1. Types of Chemical Reactions

2. Classifying Reactions
The five general types of reaction are combination (synthesis), decomposition, single-replacement, double-replacement, and combustion.

3. Combination Reactions
Combination reactions are also called synthesis reactions.
A combination reaction is a chemical change in which two or more substances react to form a single new substance.
2Mg + O2  2MgO

4. Combination Reactions
13. Complete and balance this equation for a combination reaction:
Be + O2 
14. write and balance the equation for the formation of strontium iodide (SrI2) from its elements.

5. Decomposition Reactions
A decomposition reaction is a chemical change in which a single compound breaks down into two or more simpler products.
Decomposition reactions involve only one reactant and two or more products.
The products can by any combination of elements and compounds.

6. Decomposition Reactions
15. complete and balance this decomposition reaction.
HI
16. Write the formula for the binary compound that decomposes to the products H2 and Br2.

7. Single Replacement Reactions
A single-replacement reaction is a chemical change in which one element replaces a second element in a compound.
2K(s) + 2H2O(l)  2KOH(aq) + H2(g)

8. Single Replacement Reactions
You can identify a single-replacement reaction by noting that both the reactants and the products consist of an element and a compound.

9. Single Replacement Reactions
Whether one metal will displace another metal from a compound depends upon the relative reactivities of the two metals.
The activity series of metals lists metals in order of decreasing reactivity.

10. Single Replacement Reactions
A reactive metal will replace any metal listed below it in the activity series.
Iron will displace copper from a copper compound in solution, but iron does not similarly displace zinc or calcium.

11. Single Replacement Reactions
A halogen can also replace another halogen from a compound.
The activity of the halogens decreases as you go down Group 7A of the periodic table.

12. Single Replacement Reactions
17. Complete the equations for these single-replacement reactions in aqueous solution. Balanace each equations. Write “no reaction” if a reaction does not occur (use the activity series).
A. Fe(s) + Pb(NO3)2(aq) 
B. Cl2(aq) + NaI(aq) 
C. Ca(s) + H2O(l) 

13. Double-Replacement Reactions
A double-replacement reaction is a chemical change involving an exchange of positive ions between two compounds.
Generally takes place in aqueous solution and often produces a precipitate, a gas, or a molecular compound such as water.

14. Double-Replacement Reactions
For a double-replacement reaction to occur, one of the following is usually true:
1. One of the products is only slightly soluble and precipitates from solution.
2. One of the products is a gas.
3. One product is a molecular compound such as water.

15. Double-Replacement Reactions
18. Write the products of these double-replacement reaction. Then balance each equation.
A. NaOH + Fe(NO3)3 
B. Ba(NO3)2 + H3PO4 

16. Combustion Reactions
A combustion reaction is a chemical change in which an element or a compound reacts with oxygen often producing energy in the form of heat and light.
Often one of the reactants is a hydrocarbon, which is a compound composed of hydrogen and carbon.
2C8H O2  16CO2 + 18H2O

17. Combustion Reactions
The reactions between oxygen and some elements other than carbon are also examples of combustion reactions.
2Mg + O2  2MgO
S + O2  SO2

18. Combustion Reactions
20. Write a balanced equation for the complete combustion of each compound.
A. formic acid (HCOOH)
B. heptane (C7H16)

19. Combustion Reactions
21. Write a balanced equation for the complete combustion of glucose (C6H12O6).

20. Predicting the Products of a Chemical Reaction
The number of elements and/or compounds reacting is a good indicator of possible reaction type and possible products.