Question

For potassium chloride (KCl), calculate the radius ratio to show why the compound has the cesium chloride structure.

Answer 1

Explanation:

The radius for potassium ion, ${r^+}$  = 152 pm

The radium for the chloride ion, ${r^-}$  = 167 pm

$\frac {r^+}{r^-}=\frac {152}{167}=0.91018$

Cesium chloride has cubic unit cell and for the ionic compounds to have such lattice, the condition is:

${\frac {r^+}{r^-}}\geq 0.732$

Thus, for potassium chloride, the ratio is 0.91018 and it is greater than 0.732. It exists in the cesium chloride structure.

Answer 2

The compound exists in the cesium chloride structure as the ration if 0.91018 and it greater than 0.732.

Potassium Chloride (KCl):

According to the question,

For potassium ion, the radius is:

$r^+ = 152 \ pm$

For chloride ion, the radius is:

$r^- = 167 \ pm$

→ The ratio will be:

$\frac{r^+}{r^-} = \frac{152}{167}$

    $= 0.91018$

Cesium chloride contains a cubic unit cell, and always a lattice has been common in ionic compounds.

The condition will be:

→ $\frac{r^+}{r^-}= 0.732$

Thus the response above is correct.

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