Reactivity Series of Metals

Question 1

Metal + H2O

Answer 1

Metal Hydroxide + H2

Question 2

. Metal + H2O (g=water vapour)

Answer 2

Metal Oxide + H2

Question 3

Metal + Acid

Answer 3

Salt+H2

Question 4

Poisoned
Sausages
Can
Make
A
Zulu
Ill
Therefore
Let
Highly
Clever
Men
Slaughter
Good
Pigs

Answer 4

Potassium (MR)
Sodium
Calcium
Magnesium
Aluminium
Zinc
Iron
Tin
Lead
Hydrogen
Copper
Mercury
Silver
Gold
Platinum (LR)

Question 5

Method of extraction for PSCMA

Answer 5

Electrolysis of molten compound

Question 6

Method of extraction for ZITLHCMS

Answer 6

Heating with Carbon

Question 7

Method of extraction for SGP

Answer 7

Found naturally uncombined

Question 8

PSC reactions

Answer 8

React with cold water and steam. Reaction becomes less vigorous down the group.

React with acid to form salt and hydrogen.

Question 9

Magnesium reaction

Answer 9

Magnesium reacts very slowly with cold
water, but explodes in steam.

React with acid to form salt and hydrogen.

Question 10

Aluminium reaction

Answer 10

React with acid to form salt and hydrogen.

Question 11

ZILTL reactions

Answer 11

No reaction with cold water;
heated metal reacts with steam.

React with acid to form salt and hydrogen.

Question 12

CMSGP reactions

Answer 12

No reaction

Question 13

Why aluminium cannot react with water?

Answer 13

Protected by layer of oxide to prevent reaction with water.

Question 14

Format for answering displacement reactions

Answer 14

MORE reactive metal displaces LESS REACTIVE metal from its COMPOUND.

Question 15

Extraction of Iron in the Blast Furnace

Answer 15

Substances added from top of furnace:
1. Iron ore (haematite), Fe2O3
2. Coke (carbon), C
3. Limestone, CaCO3 [to remove acidic impurities]
* Hot air pumped in near bottom of furnace.
* Molten slag and iron are removed at the bottom, iron sinks
to the bottom and slag floats on top of it.

Question 16

Reactions in the Blast Furnace

Answer 16

1) Coke burns in air to form carbon dioxide. C + O2 → CO2

2) Carbon dioxide reacts with more coke to produce carbon monoxide. CO2 + C → 2CO

3) Carbon monoxide (reducing agent) reacts with iron (III) oxide to form iron and carbon dioxide.
3CO + Fe2O3 → 2Fe + 3CO2

4) Limestone is decomposed to form calcium oxide and carbon dioxide. CaCO3 → CaO + CO2

5) Calcium oxide reacts with acidic impurities like silicon dioxide (sand) to produce slag (calcium
silicate).

CaO + SiO2 → CaSiO3(slag)

Question 17

Pure metals texture

Answer 17

soft

Question 18

Alloys texture

Answer 18

stronger and harder

Question 19

Pure metals

Answer 19

Atoms of the same size

Question 20

Atoms of pure metals movement

Answer 20

When a force is
applied, atoms can
slide over each
other easily

Question 21

Alloys movement

Answer 21

The atoms from the other metals are of
different sizes. They disrupt the orderly
arrangement of the metals and prevent the atoms from sliding over each other making alloys stronger and harder.

Question 22

Alloys

Answer 22

Mixture of metal and other metals/non-metals

Question 23

Reasons for Recycling Metals

Answer 23

1) Recycling costs less than extracting new metals from their ores.

2) There are only limited amounts of metals in the ‘Earth’s surface, recycling will conserve resources.

3) Recycling avoids the land pollution caused by disposal of metals in landfill sites or caused by mining.

Question 24

Explain why alloys are harder than metals.

Answer 24

The addition of another element
disrupts the orderly arrangement of metal due to difference in size.

Hence, the particles are not able to
slide over one another easily.

Question 25

State the condition for rusting.

Answer 25

Oxygen and water need to be present for rusting to occur.

Question 26

Explain why more
energy is required for the extraction of sodium from its chloride than any other metals.

Answer 26

Sodium is high in the reactivity series and forms strong bonds
in its compounds.

Hence it can only be extracted by electrolysis which requires more energy.

Question 27

How is silver extracted?

Answer 27

Silver is found naturally uncombined in the ground.

Question 28

Suggest why silver, but not magnesium is found in the Earth’s crust as
the unreacted element

Answer 28

Silver is low in the reactivity series
and while magnesium is high in the reactivity series.

Hence, magnesium tends to react with other elements like
oxygen to form compounds, but
silver is unreactive and does not react easily.

Question 29

Name waste gases that are possibly produced in the extraction of iron.

Answer 29

Carbon monoxide, carbon dioxide,
nitrogen (due to hot air being introduced)