5.2- Ionic Bonding And Structure

Question 1

Define ionic bonding

Answer 1

The electrostatic attraction between positive and negative ions

Question 2

What is the structure of an ionic compound?

Answer 2

Each ion attracts oppositely charged ions in all directions that result is a giant ionic lattice structure

Question 3

What happens when there is a greater charge?

Answer 3

Greater the charge = stronger the electrostatic force of attraction = greater energy needed to separate them =high m.p and b.p

Question 4

Why do ionic compounds have high melting and boiling points?

Answer 4

• There are strong electrostatic forces of attraction between the oppositely charged ions in all directions which require lots of energy to overcome
• smallerions pack close together = increase the m. p and b.p

Question 5

Why are ionic compounds generally soluble in water?

Answer 5

-Water is a polarmolecule and so the small delta positive and delta negative charges surround and add up to the opposite charge on the ion
- due to the attraction it disrupts the electrostatic forces of attraction between them and breaks them apart

Question 6

What are the 2 processes that solubility requires?

Answer 6

1. The ionic lattice must be broken down
2. Water molecules must attract and surround the ions

Question 7

Why do they not conduct electricity when solid?

Answer 7

-The ions are held together in a fixed position by strong, electrostatic forces acting in all directions
- unable to move and carry the charge

Question 8

Why can they conduct electricity when molten or aqueous?

Answer 8

Ions are free to move and carry the charge through the structure

Question 9

Why are the compounds brittle?

Answer 9

• when moved ions no longer have their alternating lattice arrangement
• instead ions with the same charge end up next to each other
• due to the repulsion between like charges the structure breaks apart

Question 10

In what type of solvents do ionic lattices dissolvein?

Answer 10

Polar solvents Eg. Water