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Second ionization enthalpy (IE2) for alk...

Second ionization enthalpy (IE2) for alkali metals (Li, Na, K etc.) is very high as compared to their `IE_1` values. Explain why?

Text Solution

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This is due to following reasons:
(i) After the removal of first electron, the atom changes into a positive ion in which the electrons are held more tightly by the nucleus.
(ii) The second electron is to be removed from a lower shell and more energy is required for this purpose.
(iii) Positive ion formed by the removal of first electron in case of alkali metals has a stable noble gas configuration. Due to the similar reasons, the third I.E. values for Be and Mg are also very high.
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Knowledge Check

  • First ionisation energy of alkali metals is very low but second ionisation energy is very high because

    A
    alkali metals acquire noble gas configuration after losing one electron
    B
    a large amount of energy is required to remove electron from a cation
    C
    alkali metals can form only univalent ions
    D
    first group elements can lose only one electron.

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