The melting points of (i) BeCl_2, (ii) CaCl_2 | vedclass

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Question

(B) Key Point: $A$ compound with more ionic character has a higher melting point.$Be$ and $Ca$ belong to the same group $(2)$, and ionic character inc

Vedclass · Accepted Answer

$iii < i < ii$

Vedclass · Answer

(B) Key Point: $A$ compound with more ionic character has a higher melting point.$Be$ and $Ca$ belong to the same group $(2)$, and ionic character increases down the group due to the decrease in polarizing power of the cation.Thus, $BeCl_2$ is more covalent (less ionic) than $CaCl_2$, so $CaCl_2$ has a higher melting point than $BeCl_2$.$HgCl_2$ is highly covalent due to the pseudo-noble gas configuration of $Hg^{2+}$ ($18$ electrons in the outer shell), which exerts a high polarizing power on the chloride ion.Therefore, the order of melting points is $CaCl_2 > BeCl_2 > HgCl_2$, which corresponds to $(ii) > (i) > (iii)$.This is equivalent to $iii < i < ii$.

The melting points of $(i)$ $BeCl_2$, $(ii)$ $CaCl_2$, and $(iii)$ $HgCl_2$ follow the order:

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