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Why second ionization enthalpy is always...

Why second ionization enthalpy is always higher than the first ionisation enthalpy for every element?

Text Solution

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Electron is more tightly bound by the nucleus in an cation (i.e `M^(+))` as the number of proton remains the same as in neutral atom whereas number of electron is one less than the proton. This increases the attraction between the valence sheel electrons and the nucleus `(Z_(eff)` increases). So, second ionization enthalpy is always higher than the first ionisation enthalpy for every element.
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Alkaline earth metals always form divalent cations even though their second ionization enthalpies are almost double than their first ionization enthalpies.

Alkaline earth metals always form divalent cations even through their second ionization enthalpies are almost double than their first ionization enthalpies . Explain .

Knowledge Check

  • The second ionization enthalpy is

    A
    smaller than the first ionization enthalpy
    B
    salmost equal to the first ionizationn enthalpy
    C
    smallerr than the third ionization enthalpy
    D
    equal to the second electron gain enthalpy.

  • The second ionisation enthalpy is

    A
    smaller than the first ionisation enthalpy
    B
    almost equal to the first ionisation enthalpy
    C
    smaller than the third ionisation enthalpy
    D
    equal to the second electron gain enthalpy.

  • The second ionisation energy is always higher than the first ionisation energy because the

    A
    ions become more stable by attaining an octet and duplet configuration
    B
    electron is more tightly bound to the nucleus in an ion
    C
    electron is attracted more by the core electrons
    D
    none of the above

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    Why are the first ionization enthalpies of group 1 elements low?

    Why is first ionization enthalpy of Cu higher than that of Na ?

    First ionisation enthalpy of Be is higher than B.

    The second ionisation enthalpies of elements are always higher than their first ionisation enthalpies because:

    The first ionization enthalpy of magnesium is lower than the first ionizxation enthalpy of

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