Chapter 6, Problem 6.92SP

Calculate overall energy changes in kilojoules per mole for the formation of MgF(s) and ${\text{MgF}}_{\text{2}}\left(s\right)$ from their elements.In light of your answers, which compound is more likely to form in the reaction of magnesium with fluorine, MgF or ${\text{MgF}}_2$ ? The following data are needed:
$\begin{array}{l}{E}_{\text{ea}}\text{for F}\left(g\right)=-\text{328 kJ/mol}\\ E_{\text{i1}}\text{for Mg}\left(g\right)=+\text{737}.\text{7 kJ/mol}\\ E_{\text{i2}}\text{for Mg}\left(g\right)=+\text{1450}\text{.7 kJ/mol}\\ \text{Heat of sublimation for Mg}\left(s\right)=+1\text{47}.7\text{ kJ/mol}\\ {\text{Bond dissociation energy for F}}_{\text{2}}\left(g\right)=+\text{158 kJ/mol}\\ {\text{Lattice energy for MgF}}_2\left(s\right)=+2952\text{ kJ/mol}\\ \text{Lattice energy for MgF}\left(s\right)=930\text{ kJ/mol}\left(\text{estimated}\right)\end{array}$