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(A) $He, Li^{+}$,and $Be^{2+}$ are isoelectronic species,each containing $2$ electrons.For isoelectronic species,the ionisation enthalpy increases as

Vedclass · Accepted Answer

$He < Li^{+} < Be^{2+}$

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(A) $He, Li^{+}$,and $Be^{2+}$ are isoelectronic species,each containing $2$ electrons.For isoelectronic species,the ionisation enthalpy increases as the nuclear charge $(Z)$ increases.The atomic numbers are: $He = 2$,$Li = 3$,$Be = 4$.Since the number of electrons $(e)$ is the same $(2)$ for all,the effective nuclear charge increases in the order $He Therefore,the ionisation enthalpy follows the order: $He < Li^{+} < Be^{2+}$.

The correct increasing order of ionisation enthalpy of $He, Li^{+}, Be^{2+}$ is

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