Consider the following elements $\mathrm{In}, \mathrm{Tl}, \mathrm{Al}, \mathrm{Pb}, \mathrm{Sn}$ and Ge.…

Consider the following elements $\mathrm{In}, \mathrm{Tl}, \mathrm{Al}, \mathrm{Pb}, \mathrm{Sn}$ and Ge.
The most stable oxidation states of elements with highest and lowest first ionisation enthalpies, respectively, are
  1. $+4$ and +1
  2. +1 and +4
  3. +4 and +3
  4. +2 and +3

Solution

Among $\mathrm{Al}, \mathrm{In}, \mathrm{Tl}, \mathrm{Ge}, \mathrm{Sn}, \mathrm{Pb}$, the metal having highest $\mathrm{IE}_1$ is Ge and lowest $\mathrm{IE}_1$ is In.
Most stable oxidation state of Ge is +4 and In is +3.

Asked in: JEE Main 2025 (28 Jan Shift 1)

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