Chapter 6, Problem 6.88CP

Interpretation Introduction

Interpretation:

Calculate the overall energy in kilojoules per mole for the formation of $MgF\left(s\right)$ and $Mg{F}_2\left(s\right)$ from their elements. Find the compound - $MgF\left(s\right)$ or $Mg{F}_2\left(s\right)$ which is more probable to form in the reaction of magnesium with fluorine.
The data is given as follows:

$E_{ea}forF(g)=-328kJ/mol$

$E_{i1}forMg(g)=\text{ +737}\text{.7 }kJ/mol$

$E_{i2}forMg(g)=\text{ +1450}\text{.7 }kJ/mol$

$HeatofsublimationforMg(g)=\text{ +147}\text{.7 }kJ/mol$

$Bonddissociationenergyfor{F}_2(g)=\text{ +158 }kJ/mol$

$LatticeenergyforMg{F}_2(s)=\text{ +2952 }kJ/mol$

$LatticeenergyforMgF(s)=\text{ +930 }kJ/mol$

Concept Introduction:
Calculate the net energy change for the formation of the compounds $MgF\left(s\right)$ or $Mg{F}_2\left(s\right)$. The compound with the more negative energy change is more likely to be formed in the reaction.