1. Types of Chemical Reactions What you got, fool?

2. Chemical Reactions, a Review Chemical reactions are the processes that take place that form new and different compounds. Chemical equations use symbols and formulas to describe the reactions. Law of Conservation of Matter states that matter cannot be created or destroyed. (but you knew that already)

3. Reactants vs. Products Reactants are on the left of the arrow. –They are what you start with. Products are on the right of the arrow. –They are what you end up with. The arrow means yield, produces, makes. Based on the reactants, you can tell which type of chemical reaction you have!

4. 5 Types of Reactions There are thousands upon thousands of reactions that occur everyday. Lucky for you, they fall into 5 main categories: 1.Combination 2.Decomposition 3.Single Replacement 4.Double Replacement 5.Combustion

5. Combination Reactions Combine = to put together. These reactions will occur when 2 different substances come together to make a compound. Also called synthesis (to make). Ca + O 2  CaO(is it balanced?) Al + Cl 2  AlCl 3 (is is balanced?)

6. The Reactants Involved Most often reactants are 2 elements. Nonmetal oxides (nonmetal hooked to oxygen) react with water to produce an acid (acids start with H): SO 3 + H 2 O  H 2 SO 4 (acid rain) Metallic oxides (metal hooked to oxygen) react with water to produce a base (bases have OH): CaO + H 2 O  Ca(OH) 2

7. Decomposition Reaction Decompose = to break apart These reactions involve one compound breaking down into simpler pieces. Energy (electricity, heat, light, etc.) is usually required for these reactions to happen. NaCl Na + Cl 2 CaCO 3 CaO + CO 2 electricity ∆

8. Single Replacement Reactions Single = 1 Replace = to take the place of These reactions occur when one element takes the place of another element in a compound. Reactants must be an element and a compound. Na + KCl  K + NaCl (cations switch) F 2 + LiCl  LiF + Cl 2 (anions switch)

9. Double Replacement Reaction Double = 2 Replace = to take the place of These reactions occur when two ions take the place of others (2 things switch). Reactants must be 2 ionic compounds in aqueous solutions. NaOH + FeCl 3  Fe(OH) 3 + NaCl (is it balanced?)

10. Combustion Reactions Combust = to burn in the presence of oxygen These reactions occur when a compound made of C and H (sometimes also O) reacts with oxygen This is what happens when things burn. C 4 H 8 + O 2  CO 2 + H 2 O (is it balanced?)

11. Products of Combustion When a hydrocarbon (C, H, and sometimes O) burns, it always produces H 2 O. If it burns completely, the other product is CO 2. If combustion is incomplete (maybe you didn’t give it enough oxygen), the other product will be CO, or maybe even just C. **We are usually going to assume the products are CO 2 or CO in this class…

12. General Rules A + B  AB Combination (there are a few exceptions) AB  A + BDecomposition A + BC  B + AC Single Replacement AB + CD  AD + CB Double Replacement C x H y + O 2  CO 2 + H 2 O Combustion

13. Yay Practice! Name the type of reaction present just by looking at the reactants: 1.H 2 + O 2  2.H 2 O  3.Zn + H 2 SO 4  4.HgO  5.KBr + Cl 2  6.AgNO 3 + NaCl  7.C 10 H 8 + O 2  8.Mg(OH) 2 + H 2 SO 3  Combination Decomposition Single Replacement Decomposition Single Replacement Double Replacement Combustion Double Replacement