1. Types of Reactions

2. Synthesis Decomposition Single-replacement Double-replacement Combustion

3. Reaction Classification Reactions are classified based on the: Type of reactant Number of reactants Number of products

4. Synthesis Reactions 2+ substances react to form a single substance The reactants may be single elements or compounds The product is always a compound A + B → AB

5. Synthesis Reactions Examples: 2Na + Cl 2 → 2NaCl (table salt) Sodium reacts with chlorine to form sodium chloride. 2H 2 + O 2 → 2H 2 O (water) Hydrogen reacts with oxygen to form dihydrogen monoxide or water.

6. Decomposition Reactions The opposite of synthesis reactions A compound breaks down into 2+ simpler substances. The reactant must be a compound. The products may be single elements or compounds. AB → A + B

7. Decomposition Reactions Examples: 2H 2 O → 2H 2 + O 2 Water breaks down into hydrogen and oxygen. CaCO 3 → CaO + CO 2 Calcium carbonate breaks down into calcium oxide and carbon dioxide.

8. Single Replacement Reactions 1 element takes the place of another element in a compound A + BC → B + AC

9. Single Replacement Reactions Examples: Cu + 2AgNO 3 → 2Ag + Cu(NO 3 ) 2 Copper reacts with silver (I) nitrate and replaces silver to form copper (II) nitrate and silver. 2K + 2H 2 O → H 2 + 2KOH Potassium reacts with dihydrogen monoxide and replaces a hydrogen to produce potassium hydroxide and hydrogen.

10. Double Replacement Reactions 2 different compounds exchange positive ions and form 2 new compounds AB + CD → AD + CB

11. Double Replacement Reactions Examples: Pb(NO 3 ) 2 + 2KI → PbI 2 + 2KNO 3 Lead (II) nitrate reacts with potassium iodide to form lead (II) iodide and potassium nitrate. CaCO 3 + 2HCl → CaCl 2 + H 2 CO 3 Calcium carbonate reacts with hydrogen monochloride to form calcium chloride and dihydrogen carbonate.

12. Combustion Reactions A substance reacts rapidly with oxygen Often heat and light are produced This is what happens when gas is burned to power cars or fireplaces or Bunsen burners.

13. Combustion Reactions Examples: CH 4 + 2O 2 → CO 2 + 2H 2 O + heat Carbon tetrahydride or methane reacts with oxygen to produce carbon dioxide, water, and heat. 2H 2 + O 2 → 2H 2 O This can also be called a synthesis reaction. Sometimes classifications can overlap. Hydrogen reacts with oxygen to produce water and heat.

14. Questions! What type of reaction is it if: 1. Oxygen is a reactant? 2. 2 reactants form 1 product? 3. 1 reactant forms 2 products? 4. Both the reactants and products contain 2 compounds? 5. Both the reactants and products contain 1 compound and 1 single element?

15. Answers! 1. Combustion 2. Synthesis 3. Decomposition 4. Double replacement 5. Single replacement

16. Oxidation-Reduction Reactions Electrons are transferred from 1 reactant to another Also called redox reactions This was the last reaction discovered because it is based on subatomic particle (electron) transfer that was not originally known about.

17. Oxidation Any process in which an element loses electrons during a chemical reaction. A reactant is oxidized if it loses electrons. Originally scientists thought that oxygen had to be present for this to happen. Now we know that several elements are capable of taking electrons.

18. Oxidation Examples: 2Ca + O 2 → 2CaO Calcium loses electrons to oxygen and forms calcium oxide. Na + Cl → NaCl Sodium loses electrons to chlorine and forms sodium chloride.

19. Reduction The process in which an element gains electrons during a chemical reaction. A reactant is said to be reduced if it gains electrons. Oxidation and reduction ALWAYS occur together because when 1 element loses electrons the other element gains them.