Write the reaction of the formation of the ionic compound $MgCl,$ from its elements $($in elemental form at STP$)$:

$A{H}_1=-542k\frac{J}{m}ol$

Next to each piece of useful information below, write the representative chemical reaction: $($Make sure to include phasesi$)$

Heat of sublimation for $M_B(s)=147\mathrm{.}7k\frac{J}{m}ol$

a$.$

$E{l}_1$ for $MB(B)=737\mathrm{.}7k\frac{J}{m}ol$

b$.$

$E{l}_2$ for $MB(B)=1450\mathrm{.}7k\frac{J}{m}ol$

c$.$

Bond dissociation energy for $C{l}_2(B)=121\mathrm{.}5k\frac{J}{m}ol$

d$.$

$E{A}_1$ for $Cl=-348\mathrm{.}6k\frac{J}{m}ol$

e$.$

Diagram $($pictorially showing atoms, phases, ions, etc.$)$ the process $($step by stepl$)$ of the formation of the ionic compound $MBC{l}_2$ from its elements.

Then label each according to the reactions shown in $112.$

Calculate the lattice energy in kilojoules per mole for the formation of $MgC{l}_2(s)$ from the reaction: