Which of the following will be a coloured ion | vedclass

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(A, D) An ion is coloured if it has unpaired electrons in its $d$-orbitals,allowing for $d-d$ transitions.$1$. $Fe^{2+}$ $([Ar] 3d^6)$: Has $4$ unpair

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$Fe^{2+}$

Vedclass · Answer

(A, D) An ion is coloured if it has unpaired electrons in its $d$-orbitals,allowing for $d-d$ transitions.$1$. $Fe^{2+}$ $([Ar] 3d^6)$: Has $4$ unpaired electrons. It is coloured.$2$. $Cu^{+}$ $([Ar] 3d^{10})$: Has no unpaired electrons. It is colourless.$3$. $Sc^{3+}$ $([Ar] 3d^0)$: Has no unpaired electrons. It is colourless.$4$. $Mn^{2+}$ $([Ar] 3d^5)$: Has $5$ unpaired electrons. It is coloured.Note: Both $Fe^{2+}$ and $Mn^{2+}$ are coloured. However,in many standard contexts,$Mn^{2+}$ is specifically noted for its distinct pale pink colour,and $Fe^{2+}$ is green. Given the options,both $A$ and $D$ are technically correct. If a single choice is required,$Mn^{2+}$ is often the standard answer for $d^5$ systems.

List-$I$ (Transition metal,$M$)	List-$II$ ($E_{M^{2+}/ M}^{\ominus}$ in $V$)
$A$. $Ni$	$I$. $-1.18$
$B$. $Mn$	$II$. $-0.91$
$C$. $Fe$	$III$. $-0.25$
$D$. $Cr$	$IV$. $-0.44$

Which of the following will be a coloured ion?

Similar Questions

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.)

The aqueous solution of which of the following ion is colourless?

In transition elements,the orbitals that are partially filled by electrons are:

Match the following:

List-$I$ (Transition metal,$M$) List-$II$ ($E_{M^{2+}/ M}^{\ominus}$ in $V$)

$A$. $Ni$ $I$. $-1.18$

$B$. $Mn$ $II$. $-0.91$

$C$. $Fe$ $III$. $-0.25$

$D$. $Cr$ $IV$. $-0.44$

The correct answer is

Identify the ferromagnetic element from the following.

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