Package 2

Question 1

Lattice enthalpy

Answer 1

The heat that is absorbed when 1 mole of solid ionic compound is broken up to form gaseous ions under standard conditions

Question 2

Lattice enthalpy depends on what factors

Answer 2

1. The electrostatic forces between two oppositely charged ions
2. The distance between ions

Question 3

What happens to the lattice enthalpy when the ionic charge increases

Answer 3

The ionic attraction increases and increases the lattice energy

Question 4

Lattice energy vs boiling/melting point

Answer 4

Proportional

Question 5

Volatility in ionic compounds

Answer 5

Very low because the electrostatic forces of attraction are very strong

Question 6

Solubility of ionic compounds in water

Answer 6

Since water has a negative and positive end, it attracts the negative and positive ions of a compound and are hydrated

Question 7

Solubility of ionic compounds in non polar things

Answer 7

Insoluble because there is no attraction between the liquid and the ions

Question 8

CaCO3 in water

Answer 8

Only a small amount dissolves

Question 9

Conducting electricity

Answer 9

Only possible in molten or dissolved in water

Question 10

Why are ionic compounds brittle

Answer 10

When force is applied the same charge ions line up and therefore cause repulsion forces, splitting apart

Question 11

Chlorides of later elements (Al, Si, P and S)

Answer 11

Molecular covalent and have very low melting points and do not conduct electricity

Question 12

Electronegativity

Answer 12

Amount of attraction that an atom has for the shared pair in a covalent bond

Question 13

Xp for each bond

Answer 13

Ionic: Xp is greater than 1.8
Polar covalent: 0 < Xp < 1.8
Pure covalent: 0

Question 14

Sharing of electrons in each bond

Answer 14

Ionic: Complete transfer
Polar: Uneven sharing
Pure: Equal sharing