Give the electron configuration of the given metal (atom/ions).
$F e O_{4}^{2 -}$ (ferrate ion)

[A r] 3 s^{2}

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[A r] 4 s^{2}

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[A r] 3 d^{2}

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none of these

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Solution

The correct option is C $[A r] 3 d^{2}$
Atomic no. of iron is 26. Oxidation no. of iron in ferrate ion is +6..

Electron configuration of Fe(IV) cation in $F e O_{4}^{2 -}$ is $[A r] 3 d^{2}$ or
$1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{2} 4 s^{0}$

Option (C) is correct

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H^{-} (b) {N a}^{+} (c) O^{2 -} (d) F^{-}

.
(ii) What are the atomic numbers of elements whose outermost electrons are represented by

(a) {3 s}^{1} (b) {2 p}^{3}

and

(c) {3 d}^{1}

?
(iii) Which atoms are indicated by the following configurations ?
(a)

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(b)

[N e] {3 s}^{2} {3 p}^{3}

(c)

[A r] {4 s}^{2} {3 d}^{1}

Sir/Madam

In the structure of copper sulphate(CuSO4.5H2o),4 water molecules are coordinated and 1 is hydrogen bonded. The electronic configuration of Cu is [Ar]4s¹3d¹⁰. When the water molecules are sharing 8 electrons, it becomes 4s2 3d10 4p6 5s1. When cu becomes cu2+ion, the configuration becomes 4s2 3d10 4p5. But these 2 configurations aren't stable. Then why did cuso4.5h2o occurs at a reasonably good amount in nature. Kindly explain in "detail"?

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Give the electron configuration of the given metal (atom/ions).FeO2−4 (ferrate ion)

The correct option is C [Ar]3d2Atomic no. of iron is 26. Oxidation no. of iron in ferrate ion is +6.. Electron configuration of Fe(IV) cation in FeO2−4 is [Ar]3d2 or 1s22s22p63s23p63d24s0Option (C) is correct

Give the electron configuration of the given metal (atom/ions).
$F e O_{4}^{2 -}$ (ferrate ion)

The correct option is C $[A r] 3 d^{2}$
Atomic no. of iron is 26. Oxidation no. of iron in ferrate ion is +6..

Electron configuration of Fe(IV) cation in $F e O_{4}^{2 -}$ is $[A r] 3 d^{2}$ or
$1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{2} 4 s^{0}$

Option (C) is correct