Metals And Their Reactivity

Question 1

Acid + metal

Answer 1

Acid + metal = salt + hydrogen

Question 2

The reactivity series

Answer 2

Potassium
Sodium
Lithium
Calcium
Magnesium
Carbon
Zinc
Iron
Hydrogen
Copper

Question 3

What ions do metals always form

Answer 3

When metals react they lose electrons, forming POSITIVE ions

Question 4

Metal + water

Answer 4

Metal + water = metal hydroxide + hydrogen

Question 5

In what form are most metals in the Earth

Answer 5

Most metals tend to be fairly reactive, so they’re usually found as compounds and have to be extracted.

Question 6

Oxidation and reduction of common metals

Formation of metal ore:
Oxidation = gain of oxygen
Eg. Magnesium can be oxidised to form magnesium oxide

Extraction of metal:
Reduction = loss of oxygen
Eg. Copper oxide can be reduced to copper

Answer 6

Many common metals react with oxygen to form their oxides, which are found in the ground. This process is an example of oxidation.

A reaction that separates a metal from its oxide is called a reduction reaction.

Question 7

OILRIG

Answer 7

Oxidation
Is
Loss of electrons
Reduction
Is
Gain of electrons

Question 8

Redox reactions

Answer 8

In redox reactions, reduction and oxidation happen at the same time

Redox reactions include:

• metals reacting with acids
• halogen displacement reactions
• metal displacement reactions

Question 9

Ionic equations

Answer 9

Redox reactions are often shown using ionic equations.

In an ionic equation only the particles that react and the products they form are shown.

Eg. Mg + ZnCl2 = MgCl2 + Zn
This broken down: 
Mg + Zn2+ +2Cl- = Mg2+ + 2Cl- + Zn
You ignore the chloride ions because they don’t change, so the correct ionic equation is:
Mg + ZnCl2 = MgCl2 + Zn