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Published by meksue933, 2020-04-05 01:10:25

CHAPTER 4 REACTIVITY OF METALS

CHAPTER 4 REACTIVITY OF METALS

Keywords: METALS

SCIENCE FORM 3

REACTIVITY OF
METALS

TC SUHAIZA MAT SAID

4.1 VARIETY OF MINERALS

• Mineralogy or the study of minerals is an active field

of science because the number and properties of
minerals keep increasing.
• Example :

Petrol or Diesel Car Electric Car

Using 2 minerals which can produce long lasting
batteries (Lithium and Cobalt).

Various Form of Minerals in Earth’s Crust

• Minerals are solid elements or compounds The common and systematic names of natural
present naturally with definite crystalline compounds and the combination of their
structures and chemical compositions. elements.

• Various minerals are contained in rocks Common Systematic Combination
found in Earth’s Crust. Name Name of elements

Hematite Iron (III) Oxide Iron, oxygen

Minerals are made up: Cassiterite Tin (IV) Oxide Tin, oxygen

1. Gold Quartz Silicon Dioxide Silicon, oxygen

2. Silver Bauxite Aluminium Aluminium,
Oxygen
(aluminium ore) Oxide

3. Compounds Bauxite Galena Lead (II) Lead, Sulphur
(lead ore) Sulphide
Hematite

Galena Pyrite Iron (II) Sulphide Iron, Sulphur

Cassiterite Calcite Calcium Calcium,
Carbonate Carbon, oxygen

Natural Compounds are the Combination of Several Elements

MINERALS USES IN DAILY LIFE

Limestone • Construction of roads and buildings
Graphite • Table tops
Lignite
Phosphorus • Writing tool
Copper • Pencil

Lithium • Help generate electricity
• Plant fertilizer product

• Baking soda
• Glass
• Kitchenware

• Weapons
• Hunting tools

• Li-Ion batteries
• Electric vehicles
• Power telecommunication devices

4.2 Reactivity Series of Metals

Reaction between metals and oxygen

Vigorous Reaction Less Vigorous

between a more reactive metal Reaction between a less
such as magnesium and
oxygen, a bright flame is reactive metal such as iron and
observed. oxygen, only a glow or slow
change in colour is observed.

Constructing Reactivity Series of Metals

Different metals have different reactivities towards oxygen.
Metals that are more reactive towards oxygen react more
vigorously with oxygen.

Au Ag Hg Cu Pb Sn Fe Zn Al Mg Ca Na K

Reactivity of metals towards oxygen increases

Investigate the reactivity of several metals towards oxygen

Equations for the reactions between
metals and oxygen

Magnesium + oxygen Magnesium oxide

Aluminium + oxygen Aluminium oxide
Zinc + oxygen Zinc oxide
Iron + oxygen Iron oxide

OBSERVATION

METAL Metal burns very Metal burns Metal burns Metal glows Metal glows dimly
quickly & brightly quickly & brightly slowly brightly
Magnesium √
Aluminium √ √

Zinc √
Iron √
Lead

Position of Carbon in the Reactivity Series of Metals

Equations for the reactions between metals
and carbon

Zinc oxide + carbon Zinc + carbon dioxide

Aluminium oxide + carbon Aluminium + carbon
Lead (II) oxide + carbon dioxide

Lead + carbon dioxide

Mixture Observation Reactivity of
carbon
Zinc oxide & Mixture glows
carbon No change Carbon is more
reactive than zinc
Aluminium Mixture glows
oxide & carbon Carbon is less
reactive than
Lead (II) oxide aluminium
& carbon
Carbon is more
reactive than lead

Position of Hydrogen in the Reactivity Series of Metals

Mixture Observation Inference

Hydrogen and Aluminium Oxide Aluminium oxide does not glow. Hydrogen does not reduce aluminium oxide.
Hydrogen and Zinc Oxide Aluminium oxide is white in colour.
Hydrogen and Iron (III) Oxide Hydrogen does not reduce zinc oxide.
Hydrogen and Lead (II)Oxide Zinc oxide does not glow.
Hydrogen and Copper (II) Oxide Zinc oxide turns yellow when hot and white on cooling. Iron is produced.
Hydrogen reduce iron (III) oxide to iron.
Iron (III) oxide burns brightly. Lead is produced.
Reddish brown powder turns shiny grey. Hydrogen reduce Lead (II) Oxide to Lead.
Copper is produced.
Lead (II) oxide burns brightly. Y Hydrogen reduce Cooper (II) oxide to Cooper.
Yellow powder turns shiny grey.

Copper (II) oxide burns very brightly.
Black powder turns brown.

Conclusion on the Position of Carbon and Hydrogen in the
Reactivity Series of Metal

Reactivity Series K Potassium
of Metals Na Sodium
Ca Calcium
Reactivity of Mg Magnesium
metal towards Al Aluminium
oxygen increases C Carbon
Zn Zinc
H Hydrogen
Fe Iron
Sn Tin
Pb Lead
Cu Copper
Hg Mercury
Ag Silver
Au Gold

4.3 Extraction Metals from their Ores

Extraction of metals is the process to obtain metals from their ore

K Potassium Extraction through Metals higher than
Na Sodium electrolysis of metallic carbon in the reactivity
Ca Calcium compounds in molten form series of metals, the
Mg Magnesium extraction of the metal
Al Aluminium Extraction through reduction from its metallic
C Carbon of metal oxides by carbon compound is through
Zn Zinc electrolysis.
H Hydrogen
Fe Iron Metals lower than
Sn Tin carbon in the reactivity
Pb Lead series of metals, the
Cu Copper extraction of the metal
Hg Mercury from its ore is through
Ag Silver the reduction of its
Au Gold oxide with carbon.

Extraction of the metals is done through
direct heating of the metallic compounds.

Exist in the form of elements in Earth’s crust.

Process Of Iron Extraction

A mixture of concentrated iron ore or iron oxide, coke and limestone is added

1 into a blast furnace through the top.

Reactions that occur in the furnace at high temperature.

Production of Iron
• Coke or carbon reacts with oxygen in the hot air to produce

carbon dioxide and heat.

• Carbon dioxide that is produced reacts with the rest of the hot
coke to form carbon monoxide which is a strong reducing
agent.

3 • Carbon monoxide and carbon reduced iron oxide into iron.

Production of Slag
• Limestone or calcium carbonate decomposes to form calcium

oxide and carbon dioxide.

• Calcium oxide reacts with impurities such as sand or silicon
dioxide in iron ore to form slag or calcium silicate.

2 A very hot blast of air is pumped into the At high temperature in the furnace.
furnace throught the bottom. • Iron that is produced will met. The molten irons flows to the bottom part

of the furnace. The molten iron is tapped off and channelled into moulds

4 and allowed to cool and freeze. Its known as cast iron.
• Slag that is produced will melt. This molten slag flows to the bottom.
Molten slag is less denser than molten iron. The molten slag is tapped off
and used to make the base of buildings and roads.

Process Of Iron Extraction

Reactions that occur in the furnace at high temperature.

Production of Iron

 Coke or carbon reacts with oxygen in the hot air to produce carbon dioxide and heat.

Carbon + Oxygen Carbon Dioxide

 Carbon dioxide that is produced reacts with the rest of the hot coke to form carbon monoxide
which is a strong reducing agent.

Carbon Dioxide + Carbon Carbon Monoxide

 Carbon monoxide and carbon reduced iron oxide into iron.

Iron (III) oxide + Carbon Iron + Carbon Dioxide
Iron (III) oxide + Carbon Monoxide Iron + Carbon Dioxide
Iron (II) oxide + Carbon Iron + Carbon Dioxide
Iron (II) oxide + Carbon Monoxide Iron + Carbon Dioxide

Production of Slag

 Limestone or calcium carbonate decomposes to form calcium oxide and carbon dioxide.

Calcium Carbonate Calcium oxide + Carbon Dioxide

 Calcium oxide reacts with impurities such as sand or silicon dioxide in iron ore to form slag or
calcium silicate.

Calcium Oxide + Silicon dioxide Calcium Silicate

Mining Issues In Malaysia

Air pollution Usage of large Air pollution by
due to burning amount of gases released

of fuels electrical energy from blast
furnaces
Water pollution Mining
due to cleaning Issues in Destruction of
Malaysia habitat due to
of ore construction of

mines

Soil erosion due Sound pollution
to mining of ore from mining
machinery

THANK YOU

REFERENCE : KPM (2019). SCIENCE FORM 3 TEXTBOOK


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