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p-Block Elements - I
hard
Explain the following :
$(1)$ Gallium has higher ionisation enthalpy than aluminum.
$(2)$ Boron does not exist as $B^{3+}$ ion.
Option A
Option B
Option C
Option D
Solution
The ionization enthalpy value of $\mathrm{Ga}$ is higher than $\mathrm{Al}$ due to inability of $d$ – and $f$-electrons, which have screening effect, to compensate the increase in nuclear charge.
Boron has small size and sum of $\Delta_{i} \mathrm{H}_{1}+\Delta_{i} \mathrm{H}_{2}+\Delta_{i} \mathrm{H}_{3}$ is very high. Boron does not form $\mathrm{B}^{3+}$ ion therefore, give covalent compounds.
Standard 11
Chemistry
