1. Section 2 - Types of Reactions Classify 5 major types. Predict the products For some, we will be able to predict whether or not they will happen at all.

2. How to recognize which type Look at the reactants: A + B  AB Combination (Synthesis) AB  A + B Decomposition AX + B  A + BX Single Replacement AX + BY  AY + BX Double replacement C x H y + O 2  CO 2 + H 2 O Combustion

3. Combination (Synthesis) A + B  AB H 2 + O 2  H 2 O Ca +O 2  CaO SO 3 + H 2 O  H 2 SO 4 We can predict the products if the reactants are two elements. Mg + N 2 

4. Decomposition To break apart AB  A + B H 2 O  H 2 + O 2 one reactant breaks apart into two or more elements or compounds. NaCl  Na + Cl 2 CaCO 3  CaO + CO 2 Note that energy (heat, sunlight, electricity, etc.) is usually required

5. Combination Mg + O 2  Na + Cl 2  Decomposition H 2 O  HgO 

6. Single-Replacement Reaction A + BX  AX + B One element replaces another Reactants must be an element and a compound. Products will be a different element and a different compound. Na + KCl  K + NaCl F 2 + LiCl  LiF + Cl 2

7. Single-Replacement Reaction Only more reactive metals can replace a metal already in solution. The activity series (p. 333) lists the relative reactivity of metals. Higher on the list replaces lower metals.

8. The Activity Series of the Metals Lithium Potassium Calcium Sodium Magnesium Aluminum Zinc Chromium Iron Nickel Lead Hydrogen Bismuth Copper Mercury Silver Platinum Gold 1)Metals can replace other metals provided that they are above the metal that they are trying to replace. The single metal is above the metal in the compound If it isn’t, there is no reaction 2)Metals above hydrogen can replace hydrogen in acids. 3)Metals from lead upward can replace hydrogen in water. Higher activity Lower activity

9. Double-Replacement Reaction Two things replace each other. AX + BY  AY + BX NaOH + FeCl 3  Fe(OH) 3 + NaCl –Reactants must be two ionic compounds. –Usually in aqueous solution

10. Double Replacement Has certain “driving forces” –Will only happen if one of the products: a) doesn’t dissolve in water and forms a solid (a “precipitate”), or b) is a gas that bubbles out, or c) is a molecular compound (usually water). CaCl 2 + NaOH  KOH + Fe(NO 3 ) 3 

11. Complete and Balance CaCl 2 + NaOH  KOH + Fe(NO 3 ) 3 

12. Single-Replacement Zn + H 2 SO 4  KBr +Cl 2  Double Replacement AgNO 3 + NaCl  Mg(OH) 2 + H 2 SO 3 

13. Combustion Reaction Means “add oxygen” C x H y + O 2  CO 2 + H 2 O Normally, a compound composed of only C, H, (and maybe O) is reacted with oxygen – usually called “burning” If the combustion is complete, the products will be CO 2 and H 2 O. If the combustion is incomplete, the products will be CO (or possibly just C) and H 2 O.

14. Combustion Reaction Examples C 4 H 10 + O 2  H 2 O + CO 2 C 4 H 10 + O 2  H 2 O + CO C 6 H 12 O 6 + O 2  (complete) C 8 H 8 +O 2  (incomplete)

15. Combustion (complete) C 6 H 12 O 6 + O 2  C 3 H 8 + O 2