MCQ
Amongst the elements with following electronic configurations, which one of them may have the highest ionisation energy ?
- A$Ne \ [3s^2 \ 3p^2]$
- B$Ar\ [3d^{10} \ 4s^2 \ 4p^3]$
- C$Ne\ [3s^2 \ 3p^1]$
- ✓$Ne \ [3s^2 \ 3p^3]$
✓
Answer
Correct option: D.
$Ne \ [3s^2 \ 3p^3]$
d
Ionisation energy usually increases from left to right in a period with a decrease in atomic size and decrease from up to down in a group with an increase in atomic size.
Ionisation energy usually increases from left to right in a period with a decrease in atomic size and decrease from up to down in a group with an increase in atomic size.
$\left[\text {Ne}\right] 3 s^{2} 3 p^{3}=\text { Group } V$
$[\mathrm{Ne}] 3 \mathrm{s}^{2} 3 \mathrm{p}^{2}=$ $\mathrm{IV}$
$[\mathrm{Ar}] 3 \mathrm{d}^{10} 4 \mathrm{s}^{2} 4 \mathrm{p}^{3}=$ Group $\mathrm{V}$
$\left[\text {Ne}\right] 3 s^{2} 3 p 1=$ Group $\mathrm{III}$
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