1. Which is which???

2.  Synthesis—when two or more different reactants combine to form one product  Example ◦ 2Mg + O 2  2MgO  Decomposition—when one reactant breaks up into two or more products  Example ◦ H 2 CO 3  CO 2 + H 2 O

3.  Single-replacement—a reaction in which an element reacts with a compound and replaces another element in the compound  Example ◦ Mg + 2HCl  2MgCl 2 + H 2  Double-replacement reaction—a reaction in which there is an exchange of positive ions between two compounds. These reactions generally take place between two ionic compounds.  Example ◦ Al 2 (SO 4 ) 3 + 3Ba(OH) 2  2Al(OH) 3 + 3BaSO 4

4.  Combustion—a reaction in which a substance reacts with oxygen, usually with the rapid release of heat and the production of a flame. Organic compounds usually burn in the oxygen in air to produce carbon dioxide and water.  Example ◦ 2 C 4 H 10 + 13 O 2  8 CO 2 + 10 H 2 O

5.  Combustion—a reaction in which a substance reacts with oxygen, usually with the rapid release of heat and the production of a flame. Organic compounds usually burn in the oxygen in air to produce carbon dioxide and water. Always the same  Example ◦ 2 C 4 H 10 + 13 O 2  8 CO 2 + 10 H 2 O ◦ THE PRODUCTS ARE CARBON DIOXIDE AND WATER

6.  Each of the following slide will have a chemical equation on it. You will use your clickers to classify said reaction. 1. Synthesis 2. Decomposition 3. Single replacement 4. Double replacement 5. Combustion

7.  The reaction ◦ 2H 2 +O 2  2H 2 O 1. Synthesis 2. Decomposition 3. Single replacement 4. Double replacement 5. Combustion

8.  The reaction ◦ 2HgO  2Hg + O 2 1. Synthesis 2. Decomposition 3. Single replacement 4. Double replacement 5. Combustion

9.  The reaction ◦ Zn + 2HCl  ZnCl 2 + H 2 1. Synthesis 2. Decomposition 3. Single replacement 4. Double replacement 5. Combustion

10.  The reaction ◦ 2C 7 H 6 O 2 +17O 2  6H 2 O + 14CO 2 1. Synthesis 2. Decomposition 3. Single replacement 4. Double replacement 5. Combustion

11.  The reaction ◦ LiCl + AgNO 3  LiNO 3 + AgCl 1. Synthesis 2. Decomposition 3. Single replacement 4. Double replacement 5. Combustion

12.  The reaction ◦ Fe 2 O 3 + 3H 2  2Fe +3H 2 O 1. Synthesis 2. Decomposition 3. Single replacement 4. Double replacement 5. Combustion

13.  The reaction ◦ P 4 O 10 + 6H 2 O  4H 3 PO 4 1. Synthesis 2. Decomposition 3. Single replacement 4. Double replacement 5. Combustion

14.  The reaction ◦ N 2 + 3H 2  2NH 3 1. Synthesis 2. Decomposition 3. Single replacement 4. Double replacement 5. Combustion

15.  The reaction ◦ Ca(OH) 2 + CuCl 2  Cu(OH) 2 +CaCl 2 1. Synthesis 2. Decomposition 3. Single replacement 4. Double replacement 5. Combustion

16.  The reaction ◦ 4Al + 3O 2  2Al 2 O 3 1. Synthesis 2. Decomposition 3. Single replacement 4. Double replacement 5. Combustion

17.  The reaction ◦ P 4 + 5O 2  2P 2 O 5 1. Synthesis 2. Decomposition 3. Single replacement 4. Double replacement 5. Combustion

18.  The reaction ◦ C 5 H 12 + 8O 2  5CO 2 + 6H 2 O 1. Synthesis 2. Decomposition 3. Single replacement 4. Double replacement 5. Combustion

19.  The reaction ◦ N 2 O 5 + H 2 O  2HNO 3 1. Synthesis 2. Decomposition 3. Single replacement 4. Double replacement 5. Combustion

20.  The reaction ◦ 2Al(OH) 3 + 3H 2 SO 4  Al 2 (SO 4 ) 3 + 6H 2 O 1. Synthesis 2. Decomposition 3. Single replacement 4. Double replacement 5. Combustion