Topic 2- Bonding And Structure

Question 1

Define ionic bonds

Answer 1

The electrostatic force of attraction between oppositely charged ions

Question 2

What happens to ionic radius with increasing negative charge?

Answer 2

Increases

Question 3

What are isoelectric ions?

Answer 3

Ions that have the same electronic configurations. Same number of electrons, different number of protons.

Question 4

Why are ionic compounds solids at room temperature?

Answer 4

Because there isn’t enough energy to overcome the strong electrostatic forces of attraction between oppositely charged ions that make up the lattice.

Question 5

What happens as the ion gets smaller?

Answer 5

The charge increases, higher ESFOA, higher MP

Question 6

What is the solubility of ionic compounds dependent on?

Answer 6

1. The breaking down of the ionic lattice
2. The polar molecules attracting surrounding ions

Question 7

What happens to solubility as the ionic charge gets greater? (General rule)

Answer 7

The less soluble an ionic compounds is

Question 8

What is a covalent bond?

Answer 8

The electrostatic force of attraction between the shared pair of electrons and the positive nuclei of bonds

Question 9

What is a dative covalent bond?

Answer 9

Electrons that can be donated to form a bond with an electron deficient atom.

Question 10

What happens as a covalent bond length increases?

Answer 10

Greater atomic radius, weaker bond.

Question 11

Describe triple bonds

Answer 11

Shortest, strongest.
Due to large electron density between the nuclei of the two atoms. This increases forces of attraction and so pulls together, making shorter bond length