Ionic Bonding & Structure

Question 1

Describe the structure and bonding of ionic compounds.

Answer 1

C - giant ionic lattice
B - many strong ionic bonds
D - strong electrostatic force of attraction between positive and negative ions

Question 2

Describe and explain the melting and boiling points of ionic compounds.

Answer 2

1. Solids at room temperature so have high melting and boiling points
   —> there is insufficient energy to over come the strong electrostatic force of attraction between oppositely charged ions, so require high temperatures
2. Melting points increases as ionic charge ratio increases
   —> there is stronger attraction between ions

Question 3

Describe and explain the solubility of ionic compounds.

Answer 3

1. Dissolve in polar solvents
   —> polar water molecules break down the lattice and surround each ion in solution
2. The larger the ionic charge, the lower the solubility
   —> ionic attraction may be to strong for water to be be able to break down the ionic lattice

Question 4

Describe and explain the electrical conductivity of ionic compounds in solid vs. in liquid or molten states.

Answer 4

Solid state:
Does not conduct electricity
—> ions are in a fixed position so cannot move and carry a charge

Liquid or molten states:
Do conduct electricity
—> ionic lattice breaks down so ions are free to move and carry a charge