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Question

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

Vedclass · Accepted Answer

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

Vedclass · Answer

(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: $He < Li^{+} < Be^{2+}$.

$(IP)_1$	$7.1 \ eV$
$(IP)_2$	$10.3 \ eV$
$(IP)_3$	$36.2 \ eV$
$(IP)_4$	$39.1 \ eV$

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

Similar Questions

The ionization potential $(IP)$ values for an element are given below. Identify the element:
$(IP)_1$ $7.1 \ eV$
$(IP)_2$ $10.3 \ eV$
$(IP)_3$ $36.2 \ eV$
$(IP)_4$ $39.1 \ eV$

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