2. Synthesis Reaction Two or more substances combine to form a more complex substance 2 Mg (s) + O 2 (g) 2 MgO (s)

3. Decomposition Reaction: A complex substance breaks down into its parts One reactant yields (forms) 2 or more products SYNTHESIS and DECOMPOSITION reactions are OPPOSITES + turtle eggturtleegg shell CaCO 3 (s)CaO (s) + CO 2 (g)

4. Single Replacement Reaction: A single uncombined element replaces another in a compound Two reactants yield two products Zn (s) + 2 HCl (aq)ZnCl 2 (aq) + H 2 (g)

5. Double Replacement Reaction: Parts of two compounds switch places to form two new compounds Two reactants yield two products. They’ve swapped their ‘cats’! Al 2 (SO 4 ) 3 + 6 NH 4 OH 3 (NH 4 ) 2 SO 4 + 2Al(OH) 3

6. Reactants: oxygen gas and a hydrocarbon Products: CO 2 and H 2 O ___ C 6 H 6 + ___ O 2 ___ CO 2 + ___ H 2 O63215126 Balance carbons Balance hydrogens Check oxygen count 12 + 3 = 15 oxygens  Odd number of oxygens, so multiply through by 2 24 + 6 = 30 oxygens

7. Zn (s) + 2 HCl (aq)ZnCl 2 (aq) + H 2 (g) Cu (s) + 2 AgNO 3 Cu(NO 3 ) 2 + 2 Ag (s) Note that the reactions won’t work the other way around!!! The reaction only takes place if the element on the reactant side is ‘hotter’ than the element that ends up being formed. The higher up on the activity series the element is, the ‘hotter’ it is.

8. Single Replacement Reaction: A single uncombined element replaces another in a compound Two reactants yield two products Zn (s) + 2 HCl (aq)ZnCl 2 (aq) + H 2 (g)

9. Metals Lithium Potassium Calcium Sodium Magnesium Aluminum Zinc Chromium Iron Nickel Tin Lead Hydrogen* Copper Mercury Silver Platinum Gold Halogens Fluorine Chlorine Bromine Iodine Decreasing Activity

10. Double Replacement Reaction: Parts of two compounds switch places to form two new compounds Two reactants yield two products. They’ve swapped their ‘cats’! Al 2 (SO 4 ) 3 + 6 NH 4 OH 3 (NH 4 ) 2 SO 4 + 2Al(OH) 3

11. Reactants: oxygen gas and a hydrocarbon Products: CO 2 and H 2 O ___ C 6 H 6 + ___ O 2 ___ CO 2 + ___ H 2 O63215126 Balance carbons Balance hydrogens Check oxygen count 12 + 3 = 15 oxygens  Odd number of oxygens, so multiply through by 2 24 + 6 = 30 oxygens

12. + Synthesis/Combination Decomposition Single-Replacement  Activity Series A + B AB AB A + B A + BC AC + B

13. Double-Replacement  Solubility Rules Combustion O2O2 ++ hydrocarbon CO 2 H2OH2OO2O2 AB + CD CB + AD

14. A redox reaction is one in which the reactants’ oxidation numbers change. What are the oxidation numbers of the metals in the reaction below? 2 FeCl 3 + SnCl 2  2 FeCl 2 + SnCl 4 +3+2 +4 The iron’s charge has become more negative, so it is reduced. The tin’s charge has become more positive, so it is oxidized. reduced oxidized 0 +2 +4 +6 +8 -2 -6 -4 0 +2 +4 +6 +8 -2 -6 -4 Fe Sn x + 3(-1) = 0 x + 2(-1) = 0 x + 4(-1) = 0

15. Which reactant is oxidized and which is reduced in the following? 2) Cu + 2AgNO 3  Cu(NO 3 ) 2 + 2Ag 0+1+20 reduced oxidized 1) Cl 2 + SnCl 2  SnCl 4 0 reduced oxidized +2+4 3) 2KClO 3  2KCl + 3O 2 -20 +5 reduced oxidized Synthesis Single-replacement Decomposition Note that a redox reaction can also be another type of reaction. +1 + x + 3(-2) = 0