The correct order of IE_2 (second ionization | vedclass

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Question

(C) The second ionization enthalpy $(IE_2)$ corresponds to the energy required to remove an electron from a unipositive ion $(M^+ \rightarrow M^{2+} +

Vedclass · Accepted Answer

$Ne > O > F > N$

Vedclass · Answer

(C) The second ionization enthalpy $(IE_2)$ corresponds to the energy required to remove an electron from a unipositive ion $(M^+ \rightarrow M^{2+} + e^-)$.Electronic configurations of the corresponding unipositive ions are:$N^+: 1s^2 2s^2 2p^2$$O^+: 1s^2 2s^2 2p^3$$F^+: 1s^2 2s^2 2p^4$$Ne^+: 1s^2 2s^2 2p^5$As we move from $N^+$ to $Ne^+$,the effective nuclear charge increases,which generally increases $IE_2$.However,$N^+$ has a stable half-filled $2p$ subshell,and $Ne^+$ has a stable configuration. Comparing the values,the order is $Ne > O > F > N$.

List-$I$ ($IE_1, IE_2, IE_3$ in $kJ \ mol^{-1}$)	List-$II$ (Element)
$A$. $1510$	$1$. $H$
$B$. $495, 6500, 10200$	$2$. $Li$
$C$. $840, 1630, 13100$	$3$. $Be$
$D$. $600, 2050, 3100$	$4$. $B$

The correct order of $IE_2$ (second ionization enthalpy) is:

Similar Questions

Match List-$I$ with List-$II$ with correct code:

List-$I$ ($IE_1, IE_2, IE_3$ in $kJ \ mol^{-1}$) List-$II$ (Element)

$A$. $1510$ $1$. $H$

$B$. $495, 6500, 10200$ $2$. $Li$

$C$. $840, 1630, 13100$ $3$. $Be$

$D$. $600, 2050, 3100$ $4$. $B$

Which of the following sets has the highest sum of $IE$ values compared to all other sets mentioned?

The first four $I.E.$ values of an element are $284, 412, 656$ and $3210 \ kJ \ mol^{-1}$. The number of valence electrons in the element are

The electronic configurations of elements $A, B$ and $C$ are $[He] 2s^1$,$[Ne] 3s^1$ and $[Ar] 4s^1$ respectively. Which one of the following orders is correct for the first ionization potentials (in $kJ \ mol^{-1}$) of $A, B$ and $C$?

Which of the following has maximum first ionisation energy?

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