Lattice Energy The following compounds all display the $\mathrm{NaCl}$ structure. (i.e. They are isomorphous.) For each pair, indicate which would have the lattice energy of greater magnitude. $\mathrm{SrTe}$ $\mathrm{SrS}$ $\mathrm{NaI}$ $\mathrm{BaO}$ $\mathrm{MgO}$ $\mathrm{CaO}$ $\mathrm{KCl}$ $\mathrm{RbCl}$ $\mathrm{MgO}$ $\mathrm{MgSe}$
Born-Fajans-Haber Cycle Suppose a chemist discovers a new metallic element and names it "Xtrinsium" (Xt). $\mathrm{Xt}$ exhibits chemical behaviour similar to an alkaline earth. \[ X t(s)+F_{2}(g) \rightarrow X t F_{2}(s) \] Lattice energy for $\mathrm{XtF}_{2}$ First Ionization energy of $\mathrm{Xt}$ Second Ionization energy of $\mathrm{Xt}$ Electron affinity of $\mathrm{F}$ Bond energy of $\mathrm{F}_{2}$ Enthalpy of sublimation (atomization) of $\mathrm{Xt}$ $-2140 . \mathrm{kJ} / \mathrm{mol}$ 360. $\mathrm{kJ} / \mathrm{mol}$ $648 \mathrm{~kJ} / \mathrm{mol}$ $-327.8 \mathrm{~kJ} / \mathrm{mol}$ $154 \mathrm{~kJ} / \mathrm{mol}$ 200. $\mathrm{kJ} / \mathrm{mol}$ Use the above data to calculate $\Delta H^{\circ}{ }_{f}$ for Xtrinsium fluoride.

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