This document discusses different types of chemical reactions including synthesis, decomposition, single-replacement, double-replacement, combustion, and neutralization reactions. Synthesis reactions involve two or more reactants combining to form a single new product. Decomposition reactions involve a single reactant breaking down into simpler products. The document provides examples of common synthesis and decomposition reactions.

1. Chemical Reactions
Predicting Products of Different
Types of Reactions

2. Classifying Reactions
• Synthesis Reactions (combination)
• Decomposition Reactions
• Single-Replacement Reactions
• Double-Replacement Reactions
• Combustion Reactions
• Neutralization Reactions

3. Synthesis Reactions
• Also called combination reactions
• Two or more substances react to form a single
new substance
• Only 1 product in the reaction
• A + B AB

4. • 2 elements react to produce a binary
compound
– 2Na + Cl2 2NaCl
– 2Mg + O2 2MgO
– S + O2 SO2
• Metal oxide + water metal hydroxide
– CaO + H2O Ca(OH)2
• Nonmetal oxide + water oxyacid
– SO3 + H2O H2SO4

5. 1. Ca + F2
2. N2O5 + H2O
3. MgO + H2O
4. Al + O2
5. SO3 + H2O
6. K + O2
7. Li + N2
8. ZnO + H2O
9. P2O5 + H2O
10. K2O + H2O

6. Decomposition Reactions
• A single compound breaks down into two or
more simpler products
• AB A + B
• Only 1 reactant

7. • Metal chlorates metal chlorides + oxygen
– 2NaClO3 2NaCl + 3O2
• Metal hydroxides metal oxides + water
– Mg(OH)2 MgO + H2O
• Metal carbonates metal oxides + carbon
dioxide
– CaCO3 CaO + CO2
• Oxyacids nonmetalic oxides + water
– H2SO3 SO2 + H2O
• Binary compounds individual elements
– 2NaCl 2Na + Cl2

8. 1. CaCO3
2. AlCl3
3. H2CO3
4. KClO3
5. KOH
6. MgCO3
7. Al(ClO3)3
8. Ag2O
9. Fe(OH)2
10. Al2(CO3)3