If the colours of salts of transition element | vedclass

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(B) The colour of transition metal ions in aqueous solution is primarily due to $d-d$ transitions,which require the presence of unpaired electrons in

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$Ti^{4+}$

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(B) The colour of transition metal ions in aqueous solution is primarily due to $d-d$ transitions,which require the presence of unpaired electrons in the $d$-orbitals.$1$. Electronic configuration of $Ti$ $(Z=22)$: $[Ar] 3d^2 4s^2$. $Ti^{4+}$ ion: $[Ar] 3d^0 4s^0$. Since there are no unpaired electrons,$Ti^{4+}$ is colourless.$2$. Electronic configuration of $Ti^{3+}$ $(Z=22)$: $[Ar] 3d^1$. It has $1$ unpaired electron,so it is coloured.$3$. Electronic configuration of $Fe^{2+}$ $(Z=26)$: $[Ar] 3d^6$. It has $4$ unpaired electrons,so it is coloured.$4$. Electronic configuration of $Fe^{3+}$ $(Z=26)$: $[Ar] 3d^5$. It has $5$ unpaired electrons,so it is coloured.Therefore,the correct option is $B$.

If the colours of salts of transition elements are due to the presence of unpaired electrons in the transition metal ions,which of the following ions will be colourless in aqueous solution? (The atomic numbers of $Ti$ and $Fe$ are $22$ and $26$ respectively.)

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