Stable electronic configuration of a transition metal is:

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{9} 4 s^{2}

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1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{5}

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1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2}

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1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{6}

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Solution

The correct option is B $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{5}$
Generally, the elements having half-filled and completely filled outer electronic configurations are stable elements.

Here in given options the configuration: $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{5}$ contains half filled outer electronic configuration $(3 d^{5})$ .

Hence option B is correct.

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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"?

Q. Electrons are speed throughout the atom on different levels and subshells. The electron configuration for calcium is:

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2}

According to this configuration, how many electrons are found on the valence level?

Q. Two elements X and Y have the following electronic configurations

X = 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2}

and

Y = 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5}

. The formula of the compound formed by the combination of X and Y is :

Q. The general electronic configuration of transition metals is:

Which of the following elements belongs to the same group as the element having configuration 1s² 2s² 2p¹

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