Oceans

Question 1

Define the lattice dissociation enthalpy

Answer 1

The enthalpy change when one mole of a solid ionic compound is completely dissociated into its gaseous constituent ions under standard conditions.

Question 2

Define the lattice formation enthalpy

Answer 2

The enthalpy change when one mole of a solid ionic compound is formed from its gaseous constituent ions under standard conditions.

Question 3

Define the Enthalpy of solution

Answer 3

The enthalpy change one mole of ionic solid is dissolved in water to infinite dilution so that the ions no longer interact under standard conditions.

Question 4

Define the Enthalpy of hydration

Answer 4

The enthalpy change when one mole of gaseous ions is dissolved in water to form one mole of aqueous ions under standard conditions.

Question 5

What factors effect Hydration and Lattice Enthalpy?

Answer 5

The smaller the ion the greater the attraction, increasing the enthalpy.
The greater the nuclear charge the greater the attraction, increasing the enthalpy

Question 6

What is Entropy?

Answer 6

Entropy is a measure of disorder. Higher entropy means more disorder.
Entropy increases from solids to liquids to gases and to an increase in temperature. Larger molecules have a greater disorder. Dissolving a substance increasing the entropy.

Question 7

How do you calculate entropy?

Answer 7

S Total = S System + S Surroundings
S System = S Products - S Reactants
S Surrounding = - ∆H/T

Question 8

What is the Solubility constant, Ksp?

Answer 8

T