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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.

List-$I$ (Electronic configuration of neutral atom where $n=2$)	List-$II$ ($1^{st}$ Ionization Energy in $\text{kJ mol}^{-1}$)
$A. ns^2$	$I. 2080$
$B. ns^2np^1$	$II. 899$
$C. ns^2np^3$	$III. 800$
$D. ns^2np^6$	$IV. 1402$

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

Similar Questions

Which of the following represents the correct order of first ionization enthalpy?
$(i) \ Li < B < Be < C$ $(ii) \ O < N < F$ $(iii) \ Be < N < Ne$

Both nitrogen and oxygen have electrons in the $2p$ orbital. In which of these is the electron-electron repulsion greater,and what is its effect?

The first ionization enthalpies of $N$ and $O$ are respectively....... $eV$.

Match List-$I$ with List-$II$:
List-$I$ (Electronic configuration of neutral atom where $n=2$) List-$II$ ($1^{st}$ Ionization Energy in $\text{kJ mol}^{-1}$)
$A. ns^2$ $I. 2080$
$B. ns^2np^1$ $II. 899$
$C. ns^2np^3$ $III. 800$
$D. ns^2np^6$ $IV. 1402$

Suppose a gaseous mixture of $He$, $Ne$, $Ar$ and $Kr$ is treated with photons of the frequency appropriate to ionize $Ar$. What ion$(s)$ will be present in the mixture?

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