4.1 Lattice Enthalpy

Question 1

Lattice Enthalpy
(Endothermic)

Answer 1

The enthalpy change when one mole of an ionic compound is converted into its constituent gaseous ions.

Question 2

First Ionisation Energy
(Endothermic)

Answer 2

The energy required to convert one mole of gaseous atoms into gaseous ions with a single positive charge.

Question 3

Second Ionisation Energy
(Endothermic)

Answer 3

The energy required to convert one mole of gaseous ions with a single positive charge to gaseous ions with a double positive charge.

Question 4

First Electron Affinity
(Mostly Exothermic)

Answer 4

The enthalpy change when one mole of gaseous atoms is converted to gaseous ions with a single negative charge.

Question 5

Second Electron Affinity
(Endothermic)

Answer 5

The enthalpy change when one mole of gaseous ions with a single negative charge is converted to gaseous ions with a double negative charge.

Question 6

Standard Enthalpy of Atomisation
(Endothermic)

Answer 6

The enthalpy change when one mole of gaseous atoms is formed from the element in its standard state in standard conditions.

Question 7

Standard Enthalpy Of Formation
(Mostly Exothermic)

Answer 7

The enthalpy change when one mole of the substance is formed from its elements under standard conditions.

Question 8

Bond (Dissociation) Energy
(Endothermic)

Answer 8

The energy required to break one mole of a specific bond.

Question 9

Hess’ Law

Answer 9

The total enthalpy change for a reaction is independent of the route taken, provided initial and final conditions are the same.

Question 10

Enthalpy of Solution
(Endothermic or Exothermic)

Answer 10

The enthalpy change when one mole of solute dissolves in water.

Question 11

Enthalpy of Hydration
(Exothermic)

Answer 11

The enthalpy change when one mole of gaseous ions is converted to one mole of aqueous ions.