The correct answer is Option (2) → (A)-(II), (B)-(I), (C)-(III), (D)-(IV)
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List-I Transition metal ion
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List-II Property
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(A) $Mn^{3+}$
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(II) $3d^4$, violet
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(B) $Fe^{2+}$
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(I) $3d^6$, green
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(C) $Ti^{4+}$
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(III) $3d^0$, colorless
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(D) $V^{2+}$
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(IV) $3d^3$, violet
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(A) $Mn^{3+}$:
- Manganese ($Mn$) has the configuration $[Ar] 3d^5 4s^2$.
- $Mn^{3+}$ (loses 3 electrons) becomes $3d^4$.
- In aqueous solution, $Mn^{3+}$ ions typically appear violet.
- Match: (II)
(B) $Fe^{2+}$:
- Iron ($Fe$) has the configuration $[Ar] 3d^6 4s^2$.
- $Fe^{2+}$ (loses 2 electrons) becomes $3d^6$.
- Ferrous ions ($Fe^{2+}$) are well known for their pale green color.
- Match: (I)
(C) $Ti^{4+}$:
- Titanium ($Ti$) has the configuration $[Ar] 3d^2 4s^2$.
- $Ti^{4+}$ (loses 4 electrons) becomes $3d^0$.
- Since there are no electrons in the $d$-orbitals, $d-d$ transitions are impossible, making the ion colorless.
- Match: (III)
(D) $V^{2+}$:
- Vanadium ($V$) has the configuration $[Ar] 3d^3 4s^2$.
- $V^{2+}$ (loses 2 electrons) becomes $3d^3$.
- The $V^{2+}$ ion typically exhibits a violet color in solution.
- Match: (IV)
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