# Problem: Consider an ionic compound, MX, composed of generic metal M and generic, gaseous halogen X.The enthalpy of formation of MX is ΔH°f = -453 kJ/mol. The enthalpy of sublimation of M is ΔHsub = 127 kJ/mol. The ionization energy of M is IE = 431 kJ/mol. The electron affinity of X is ΔHEA = -301 kJ/mol. The bond energy of X2 is BE = 171 kJ/mol.Determine the lattice energy of MX.

###### FREE Expert Solution

We’re being asked to calculate the lattice energy of MX

Recall that lattice energy is the energy required to combine two gaseous ions into a solid ionic compound:

Mx+(g) + Ny–(g)  MyNx(s)

To calculate for lattice energy, we need to do the Born-Haber cycle for MX

2 M(s) + X2(g)  2 MX(s), ΔH˚f

89% (118 ratings) ###### Problem Details

Consider an ionic compound, MX, composed of generic metal M and generic, gaseous halogen X.

The enthalpy of formation of MX is ΔH°f = -453 kJ/mol. The enthalpy of sublimation of M is ΔHsub = 127 kJ/mol. The ionization energy of M is IE = 431 kJ/mol. The electron affinity of X is ΔHEA = -301 kJ/mol. The bond energy of X2 is BE = 171 kJ/mol.

Determine the lattice energy of MX.