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(B) The energy required to remove an electron from a gaseous atom or ion is called ionization energy.Successive ionization energies always increase be

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$Al^{2+}_{(g)} \longrightarrow Al^{3+}_{(g)} + e^-$

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(B) The energy required to remove an electron from a gaseous atom or ion is called ionization energy.Successive ionization energies always increase because the effective nuclear charge increases as electrons are removed,making it harder to pull the next electron away.For Aluminum $(Al)$,the successive ionization energies are $IE_1 - $IE_1$: $Al_{(g)} \longrightarrow Al^{+}_{(g)} + e^-$- $IE_2$: $Al^{+}_{(g)} \longrightarrow Al^{2+}_{(g)} + e^-$- $IE_3$: $Al^{2+}_{(g)} \longrightarrow Al^{3+}_{(g)} + e^-$Since $IE_3$ involves removing an electron from a more positively charged ion $(Al^{2+})$,it requires the highest amount of energy.

Which of the following processes requires the largest amount of energy?

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