1. Types of Chemical Reactions (rxns.)
Types of Chemical Reactions (rxns.)

2. Introduction
Chemical reactions occur when bonds (between the electrons of atoms) are formed or broken
Chemical reactions involve
changes in the chemical composition of matter
(the making of new materials with new properties)
energy changes
Bond breaking absorbs Energy (endothermic process)
Bond making releases Energy (exothermic process)
Symbols represent elements
Formulas describe compounds
Chemical equations describe a chemical reaction

3. Types of Reactions Reactions are classified by their products.
Reactions are classified by their products.
There are five main types of chemical reactions we will talk about:
Synthesis reactions
Decomposition reactions
Single replacement reactions
Double replacement reactions
Combustion reactions
You need to be able to identify the type of reaction and predict the product(s)

4. Steps to Writing Reactions
Some steps for doing reactions:
Identify the type of reaction
Predict the product(s) using the type of reaction as a model
Balance it
Don’t forget about the diatomic elements! (BrINClHOF) For example, Oxygen is O2 as an element.
In a compound, it can’t be a diatomic element because it’s not an element anymore, it’s a compound!

5. Synthesis Reactions Synthesis (meaning to make) are
Synthesis (meaning to make) are
Also called
Direct combination or combination reactions
Addition reactions
typified by their single product.
If you have a reaction in which at least 2 elements or compounds are reacted and produce a single product, the reaction is a synthesis reaction.

6. Synthesis Reactions reactant + reactant  1 product
reactant + reactant  1 product
Basically: A + B  AB
Example: 2H2 + O2  2H2O
Example: C + O2  CO2
Note: Single Product! This is your clue that this is a synthesis or combination reaction.

7. Examples of Synthesis Reactions
2Na + S Na2S
This one is an example of two elements in atomic form (Na and S) combining to form a compound (sodium sulfide).
2H2 + O2 2H2O
In this example, A and B are two elements in molecular form (hydrogen and oxygen molecules), and the product is water, which is simply the chemical combination of hydrogen and oxygen.

8. Examples of Synthesis Reactions
4Fe + 3O Fe2O3
In this example, substance “A” is an element in atomic form (Fe), and substance “B” is an element in molecular form (O2). The result is a direct chemical combination of the two elements (FeO, iron oxide, which is “rust”).
CuO + H2O Cu(OH)2
This is an example where both substances going into the reaction are molecules. The result is what you get when you “add” all of the atoms in the reaction together.

9. Decomposition Reactions
Decomposition reactions are really just the opposite of a synthesis reaction. Remember, if you can make a substance, you should be able to break it back apart into its components. A good way to remember decomposition reactions to to remember what happens when something decomposes. It falls apart!

10. Decomposition Reactions
Decomposition reactions occur when a compound breaks up into the elements or in a few to simpler compounds
1 Reactant  Product + Product
Basically: AB  A + B
Example: 2 H2O  2H2 + O2
Example: 2 HgO  2Hg + O2
Note: Single Reactant! The single reactant is your clue that this is a decomposition reaction.

11. Decomposition Exceptions
Carbonates and chlorates are special case decomposition reactions that do not go to the elements.
Carbonates (CO32-) decompose to carbon dioxide and a metal oxide
Example: CaCO3  CO2 + CaO
Chlorates (ClO3-) decompose to oxygen gas and a metal chloride
Example: 2 Al(ClO3)3  2 AlCl3 + 9 O2
There are other special cases, but we will not explore those in this class

12. Practice
Predict the products. Then, write and balance the following decomposition reaction equations:
Solid Lead (IV) oxide decomposes PbO2(s) 
Aluminum nitride decomposes
2AlN(s)  2Al(s) + N2 (g)
Pb(s) + O2 (g)

13. Single Replacement Reactions
Single replacement reactions occur when one chemical takes the place of another in a reaction. In the typical single replacement reaction, an element trades places with one of the ions in a compound.

14. Single Replacement Reactions
Single Replacement Reactions:
A metal can replace a metal (+) OR a nonmetal can replace a nonmetal (-).
element + compound product + product
A + BC  AC + B (if A is a metal) OR
A + BC  BA + C (if A is a nonmetal)
(remember the cation always goes first!)
When H2O splits into ions, it splits into
H+ and OH- (not H+ and O-2 !!)

15. The Activity Series
Not all single replacement reactions will occur.
This depends upon the location of the elements present in the activity series
Elements above MAY replace elements below; elements below MAY NOT replace elements above them on the series

16. Single Replacement Reactions
Write and balance the following single replacement reaction equation:
Zinc metal reacts with aqueous hydrochloric acid
Zn(s) HCl(aq)  ZnCl2 + H2(g)
Note: Zinc replaces the hydrogen ion in the reaction
[If ZnCl2 + H2(g)  Zn(s) HCl(aq) the reaction WOULD NOT OCCUR because Hydrogen is below zinc on the activity series] 2

17. Single Replacement Reactions
Sodium chloride solid reacts with fluorine gas
NaCl(s) + F2(g)  NaF(s) + Cl2(g)
Note that fluorine replaces chlorine in the compound
Aluminum metal reacts with aqueous copper (II) nitrate
Al(s)+ Cu(NO3)2(aq) Cu(s)+ Al(NO3)3(aq) 2 2

18. Double Replacement Reactions
Double Replacement Reactions
Double replacement reactions are identified by two ions trading places and forming new compounds.

19. Double Replacement Reactions
Double Replacement Reactions occur when a metal replaces a metal in a compound and a nonmetal replaces a nonmetal in a compound
two ions trade places and forming new compounds.
Compound + compound  product + product
AB + CD  AD + CB
Notice that one ion from compound AB replaces one ion from compound CD.

20. 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(aq)  AgCl(s) + NaNO3(aq)
Another example:
K2SO4(aq) + Ba(NO3)2(aq)  KNO3(aq) + BaSO4(s) 2

21. Solubility
For a double replacement reaction to have occurred, a solid (precipitate) MUST be formed
There are rules to determine which of the materials formed is the solid
If no solid is formed, there is said to be no reaction.

22. Figure 8.4: The forming of solid AgCl.

23. You will be given a copy of this!!!!
Solubility Tables
Solubility tables help determine which materials are soluble in water and which are not
In general, Solubility Rules can be summarized as follows
All compounds containing alkali metal cations and the ammonium ion are soluble.
All compounds containing NO3-, ClO4-, ClO3-, and C2H3O2- anions are soluble.
All chlorides, bromides, and iodides are soluble except those containing Ag+, Pb2+, or Hg22+.
All sulfates are soluble except those containing Hg22+, Pb2+, Sr2+, Ca2+, or Ba2+.
All hydroxides are insoluble except compounds of the alkali metals, Ca2+, Sr2+, and Ba2+.
All compounds containing PO43-, S2-, CO32-, and SO32- ions are insoluble except those that also contain alkali metals or NH4+.
You will be given a copy of this!!!!

24. Combustion Reactions
Combustion reactions are the ones that burn (or explode!). There are two types of combustion reactions—complete or incomplete reactions. These reactions are identified by their products. They either produce carbon monoxide and water or carbon dioxide and water.

25. Complete Combustion Reactions
These reactions burn “efficiently” which means they produce carbon dioxide and water. These reactions typically burn cleanly and leave very little residue behind.

26. Combustion Reactions
Combustion reactions occur when a hydrocarbon reacts with oxygen gas.
This is also called burning!!! In order to burn something you 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)

27. Combustion Reactions In general: CxHy + O2  CO2 + H2O
In general: CxHy + O2  CO2 + H2O
Products in combustion are ALWAYS carbon dioxide and water. (although incomplete burning does cause some by-products like carbon monoxide)
Combustion is used to heat homes and run automobiles (octane, as in gasoline, is C8H18)

28. Complete Combustion Reactions
CH4 + O2  CO2 + H2O
They may also be written:
CH4  CO2 + H2O
With O2 written above the arrow
Clues: CO2 (carbon dioxide) in the product along with water O2

29. Combustion
Example
C5H O2  CO2 + H2O
Write the products and balance the following combustion reaction:
C10H O2  8 5 6

30. Incomplete Combustion Reactions
Incomplete combustion reactions occur when something does not burn efficiently. This can cause a lot of harm if the gases produced cannot escape. Carbon monoxide,an odorless and colorless gas, is dangerous. People poisoned by this gas usually become sleepy and can die due to exposure.

31. Incomplete Combustion Reactions
CH4 + O2  CO + H2O + CO2
These reactions may also be written by:
CH4  CO + H2O + CO2
Again, the O2 is usually written over the arrow.
Clue: CO (Carbon monoxide as a product.) O2

32. Predicting Products of Reactions
Completing reactions requires knowledge of the different reaction types (sometimes called mechanisms).
You must first identify the reaction type by the reactants. The only type of reaction that cannot be predicted this way is the combustion reaction since the products are very similar.

33. First Step: Identify reaction type Example: Al + O2 
First Step:
Identify reaction type
Example:
Al + O2 
Clue: 2 elements – Synthesis or combination reaction

34. Second Step:
Write the net ionic equation for the reactants
Al + O2  becomes
Al O2- 

35. Step 3
Using clues, complete reaction taking care to write each formula correctly by checking charges and “criss-crossing” if necessary.
Al + O2  Al3+O2-
Al + O2  Al2O3

36. Predicting Products of Reactions (cont.)
For Single Replacement reactions, check activity series to make sure the reaction goes.
Once you write the molecular equation, you should check for reactants and products that are soluble or insoluble. (Double Replacement only)

37. Reactions in Aqueous Solutions
a.k.a. Net Ionic Equations
Molecular Equations: shows complete formulas for reactants and products
Does not show what happens on the molecular level
Total (or Complete) Ionic Equations: All substances that are strong electrolytes (are soluble and dissociate) are written as their ions.
Some ions participate in the reaction
Some ions do NOT participate in the reaction-called spectator ions.
Net Ionic Equations: show only the ions that participate in the reaction

38. Writing Total Ionic Equations
Once you write the molecular equation (synthesis, decomposition, etc.), you should check for reactants and products that are soluble or insoluble.
We usually assume the reaction is in water
We can use a solubility table to tell us what compounds dissolve in water.
If the compound is soluble (does dissolve in water), then splits the compound into its component ions
If the compound is insoluble (does NOT dissolve in water), then it remains as a compound

39. Writing Total Ionic Equations
Molecular Equation: K2CrO4 + Pb(NO3)2  PbCrO4 + 2 KNO3 Soluble Soluble Insoluble Soluble Total Ionic Equation: 2 K+ + CrO Pb NO3-  PbCrO4 (s) + 2 K+ + 2 NO3-

40. Net Ionic Equations
These are the same as total ionic equations, but you should cancel out ions that appear on BOTH sides of the equation
Total Ionic Equation:
2 K+ + CrO Pb NO3- 
PbCrO4 (s) + 2 K+ + 2 NO3-
(Spectator ions)
Net Ionic Equation:
CrO Pb+2  PbCrO4 (s)