Lattice Enthalpy

Question 1

Define lattice enthalpy

Answer 1

Formation of one mole of ionic lattice from gaseous ions under standard conditions

Question 2

What does a more exothermic lattice enthalpy mean

Answer 2

Stronger ionic bonds

Question 3

Why is it not possible to measure lattice enthalpy directly

Answer 3

Its not possible to form 1 mole of ionic solid from its gaseous ions

Question 4

Define enthalpy change of solution

Answer 4

Enthalpy change that takes place when 1 mole of a solute is completely dissolved in water under standard conditions

Question 5

Define enthalpy change of hydration

Answer 5

The enthalpy change that takes place when dissolving one mole of gaseous ions in water.

Question 6

What are factors that impact the size of lattice enthalpy

Answer 6

Size of ions involved
Charges of ions
Ionic bond strength

Question 7

Which ions have more negative lattice enthalpy values , smaller or larger ions? Why?

Answer 7

Smaller ions as they can get closer therefore have a stronger attraction

Question 8

Describe hydration

Answer 8

When an ionic lattice is broken the ions become part of the solution
Positive ions gets attracted towards slightly negative oxygen and negative ions get attracted towards the slightly positive hydrogen

Question 9

What are the factors that impact the magnitude of the enthalpy of hydration

Answer 9

Size of ion
Charge on the ion