1. Predicting Chemical Reactions

2. Activity Series
Activity Series is an order of elements organized according to the ability for the elements to undergo a chemical reaction.
(Hierarchical list)
Metals on the list: likely to lose an electron
Nonmetals on the list: likely to gain an electron
Just because a chemical reaction is written does not mean that it will take actually happen.

3. Activity Series

4. Synthesis
Remember:
Synthesis Reactions describe a chemical reaction in which two or more substances for a new compound.
Most commonly found with an element reacting with oxygen (O2) or sulfur (S8).

5. Synthesis: Oxygen & Sulfur
Consider the charges to determine name of compound.
When a metal reacts with oxygen it produces an oxide.
Fe + O2  FeO : Iron (II) Oxide
Fe + 02  Fe2O3 : Iron (III) Oxide
When a metal reacts with sulfur it produces a sulfide.
Ba + S8  BaS

6. Synthesis: Metals with Halogens
Depends on the charge of the metal.
Na + Cl2  NaCl
Mg + F2  MgF2
CO + F2  CoF3

7. Synthesis: Oxides Metals: CaO + H2O  Ca(OH)2 Nonmetals:
React with water to produce a metal hydroxide.
CaO + H2O  Ca(OH)2
Nonmetals:
React with water to produce oxyacids.
SO2 + H2O  H2SO3

8. Decomposition Remember:
Decomposition Reactions describes a chemical reaction in which one compound becomes two simpler substances.
Most commonly found as an endothermic reaction.

9. Decomposition: Binary Compounds
Binary Compound has two different types of elements bonded together.
Oxides of the less-active metals (located lower center on the periodic table), decompose into their elements when heated.
Hg0  Hg + O2

10. Decomposition: Metal Carbonates
Metal carbonate breaks down into a metal oxide and carbon dioxide.
CaCO3  CaO + CO2

11. Decomposition: Metal Hydroxides
Metal hydroxides decompose into metal oxide and water.
Except if the metal is found in Group 1.
Ca(OH)2  CaO + H2O

12. Decomposition: Metal Chlorates
After being heated, metal chlorates decompose into metal chloride and oxygen.
KClO3  2KCl + O2

13. Decomposition: Acids Decompose into metal oxides and water.
H2CO3  CO2 + H2O
H2SO4  SO3 + H2O

14. Single-Displacement Remember:
Single displacement describes a reaction which one element replaces a similar element in a compound.
Most single replacement reactions take place within an aqueous solution.

15. Single-Displacement: Metal displaced by a Metal
Reaction will take place if activity of single metal is higher than that within the compound.
Al + Pb(NO3)2  Pb + Al(NO3)3

16. Single-Displacement: H in H20 displaced by a Metal
Higher active metals react with water in liquid state to form hydroxides and hydrogen gas.
Na + H20 (l)  NaOH + H2
Lower active metals require energy input for water to be steam in order to produce a metal oxide and hydrogen gas.
Fe + H20 (g)  Fe2O3 + H2

17. Single-Displacement: H in acid displaced by a Metal
Higher active metals react with certain acidic solutions.
The reaction produces an ionic compound and hydrogen gas.
Mg + HCl  MgCl2 + H2

18. Single-Displacement: Halogens displaced by Halogens
Higher active halogens (non-metals in group17) may displace a lower active halogen.
F2 + 2NaCl  Cl2 + NaF
Remember, each halogen element has lower activity than the one above it.
Usually is displaced in an ionic compound, producing a new ionic compound.

19. Double-Displacement Remember:
Single displacement describes a reaction which two ions exchange places to form new compounds.
The reaction produces a precipitate, an insoluble gas (bubbles out), or a molecular compound (typically water).

20. Solubility Chart

21. Predicting the Products of a Double Replacement Reaction
Given the reactants, write the name of the products by switching the LAST names
Do not use acid names; use FULL NAME
ex: Don’t use Nitrous Acid; use Hydrogen Nitrite
Check the Table of Solubility Rules
If something is insoluble  it will form a precipitate (s) during the rxn
RXN WILL OCCUR
If a liquid/ gas has formed
If something is soluble  it will form an aqueous (aq) product
(If you finish with 2 soluble (aq) reactants)
NO RXN (stop there)

22. The Exceptions!
5 things that may seem soluble, but will actually produce a liquid or a gas  a reaction WILL occur
If any of these are a product, there will be a rxn
Hydrogen Carbonate  breaks into water and Carbon Dioxide
H2CO3 (aq)  H2O (l) + SO2 (g)
if you make Hydrogen Carbonate, the CO2 bubbles (gas) produced = rxn
Hydrogen Sulfite  breaks into water and Sulfur Dioxide
H2SO3 (aq)  H2O (l) + SO2 (g)
Ammonium Nitrate  breaks into water and Ammonia
NH4OH (aq)  H2O (l) + NH3 (g)

23. Exceptions (cont.) Hydrogen Sulfide - H2S Hydrogen Hydroxide – HOH
Odor produced (rotten eggs)
Hydrogen Hydroxide – HOH
Water H2O (l) (which is a rxn)