# Calculating lattice energy on ionic compound

## Homework Statement

Given the following thermodynamic data, calculate the lattice energy of CaBr2(s) caculate the lattice enegy:

(A) Δ°Hf CaBr2(s) = -675 kJ/mol
(B) Δ°Hf Ca(g) = 179 kJ/mol
(C) Δ°Hf Br(g) = 112 kJ/mol
(D) 1st ionization energy of Ca = 590 kJ/mol
(E) 2nd ionization energy of Ca = 1145 kJ/mol
(F) Electron affinity of Br = -325 kJ/mol

## Homework Equations

Heats of Formation + ionization energies + electron affinity - lattice energy = heat of formation

## The Attempt at a Solution

(B) + (C) + (D) + (E) + (F) + Lattice Energy = -675

solving for lattice energy:

[179 + 112 + 590 + 1145 + -325] + Lattice Energy = -675

Lattice energy = -675 - 1701

Lattice energy = -2376 kJ/mol

I think I am going wrong with something in the calculations of the energy bromine contributes to the equation. I know bromine is diatomic but I'm not sure how to incorporate that into the equation. I don't want you to give me the answer because I really want to be able to do this on my own but anything you can point out that can get me in the right direction are appreciated.