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Why are the ionisation energies of 5d el...

Why are the ionisation energies of 5d elements greater than 3d elements?

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In the 5d series, after alnthanium `(Z=57)` there is lanthanoid contraction. In each group the size of 5d elements Hence, ionisation energies of 5d elements are greater tan 3d elements.
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Knowledge Check

  • The ionisation energy of an element is

    A
    The same as the electron affinity of the element
    B
    Equal in magnitude but of opposite sign to the electron affinity of the element
    C
    The energy released when an electron is added to an atom of the element
    D
    The energy required to remove the outermost electron of an atom of the element

  • The ionisation energies of tranition elements are:

    A
    less than p-block elements
    B
    more than s-block elements
    C
    less than s-block elements
    D
    more than p-block elements.

  • Consider the following statements I.First ionisation energy of group 2 elements is greater than the corresponding elements of group 13 II.it is always difficult to pull out electrons from stable configuration Select the correct statement

    A
    only I
    B
    Only II
    C
    I and II
    D
    none of these

    • Similar Questions

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    Why is the second ionisation energy for a given element always greater than the first ionisation energy?

    Account for the following : (b) The Ist ionization energy of the 5d series are higher than 3d and 4d, transition elements in respective groups.

    The first ionisation energies of the elements of the transition series.

    How does the ionisation energy of 1st group elements very ?

    Higher values of ionisation energies of the 5d-transition elements are consistent with the:

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