TYPES OF REACTIONSReview!!

Synthesis

Example C + O2

2

OOC + O OC

OOCOOCC

C C C C C C CCCC

General: A + B AB

C

Decomposition

Example: NaCl

3

General: AB A + B

Cl Na Cl + Na

Single displacement

Example: Zn + CuCl2

4

ZnClClCu +

General: AB + C AC + B

ClClZn Cu+

Double displacement

Example: MgO + CaS

5

General: AB + CD AD + CB

SO

Mg Ca

+OS

Mg Ca+

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

ACID BASE REACTIONSMetals, Non-metals & Neutralizations

METALS

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

Group 1 Metals (Alkali Metals)

• Potassium burns in O2 to make potassium oxide

4K(s) + O2(g) → 2K2O(s)

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)

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

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.

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.

NON-METALS

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

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

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.

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.

NEUTRALIZATION

REACTIONS

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)

• The reaction of an acid and a base produces a salt and water

Acid + Base Salt + Water

• 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!!

•A salt is a compound made up of

oppositely-charged ions

Neutralization = double displacement reactions

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

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

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

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

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

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

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

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)