Reactivity Series

Question 1

What is the reactivity series?

Answer 1

List of reactivity

POTASSIUM
SODIUM
LITHIUM
CALCIUM
MAGNESIUM
ALUMINIUM
CARBON
ZINC
IRON
HYDROGEN
COPPER
SILVER
GOLD

Question 2

What is displacement

Answer 2

When a more reactive element takes the place of a less reactive element in a compound

Question 3

Why does aluminium not react and how could you get it to react?

Answer 3

Forms an oxide layer which prevents it reacting - scratched off with sand paper

Question 4

What gas is formed when reactive metals are added to dilute acids and how can we test for it?

Answer 4

Hydrogen - lit splint produces a squeaky pop

Question 5

Why would there be no reaction between magnesium and magnesium sulfate?

Answer 5

Because elements can not displace themselves

Question 6

What is oxidation?

Answer 6

The gain of oxygen

Question 7

What is reduction?

Answer 7

The loss of oxygen

Question 8

What is a redox reaction?

Answer 8

A reaction in which oxidation and reduction both occur

Question 9

What is an ore?

Answer 9

A substance which contains metal compounds found in nature + the Earths crust

Question 10

Which element can be used to obtain pure metals from their oxides and why?

Answer 10

Carbon can be used (because it is cheaper and more abundant compared to other elements eg magnesium) if the metal is less reactive than it (below in the series) if it is more reactive electrolysis (an alternative method) is used.

Question 11

What is a native element?

Answer 11

An element which is found pure in its metallic form and uncombined (anything below copper) - doesn’t need to be extracted

Question 12

What is rust?

Answer 12

Iron III oxide
Fe2O3
A red Brown solid

Question 13

In what conditions can rusting occur?

Answer 13

When Iron is exposed to oxygen and water

Question 14

Why can steel rust?

Answer 14

It is an alloy of iron and carbon (stronger)

Question 15

What is rusting a form of?

Answer 15

Corrosion - all metals can corrode (oxidise to become brittle) but only iron rusts

Question 16

How can corrosion/rusting be prevented?

Answer 16

Physical barriers - preventing oxygen and water from reaching the metal
Paint, oil/grease, plating
Disadvantage - coating must be maintained or else water + oxygen will get into iron

Sacrificial Potential- attaching a more reactive metal (mg, zn) to the iron so they react with the oxygen instead and oxidise instead of the iron.
Railways - bags of mg, Ship hulls - zinc bolted on
Disadvantage - Protecting metal must be replaced, expensive

Galvanising - Coating of molten zinc, combo of both - physical barrier until chipped then it is reacted
Bridge girders, some car body panels