq)  2 HOH (l) + Na 2 SO 4(aq)

If one reactant…+ the other reactant…  then the products include is an aqueous salt a precipitate is an acidhas carbonate ionswater and carbon dioxide has ammonium ionshas hydroxide ionswater and ammonia is an acidhas hydroxide ionswater

 Neutralization Reactions: Specific type of double displacement reaction involving acids and bases: General Formula: acid + base  salt + water Example: HCl + NaOH  NaCl + HOH

 Combustion Reactions: Oxygen combines with another substance to produce energy (heat and light) and one or more oxides

 Hydrocarbon Combustion: Complete Combustion:  A hydrocarbon reacts with an abundant amount of oxygen gas to produce water and carbon dioxide Incomplete Combustion:  A hydrogen combustion reaction with a poor supply of oxygen which produces any combination of CO 2, H 2 O, CO and C (soot)

 Oxides and Water: Metal oxides combine with water to produce hydrogen gas and metallic hydroxides.  The resulting metallic hydroxide solution is a basic solution.  BaO(s) + 2 H 2 O (l)  H 2 (g) + Ba(OH) 2 (aq)  Na 2 O(s) + 2 H 2 O (l)  H 2 (g) + 2 NaOH (aq)

Non-metallic oxides combine with water to produce acidic solutions (oxyacids). CO 2 (g) + H 2 O (l)  H 2 CO 3 (aq) P 4 O 10 (s) + 6 H 2 O (l)  4 H 3 PO 4 (aq)

 Complete worksheet on Reaction Prediction.  Check your answers AFTER you have completed your work.