9.3 Bonding in Crystalline Solids

If the dissociation energy were larger, would that make it easier or more difficult to break the solid apart?

Why is the equilibrium separation distance between $\text{K}^{+} \text{and} \text{Cl}^{−}$ different for a diatomic molecule than for solid KCl?

In sodium chloride, how many $\text{Cl}^{–}$ atoms are “nearest neighbors” of $\text{Na}^{+}$? How many $\text{Na}^{+}$ atoms are “nearest neighbors” of $\text{Cl}^{−}$ ?

The NaCl crystal structure is FCC. The equilibrium spacing is $r_{0} = 0.282 \text{nm}$. If each ion occupies a cubic volume of $r_{0}^{3}$, estimate the distance between “nearest neighbor” $\text{Na}^{+}$ ions (center-to-center)?

The CsI crystal structure is BCC. The equilibrium spacing is approximately $r_{0} = 0.46 \text{nm}$. If $\text{Cs}^{+}$ ion occupies a cubic volume of $r_{0}^{3}$, what is the distance of this ion to its “nearest neighbor” $\text{I}^{+}$ ion?

The measured density of a NaF crystal is $2.558 \text{g}/\text{cm}^{3}$. What is the equilibrium separate distance of $\text{Na}^{+}$ and $\text{Fl}^{−}$ ions?

Determine the dissociation energy of 12 moles of sodium chloride (NaCl). (Hint: the repulsion constant n is approximately 8.)

What value of the repulsion constant, n, gives the measured dissociation energy of 171 kcal/mol for KCl?