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(C) The first ionization enthalpy $(IE_1)$ generally increases across a period from left to right.For the given elements ($Al$,$Si$,$C$,$N$),they belo

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$N$

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(C) The first ionization enthalpy $(IE_1)$ generally increases across a period from left to right.For the given elements ($Al$,$Si$,$C$,$N$),they belong to the $2^{nd}$ and $3^{rd}$ periods.$Al$ and $Si$ are in the $3^{rd}$ period,while $C$ and $N$ are in the $2^{nd}$ period.Elements in the $2^{nd}$ period have higher ionization enthalpies than those in the $3^{rd}$ period due to smaller atomic size.Comparing $C$ and $N$ in the $2^{nd}$ period,$N$ has a higher $IE_1$ than $C$ because of its stable half-filled $p$-orbital configuration $(2s^2 2p^3)$.Therefore,the order of $IE_1$ is $Al < Si < C < N$.

The element having the highest first ionization enthalpy is

Similar Questions

Consider the elements $Ne$,$Na$,and $Mg$. The element with the highest first ionization enthalpy and the element with the lowest second ionization enthalpy,respectively,are:

Which has maximum first ionization potential?

Ionisation energy in group $I$ elements varies in the decreasing order as:

Assertion : First ionization energy for nitrogen is lower than oxygen.
Reason : Across a period effective nuclear charge decreases.

The first ionisation energy of oxygen is less than that of nitrogen. Which of the following is the correct reason for this observation?

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