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The electronic configuration of valence ...

The electronic configuration of valence shell of Cu is `3d^(10)4s^(1)` and not `3d^(9)4s^(2)`. How is this configuration explained?

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Configuration either exactly half-filled or fully filled orbitals are more stable due to symmetrical distribution of electrons and maximum exchange energy in `3d^(10)4s^(1)` d-orbitals are completely filled and s-orbital is half-filled. Hence it is more stable configuration.
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Knowledge Check

  • The ground state electronic configuration of Cu(29) is [Ar]3d^(10) 4s^(1) and not [Ar]3d^(0)4s^(2) . This is indicated by the fact that

    A
    Completely filled sub-shell configuration is more stable than one less filled sub-shell configuration.
    B
    Cu exhibits +1 ionic state besides `+2` states.
    C
    Copper turnings react with hot conc. `H_(2)SO_(4)` to evolve `SO_(2)(g)` rather than `H_(2)(g)`.
    D
    `Cu^(2+)` disproportionates in aqueous solution into `Cu^(2+)` and Cu.

  • Electronic configuration of M^(3+) is [Ar]3d^(10)4s^(2) , it belongs to

    A
    s-block
    B
    p-block
    C
    d-block
    D
    f-block

  • The element with electronic configuration 3d 4s is

    A
    Metalloid
    B
    Non-metal
    C
    Tansition metal
    D
    Noble gas

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    Explore conceptually related problems

    The electronic configuration of copper is [Ar] 4s^(1) 3d^(10) and not [Ar] 4s^(2) 3d^(9) . Justify.

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

    3 d^(10) 4 s^(0) electronic configuration exhibits

    Assertion : The outer electronic configuration of Cr and Cu are 3d^(5) 4s^(1) and 3d^(10) 4s^(1) respectively . Reason : Electrons are filled in orbitals in order of increasing energies given by (n+l) rule.

    The electron configuration of the element 'M' is [Ar] 3d^(10) 4s^(2) 4p^(3) . Then 'M' belong to

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