1. Basic Chemistry
Part Two
Types of Chemical
Reactions
Pisgah High School
M. Jones Rev. 5/15/01
5/2/02
3/15/04
3/16/04

2. Types of Reactions
1. Synthesis (combination)
2. Decomposition
3. Single Replacement
4. Double Replacement
5. Acid-Base Neutralization
6. Combustion of

3. Synthesis Reactions
General format: A + B → C
A = compound or element
B = compound or element
C = compound
Always a single product
2 H2(g) + O2(g) → 2 H2O(l)

4. Decomposition Reactions
General Format: A → B + C
A = compound
B = compound or element
C = compound or element
Always a single reactant
2 H2O(l) → 2 H2(g) + O2(g)

5. Most single replacement
and double replacement
reactions involve the
interaction of ions.

6. Ions either have a positive
charge or a negative charge.
Cation = Positively
charged ion
Anion = Negatively
charged ion

7. Anion
A Negative Ion
ANIon

8. Single Replacement Reactions
General Format:
M + LA → MA + L
M and L = metals, A = anion
X + CY → CX + Y
X and Y = nonmetals, C = cation
element + compd → element + compd
Zn(s) + Cu(NO3)2 → Zn(NO3)2 + Cu(s)

9. Double Replacement Reactions
General Format:
AB + CD → AD + CB
compd + compd → compd + compd
A reaction occurs when
a precipitate is formed.
ZnCl2(aq) + 2 AgNO3(aq) →
2 AgCl(s) + Zn(NO3)2(aq)

10. Acid-Base Neutralization Reactions
General Format:
HA + BOH → BA + HOH
Acid-base neutralization
reactions are actually double
replacement reactions.

11. Acid-Base Neutralization Reactions
General Format:
HA + BOH → BA + HOH
acid + base → salt + water
Water is the insoluble “precipitate”
HCl(aq) + NaOH (aq) →
NaCl(aq) + HOH (l)

12. Combustion Of Hydrocarbons
General Format:
CxHy + O2 → CO2 + H2O
hydrocarbon + oxygen →
carbon dioxide + water
C3H8(g)+ 5 O2(g)→
3 CO2(g) + 4 H2O(g)

13. Identify the reaction type:
. Na2CO3  Na2O + CO2
. MgCl2 + F2  MgF2 + Cl2
. 2SO2 + O2  2SO3
. 2HI + Ba(OH)2  BaI2 + 2HOH
. C5H12 + 8O2  5CO2 + 6H2O
. ZnCl2 + Pb(NO3)2 

14. Identify the reaction type:
1. Na2CO3  Na2O + CO2
Decomposition

15. Identify the reaction type:
2. MgCl2 + F2  MgF2 + Cl2
Single replacement

16. Identify the reaction type:
3. 2SO2 + O2  2SO3
Synthesis

17. Identify the reaction type:
4. 2HI + Ba(OH)2  BaI2 + 2HOH
Acid/base neutralization

18. Identify the reaction type:
5. C5H12 + 8O2  5CO2 + 6H2O
Complete combustion
of a hydrocarbon

19. Identify the reaction type:
ZnCl2 + Pb(NO3)2 
PbCl2 (s) + Zn(NO3)2
Double replacement

20. Predicting the
Products of
Chemical Reactions.

21. Synthesis Reactions
1. Metal + O2  metal oxide
2. Nonmetal + O2  nonmetal oxide
3. Metal + nonmetal  salt
4. Water + metal oxide  metal OH- (base)
5. Water + nonmetal oxide  oxyacid
Metal oxide = basic anhydride
Nonmetal oxide = acid anhydride
Anhydride (anhydrous) = “without water”

22. Decomposition Reactions
1. Metal carbonates  metal oxide + CO2
2. Metal bicarbonate  metal oxide +
CO2 + H2O
3. Metal oxide  metal + O2
4. Metal hydroxide  metal oxide + H2O
5. Oxygen-containing salts  salt + O2
6. Hydrates  salt + H2O

23. Predicting the products of
single replacement reactions …
A single replacement reaction
occurs when …
… one element changes from
the elemental state to an
ionic state and replaces a
second ion in a compound.

24. Consider this single
replacement reaction:
Fe(s) + CuCl2(aq) 
Use the replacement series,
and look at iron and copper.
Since Fe is above Cu in the
replacement series, the Fe will
replace Cu.

25. Consider this single
replacement reaction:
Fe(s) + CuCl2(aq) 
FeCl3(aq) + Cu(s)
The Fe replaces the copper
and goes into solution as Fe +3
ions (the Fe dissolves)…
… the copper ions comes out of
solution as solid, metallic copper.

26. Consider this single
replacement reaction:
2 Fe(s) + 3 CuCl2(aq) 
2 FeCl3(aq) +3 Cu(s)
The final balanced
equation is …

27. Predicting the products of
double replacement reactions …
A double replacement reaction
occurs when there is …
… an insoluble product,
(a precipitate).
Use the solubility rules to
determine if one or more products
are insoluble in water.

28. Double Replacement Reactions
Consider the reaction between
solutions of barium nitrate and
sodium sulfate:
Ba(NO3)2(aq) + Na2SO4(aq) 
BaSO4
What is the formula for the product
that contains barium?

29. Double Replacement Reactions
Consider the reaction between
solutions of barium nitrate and
sodium sulfate:
Ba(NO3)2(aq) + Na2SO4(aq) 
BaSO4 + 2 NaNO3
What is the formula for the other
product?

30. Double Replacement Reactions
Consider the reaction between
solutions of barium nitrate and
sodium sulfate:
Ba(NO3)2(aq) + Na2SO4(aq) 
BaSO4 + 2 NaNO3
Which of the two is insoluble in water?
The BaSO4 gets an (s) or “down arrow”

31. Double Replacement Reactions
Consider the reaction between
solutions of barium nitrate and
sodium sulfate:
Ba(NO3)2(aq) + Na2SO4(aq) 
BaSO4 + 2 NaNO3 (aq)
Since NaNO3 is soluble in water,
put an (aq).

32. Predicting the Products of
Neutralization Reactions
Neutralization reactions are in the
same format as double
replacement reactions.
Acid + base  salt + water
The formation of water is what
drives an acid-base reaction.

33. Neutralization Reaction
Consider the reaction between
nitric acid and calcium hydroxide:
HNO3(aq) + Ca(OH)2(aq) 
Write the formulas for the
reactants.

34. Neutralization Reaction
Consider the reaction between
nitric acid and calcium hydroxide:
acid base
HNO3(aq) + Ca(OH)2(aq) 
Which is the acid, and
which is the base?

35. Neutralization Reaction
Consider the reaction between
nitric acid and calcium hydroxide:
acid base
HNO3(aq) + Ca(OH)2(aq) 
Ca(NO3)2(aq)
salt
What is the formula of the
salt that is produced?

36. Neutralization Reaction
Consider the reaction between
nitric acid and calcium hydroxide:
acid base
HNO3(aq) + Ca(OH)2(aq) 
Ca(NO3)2(aq) + HOH(l)
salt water
Finally, add the formula for water.
It is the “insoluble product.”

37. Many of these reactions are
REDOX reactions.
REDOX reactions involve…
Oxidation
and
Reduction

38. Oxidation-Reduction Reactions
Oxidation – the loss
of electrons
Reduction – the gain
of electrons

39. Oxidation-Reduction Reactions
… involve an exchange of
electrons which causes …
… a change in the oxidation
number of two or more
elements.

40. Oxidation-Reduction Reactions
 Most synthesis,
decomposition and
combustion reactions are
redox reactions.
 All single replacement
reactions are redox.

41. Reactions which can be redox:
1. Synthesis (combination)
2. Decomposition
3. Single Replacement
4. Double Replacement
5. Acid-Base Neutralization
6. Combustion

42. Redox Reaction: single replacement
0 +2 -1
2 Fe(s) + 3 CuCl2(aq) 
+3 -1 0
2 FeCl3(aq) +3 Cu(s)

43. You will study redox
reactions in more detail
later in the semester.