1. The document describes different types of chemical reactions including synthesis, decomposition, single displacement, double displacement, combustion, acid-base, and neutralization reactions. 2. Metals react with oxygen to form metal oxides which are bases. Non-metals react with oxygen to form non-metal oxides which are acids. 3. Acid-base reactions involve acids and bases reacting to form salts and water in a neutralization reaction.

1. TYPES OF REACTIONS
Review!!

2. Synthesis
Example C + O2
2
OOC +  O OC
OOC
OOCC
C C C C C C C
C
C
C
General: A + B  AB
C

3. Decomposition
Example: NaCl
3
General: AB  A + B
Cl Na Cl + Na

4. Single displacement
Example: Zn + CuCl2
4
ZnClCl
Cu +
General: AB + C  AC + B
ClCl
Zn Cu+

5. Double displacement
Example: MgO + CaS
5
General: AB + CD  AD + CB
SO
Mg Ca
+
OS
Mg Ca
+

6. Combustion Reaction
• A reaction that releases carbon dioxide and
water
• A hydrocarbon and oxygen combine to form
CO2 and H2O.
CH4 + 2O2  CO2 + 2H2O
General: AB + CD  CO2 + H2O

7. ACID BASE REACTIONS
Metals, Non-metals & Neutralizations

8. METALS

9. Metal + O2  metal oxide + H2O  Base
• Metals react with oxygen to form metal
oxides
• Metal oxides always form solids
• Metal oxides also called basic oxides or basic
anhydrides
• Metal oxides react in water to form bases

10. Group 1 Metals (Alkali Metals)
• Potassium burns in O2 to make potassium oxide
4K(s) + O2(g) → 2K2O(s)

11. Group 1 Metals (Alkali Metals)
• Potassium burns in O2 to make potassium oxide
4K(s) + O2(g) → 2K2O(s)
• Potassium oxide dissolves in H2O
K2O(s) + H2O(l) → 2KOH(aq)

12. Group 1 Metals (Alkali Metals)
• Potassium burns in O2 to make potassium oxide
4K(s) + O2(g) → 2K2O(s)
• Potassium oxide dissolves in H2O
K2O(s) + H2O(l) → 2KOH(aq)
• Alternatively you can add potassium directly to water
2K(s) + 2H2O(l) → 2KOH(aq) + H2(g)
• KOH used to make soap, liquid fertilizer, paint remover,
cosmetics
Synthesis
Single
Displacement

13. Group 2 Metals (Alkali Earth Metals)
• Formation of Metal oxide
2Ca(s) + O2(g) → 2CaO(s)
• Formation of base
CaO(s) + H2O(l) → Ca(OH)2(aq)
• Lime (CaO) added to soil for growth of plants that prefer
basic soil.
• Ca(OH)2 used in bricks and as a food additive.

14. Other Metals - Zinc
• Formation of metal oxide:
Zn + O2  ZnO
• Formation of base:
ZnO + H2O  Zn(OH)2
• ZnO is often used as an additive to plastic, glass, cement,
paints, ointments, sealants, foods, batteries and fire
retardants.
• One major use of Zn(OH)2 is as an absorbent in surgical
dressings.

15. NON-METALS

16. Non-Metal + O2  N-M oxide + H2O  Acid
• React in O2 to form non-metal oxides
• Non-metal oxides are often fluids (gas/liquid)
• N-M oxides known as acidic oxides
• Non-metal oxides react in water to form
acids

17. Nitrogen
• Nitrogen reacts with O2 to make nitrogen dioxide
N2(g) + 2O2(g) → 2NO2(g)
• Nitrogen dioxide dissolves in H2O to form nitric acid
3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g)
• Nitrogen dioxide contributes to air pollution.
• Nitric acid can be used in explosives for munitions and
demolition. It can also be used for pigments in inks and
dyes.
Synthesis

18. Phosphorus
• Formation of Non-Metal oxide
4P(s) + 5O2(g) → 2P2O5(s)
• Formation of acid
P2O5(s) + 3H2O(l) → 2H3PO4(aq)
• Diphosphorus pentoxide is used as a very strong
dehydrating agent.
• Phosphoric acid used to make fertilizers, home cleaning
products and rust inhibitor.

19. Carbon
• Formation of non-metal oxide:
C + O2  CO2
• Formation of acid:
CO2(g) + H2O(l) → H2CO3(aq)
• Carbon dioxide is produced from the burning of fossil
fuels and contributes to global warming
• Carbonic acids are a major factor in ocean acidification.

20. NEUTRALIZATION
REACTIONS

21. Acids + Bases
• The H+ ions from the acid can combine with the OH- ions
from the base
H+
(aq) + OH-
(aq) --> HOH(l)
This process is called Neutralization
the resulting solution is neutral
(because water is set to pH 7)

22. • The reaction of an acid and a base produces a salt and
water
Acid + Base  Salt + Water

23. • The reaction of an acid and a base produces a salt and
water
Acid + Base  Salt + Water
2HCl(aq) + Mg(OH)2(s)  MgCl2(aq) + H2O(l)
Stomach acid Antacid No more heartburn!!

24. • A salt is a compound made up of
oppositely-charged ions
Neutralization = double displacement reactions

25. Ex. 1) Predict the products, balance the equation, state
chemical names, and classify each as either an acid, base,
salt or water.
__Ca(OH)2 + __H3PO4 

26. Ex. 1) Predict the products, balance the equation, state
chemical names, and classify each as either an acid, base,
salt or water.
_Ca(OH)2 + _H3PO4  _Ca3(PO4)2 + _H2O

27. Ex. 1) Predict the products, balance the equation, state
chemical names, and classify each as either an acid, base,
salt or water.
3Ca(OH)2 + 2H3PO4  Ca3(PO4)2 + 6H2O

28. Ex. 1) Predict the products, balance the equation, state
chemical names, and classify each as either an acid, base,
salt or water.
3Ca(OH)2 + 2H3PO4  Ca3(PO4)2 + 6H2O
Calcium hydroxide + phosphoric acid  calcium phosphate + water

29. Ex. 1) Predict the products, balance the equation, state
chemical names, and classify each as either an acid, base,
salt or water.
3Ca(OH)2 + 2H3PO4  Ca3(PO4)2 + 6H2O
Calcium hydroxide + phosphoric acid  calcium phosphate + water
Base + Acid  Salt + Water

30. Ex. 2) In there is an industrial accident, a whole barrel of
sulfuric acid (a dangerously strong acid) was spilled. Show
putting a strong base, such as calcium hydroxide, can
neutralize the acid.
Sulfuric acid + calcium hydroxide 

31. Ex. 2) In there is an industrial accident, a whole barrel of
sulfuric acid (a dangerously strong acid) was spilled. Show
putting a strong base, such as calcium hydroxide, can
neutralize the acid.
Sulfuric acid + calcium hydroxide  calcium sulfate + water

32. Ex. 2) In there is an industrial accident, a whole barrel of
sulfuric acid (a dangerously strong acid) was spilled. Show
putting a strong base, such as calcium hydroxide, can
neutralize the acid.
Sulfuric acid + calcium hydroxide  calcium sulfate + water
H2SO4(aq) + Ca(OH)2(aq)  CaSO4(s) + 2H2O(l)