1. Types of Reactions

2. Types of Reactions
There are five types of chemical reactions we will talk about.
Combustion reactions
Synthesis reactions
Decomposition reactions
Single replacement reactions
Double replacement reactions

3. __CH3CH2OH + __O2  __CO2 + __H2O
Who wants to see a demo? 1 2 7 4 2 3 6
__CH3CH2OH + __O2  __CO2 + __H2O
3.5
x 2

4. Combustion Reactions
occur when a hydrocarbon reacts with oxygen gas (a.k.a. burning)
need the 3 things in the “fire triangle”: 1) A Fuel (hydrocarbon) 2) Oxygen to burn it with 3) Something to ignite the reaction (spark)

5. Combustion Formula: CxHy + O2  CO2 + H20
Look for a Hydrocarbon and O2 in the reactants
Look for CO2 and H2O in the products

6. __C4H4 + __O2  __C4H8 + __O2  __C4H10 + __O2 
Practice:
__CO2 + __H2O __CO2 + __H2O __CO2 + __H2O
__C4H4 + __O2  __C4H8 + __O2  __C4H10 + __O2  1 5 4 2 6 4 4 1 2 1 8 4 10 5 13
6.5 x2 x2 x2 x2

7. DEMO
__Mg + __O2  __MgO

8. Synthesis reactions A + B  AB
Analogy: marriage, baking
occur when two substances (generally elements) combine and form a compound
(sometimes these are called combination or
addition reactions)
reactant + reactant  1 product
Example: 2H2 + O2  2H2O
Example: C + O2  CO2

9. Al+3 O-2 3 2 4 2 Na+1 I-1 2 1 2 Practices __ Al2O3
__ O2 (g) + __ Al (s)  __ Na (s) + __ I2 (l) 
Na+1 I-1
__ NaI 2 1 2

10. Wanna see a gummy bear dance?2 2 3
__KClO3  __KCl + __O2

11. Decomposition Reactions AB  A + B
Analogy: divorce
occur when a compound breaks up into the elements or to simpler compounds
1 Reactant  Product + Product
Example: 2 H2O  2H2 + O2
Example: 2 HgO  2Hg + O2

12. 2 2 4 3 2 1 2 2 1 2 Diatomic! Practices Practice 1: __ Al2O3 (s) 
Practice 2: __ CuO (s) 
Practice 3: __ H2O (l) 
___ Al +
___ O2 2 1 2
___ Cu +
___ O2 2 1 2
___ H2 +
___ O2
Diatomic!

13. Another demo, shall we?
___ Cu + ___ AgNO3  ___Ag + ___Cu(NO3)2

14. Single Replacement Reactions A + BC  AC + B (if A is metal)
Analogy: “homewrecker”
occur when one element replaces another
in a compound
A metal can replace a metal (ca+ion)
element + compound product + product
Zn HCl  ZnCl2 + H2
Prediction:
First identify if the single element is a METAL (will replace the cation in the compound)
Next, is the single element more reactive than the one it is trying to replace?
Look at “Activity Series of Metals” list

15. 1 2 1 1 1 2 1 1 NR   Practices Homework:
___ Mg (s) + ___ HNO3 (aq) 
___ Zn (s) + ___ HCl (l) 
___ FeBr3 (s) + ___ Ag (s) 
Homework:
Practice – Single Replacement
Determine reaction or no reaction (NR)
If reaction, balance
___ H2 + ___ Mg(NO3)2 1 2 1 1
___ H2 + ___ ZnCl2 NR  

16. One more demo…
___Pb(NO3)2 + ___KI  ___PbI2 + ___KNO3 1 2 1 2

17. Double Replacement Reaction AB + CD  AD + CB
Analogy: Flintstones couple switch
occur when a metal replaces a metal in a compound or a nonmetal replaces a nonmetal in a compound
compound + compound  product + product
Ex: AgNO3(aq) + NaCl(s)  AgCl(s) + NaNO3(aq)

18. Double Replacement Reactions
Think about it like “foil”ing in algebra, first and last ions go together & inside ions go together
Example:
AgNO3(aq) + NaCl(s)  AgCl(s) + NaNO3(aq)
Another example:
K2SO4(aq) + Ba(NO3)2(aq)  KNO3(aq) + BaSO4(s) 2

19. Prediction break both compounds into their CATIONS and ANIONS
trade partners & write your two new formulas but REMEMBER:
CA+ION always goes first
Assign charges; SWAP & DROP.
If one reactant ends in (OH) and one starts w/ H one of the products is water (H2O)
Test solubility and see which product is the precipitate (if any) and which stays in solution (aq).
if both stayed in solution (aq) we would write NO REACTION

20. YES NO AgNO3(aq) + NaCl(s)  AgCl(s) + NaNO3(aq) Precipitate formed?

21. KBr(aq) + AlPO4(aq)  K3PO4(aq) + AlBr3(aq)
Precipitate formed? NO

22. Acid-Base (Neutralization)
A special kind of double replacement
ACID + BASE  Salt + H2O (l)
Ex. HCl + NaOH → NaCl + H2O
Ex. H2SO4 + Mg(OH)2 →
MgSO4
+ H2O

23. Practice 2 1 1 1
1. __CaCO3 + __HCl → 2. __KOH + __H2SO4 → 3. __Pb(NO3)2 + __K2S →
__CaCl2 +
__H2CO3 2 1 1 2
__K2SO4 +
__H2O 1 1 2 1
__KNO3 +
__PbS

24. Classify each: synthesis single repl. combustion decomposition
CaO + H2O ----> Ca(OH)2
Cl2 + KBr ----> KCl + Br2
CH4 + O2 ----> H2O + CO2
Ag2O ----> Ag + O2
AgNO3 + NaCl ----> AgCl + NaNO3
single repl.
combustion
decomposition
double repl.