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The outer electronic configuration of th...

The outer electronic configuration of the ground state chromium atom is `3d^(2),4s^(2)`

Text Solution

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`Cr(Z = 24)`
`[Ar]3d^(6)4s^(1)`
This is because `d^(5)` is a more half -filled configuration Reason for the stablity of half-filled and fallty filled ortained are symmetry and excharge energy
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The outer electronic configuration of chromium atom is 3d^4 4s^2

What may the possible oxidation state of transition metals with the following electronic configurations in the ground state of their atoms ? (i) 3d^(3)4s^(2) (ii) 3d^(5)4s^(2) (iii) 3d^(6)4s^(2) .

Knowledge Check

  • The outer electronic configuration of chromium is

    A
    `4s^2 3d^5`
    B
    `4s^1 3d^5`
    C
    `4s^2 3d^4`
    D
    `4s^2 3d^6`

  • The electronic configuration of silver atom in ground state is.

    A
    `[Kr] 3d^10 4 s^1`
    B
    `[Xe] 4f^14 5 d^10 6 s^1`
    C
    `[Kr] 4 d^10 5 s^1`
    D
    `[Kr]4 d^9 5 s^2`

  • The correct ground state electronic configuration of chromium atom is :

    A
    `[Ar]3d^(5)4s^(1)`
    B
    `[Ar]3d^(4)4s^(2)`
    C
    `[Ar]3d^(6)4s^(0)`
    D
    `[Ar]4d^(5)4s^(1)`

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    What may be the stable oxidation state of the transition elements with the following d electron configurations in the ground state of their atoms: 3d^(3),3d^(5),3d^(4)?

    The outer electronic configurations of two transition metals are (i) 3d^(5)4s^(2) and (ii) 3d^(6)4s^(2) respectively. Based on this information predict the relative stability of +2 and +3 oxidation state of these metals. Which of the two exhibits larger number of oxidation states ?

    The correct state electronic configuration of chromium atom is

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    The ground state electronic configuration of chromium is against

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