A to A^{+} + e, E_{1} and A^{+} to A^{2+} + e | vedclass

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Question

(A) $E_{1}$ represents the first ionization energy $(I.E._{1})$,which is the energy required to remove the first electron from a neutral atom.$E_{2}$

Vedclass · Accepted Answer

$E_{1} < E_{2}$

Vedclass · Answer

(A) $E_{1}$ represents the first ionization energy $(I.E._{1})$,which is the energy required to remove the first electron from a neutral atom.$E_{2}$ represents the second ionization energy $(I.E._{2})$,which is the energy required to remove the second electron from a unipositive ion $(A^{+})$.Since the $A^{+}$ ion has a higher effective nuclear charge and a smaller size compared to the neutral atom $A$,it holds the remaining electrons more tightly.Therefore,more energy is required to remove the second electron than the first,leading to the relationship $E_{1} < E_{2}$.

Element	$IE_1$	$IE_2$	$IE_3$	Code	Element
$1$	$2080$	$3963$	$6130$	$(a)$	$H$
$2$	$520$	$7297$	$11810$	$(b)$	$Li$
$3$	$900$	$1758$	$14810$	$(c)$	$Be$
$4$	$800$	$2428$	$3660$	$(d)$	$B$
-	-	-	-	$(e)$	$Ne$

$A \to A^{+} + e, E_{1}$ and $A^{+} \to A^{2+} + e, E_{2}$. The energy required to pull out the two electrons are $E_{1}$ and $E_{2}$ respectively. The correct relationship between the two energies is:

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