A1 - Ionic Bonding

Question 1

What is a giant ionic lattice?

Answer 1

A metal and a non-metal bonded together.

Question 2

What is the definition of ionic bonding?

Answer 2

The electrostatic attraction between positive and negative ions

Question 3

Briefly describe 3 chemical properties of ionic compounds:

Answer 3

• High melting and boiling points
• Soluble in polar solvents (generally insoluble in non-polar solvents)
• Can conduct electricity when dissolved/molten (can’t conduct when solid)

Question 4

Why is it that most ionic compounds have high melting and boiling points?

Answer 4

High temperatures are needed to provide the large quantity of energy needed to overcome the strong electrostatic attraction between the ions.

Question 5

What causes the melting point to be higher in some ionic lattices than others?

Answer 5

For lattices containing ions with greater ionic charges, the melting point is higher as there is a stronger attraction between ions.

Question 6

What solvents do many ionic compounds dissolve in?

Answer 6

Polar solvents, such as water.

Question 7

Why are many ionic compounds soluble in polar solvents like water?

Answer 7

Polar water molecules break down the lattice and surround each ion in solution.

Question 8

What might lead to an ionic compound not being very soluble overall?

Answer 8

If the compound is made up of ions with large charges, the ionic attraction may be too strong for the water to be able to break down the lattice structure

Question 9

Therefore what decides the solubility of an ionic compound?

Answer 9

The relative strengths of the attractions within the giant ionic lattice and the attractions between ions and water molecules.

Question 10

When do ionic compounds conduct electricity/when do they not?

Answer 10

They conduct electricity when liquid/dissolved but they don’t conduct when solid.