Melting point of calcium halides decreases in the order.

Melting point of calcium halides decreases in the order.
  1. $\mathrm{CaF}_{2}>\mathrm{CaCl}_{2}>\mathrm{CaBr}_{2}>\mathrm{Cal}_{2}$
  2. $\mathrm{Cal}_{2}>\mathrm{CaBr}_{2}>\mathrm{CaCl}_{2}>\mathrm{CaF}_{2}$
  3. $\mathrm{CaBr}_{2}>\mathrm{Cal}_{2}>\mathrm{CaF}_{2}>\mathrm{CaCl}_{2}$
  4. $\mathrm{CaCl}_{2}>\mathrm{CaBr}_{2}>\mathrm{Cal}_{2}>\mathrm{CaF}_{2}$

Solution

Melting point of calcium halide decreases in the order.
$\mathrm{CaF}_{2}>\mathrm{CaCl}_{2}>\mathrm{CaBr}_{2}>\mathrm{CaI}_{2}$
Size of $\mathrm{Ca}^{2+}$ ions are comparatively smaller than halide ions. Since Ca belongs to the alkaline earth metal group the strength of the bond is higher when the two ions have comparable sizes. The size of $\mathrm{Ca}^{2+}$ is similar to fluorine ions. So stronger is the bond, while the bond becomes less strong as we move down to the group. So the melting point will also decreases *

Asked in: JEE-TOPICTESTS-CHEMISTRY

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