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 $E_{1} < E_{2}$.

$A \to A^{+} + e, E_{1}$ 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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