General Types of Chemical Reactions with Exercises

1. Chemical
Reactions

2. Chemical
Equation
-describes exactly
what happens in a
chemical reaction

3. Reactants
- the reacting
substances
-the substances
that enter into
the reaction

4. Products
- substances
produced by
the reaction

5. Symbols Used:
1. +
2.
3.
4.

6. 5. (s)
6. (l)
7. (g)
8. (aq)

7. 9. Pt
10. elec.

8. 7 Diatomic
Elements
1. Hydrogen (H2)
2. Oxygen (O2)
3. Nitrogen (N2)
4. Fluorine (F2)
5. Chlorine (Cl2)
6. Bromine (Br2)
7. Iodine (I2)

9. Word
Equation
gives the names of
the chemical
substances
involved in the
reaction

10. Formula
Equation
uses symbols and
formulas to represent
names of elements
and compounds

11. Factors in
Equation Writing
1.The equation
must
represent the
facts.

12. 2. The equation
must include the
symbols and
formulas that are
used as
reactants and
products.

13. 3. The Law of
Conservation
of Mass must
be satisfied

14. Law of Conservation
of Mass
“In any ordinary chemical
reaction, the total mass of
the reactants is equal to
the total mass of the
products”

15. Law of Conservation
of Atoms
“There must be the same
number of atoms of each
element represented
on each side of the
equation”

16. Coefficient
- a whole number
written before a symbol
or formula in order to
balance a chemical
equation

17. Example:
1. Hydrogen gas burns in
oxygen gas to yield
water vapor

18. Example:
2. Hydrogen reacts with
nitrogen to form
ammonia

19. Example:
3. Magnesium + oxygen
magnesium oxide

20. 4. potassium chlorate (s)
potassium chloride (s)
+ oxygen (g)
5. Chlorine + potassium
bromide potassium
chloride + bromine

21. 6. ammonia + hydrogen
sulfide ammonium
sulfide
7. Calcium chlorate
calcium chloride + oxygen

22. 8. zinc + copper (II) sulfate
zinc sulfate + copper
9. Magnesium oxide
magnesium + oxygen
10. Aluminum + sulfuric
acid aluminum
sulfate + hydrogen

23. MAJOR TYPES OF
CHEMICAL REACTIONS

24. Major Types of Chemical Reactions

25. 1) Synthesis
two or more simple
substances combine to form a
more complicated substance.
general form:
A + X → AX

26. 2) Decomposition - the opposite
of a synthesis reaction; a complex
substance breaks down to make
simpler ones.
General form:
AX ---> A + X

27. 3) Single displacement: This is
when one element trades place
with another element in a
compound. These reactions come
in the general form of:
A + BX → AX + B
AY + X → AX + Y

28. Activity Series of Elements:
Li Al Pb
K Zn (H)
Ba Fe Cu
Ca Cd Hg
Na Ni Ag
Mg Sn Au

29. 4) Double displacement: This is
when the anions and cations of
two different molecules switch
places, forming two entirely
different compounds.
General form:
AX + BY → AY + BX

30. Example:
Reaction of lead (II) nitrate with
potassium iodide to form lead (II)
iodide and potassium nitrate.

31. 5. Acid-base Reaction
(Neutralization)
This is a special kind of double
displacement reaction that takes
place when an acid and base react
with each other. Generally, the
product of this reaction is some ionic
salt and water
HX + A(OH) ---> H2O + AX

32. 6. Combustion - oxygen
combines with another
compound to form water
and carbon dioxide.
These reactions are
exothermic.
Example:
burning of butane

33. Balance the following equations and
identify the type of reaction:
1) NaOH + Ca(NO3)2--> NaNO3 + Ca(OH)2
2) C2H4 + O2 --> CO2 + H2O
3) Fe + NaBr --> FeBr3 + Na
4) CaSO4 + KOH --> Ca(OH)2 + K2SO4
5) NH4OH + HBr --> H2O + NH4Br
6) Pb + O2 --> PbO2
7) CaCO3 --> CaO + CO2