The correct order of ionisation energy for co | vedclass

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(C) The general trend of ionisation energy across a period increases from left to right due to an increase in effective nuclear charge. However,nitrog

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$C  O$

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(C) The general trend of ionisation energy across a period increases from left to right due to an increase in effective nuclear charge. However,nitrogen $(N)$ has a stable electronic configuration $(1s^2 2s^2 2p^3)$ because its $2p$ subshell is exactly half-filled. This extra stability makes it harder to remove an electron from nitrogen compared to carbon $(C)$ and oxygen $(O)$. Therefore,the correct order of ionisation energy is $C  O$.

$B$	$801$
$Al$	$577$
$Ga$	$579$
$In$	$558$
$Tl$	$589$

Element	$IE_1 + IE_2$ $(kJ/mol)$	$IE_3 + IE_4$ $(kJ/mol)$
$P$	$2.45$	$8.82$
$Q$	$2.85$	$6.11$

The correct order of ionisation energy for comparing carbon,nitrogen,and oxygen atoms is:

Similar Questions

Among the following,which has the highest first ionization energy?

Which of the following processes is non-spontaneous?

The first ionization enthalpy values (in $kJ\,mol^{-1}$) of group $13$ elements are :

$B$ $801$

$Al$ $577$

$Ga$ $579$

$In$ $558$

$Tl$ $589$

How would you explain this deviation from the general trend?

The sum of $IE_1 + IE_2$ and $IE_3 + IE_4$ for elements $P$ and $Q$ are given below:

Element $IE_1 + IE_2$ $(kJ/mol)$ $IE_3 + IE_4$ $(kJ/mol)$

$P$ $2.45$ $8.82$

$Q$ $2.85$ $6.11$

Then,according to the given information,the incorrect statement$(s)$ is/are:

The ionization energy of hydrogen is:

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