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 $Ne > O > F > N$.

$I.E.$	$1^{st}$	$2^{nd}$	$3^{rd}$	$4^{th}$	$5^{th}$
Value	$577.5$	$1810$	$2750$	$11580$	$14820$

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

Similar Questions

How many ionisation energies can carbon have?

The elements which occupy the peaks of the ionisation energy curve are

The correct order of first ionization enthalpy values of the following elements is:
$A. O$,$B. N$,$C. Be$,$D. F$,$E. B$
Choose the correct answer from the options given below:

For one of the elements,various successive ionization enthalpies (in $kJ \cdot mol^{-1}$) are given below:

$I.E.$ $1^{st}$ $2^{nd}$ $3^{rd}$ $4^{th}$ $5^{th}$

Value $577.5$ $1810$ $2750$ $11580$ $14820$

The element is:

The correct order of second ionization potential of carbon,nitrogen,oxygen and fluorine is

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