The electron configuration for the noble gas with the highest first ionization energy is:

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

1 s^{2}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

1 s^{2} 2 s^{2} 2 p^{6} 3 p^{1}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is D $1 s^{2}$
The electron configuration for the noble gas with the highest first ionization energy is $1 s^{2}$
The noble gas with the highest first ionization energy is $H e$ .
As we move down the group, extra shells of electrons are added which decreases the ionization energy. $H e$ has atomic number 2 and only first energy level. The electrons are closer to nucleus which results in maximum attraction between nucleus and electrons and maximum ionization energy.

Suggest Corrections

Similar questions

{1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{1}

{1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{1}

{1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{5}

{1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{6} {4 s}^{1}

{(I E)}_{1}

{(I E)}_{4}

The electronic configuration of Ti is 1 $s^{2}$ 2 $s^{2}$ 2 $p^{6}$ 3 $s^{2}$ 3 $p^{6}$ 3 $d^{2}$ 4 $s^{2}$ and it represents

\begin{matrix} List-I & List - II P. & 1 s^{2} & 1. & Element shows highest negative oxidation state Q. & 1 s^{2} 2 s^{2} 2 p^{5} & 2. & Element shows highest first ionisation enthalpy R. & 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5} & 3. & Element shows highest electronegativity on Pauling scale S. & 1 s^{2} 2 s^{2} 2 p^{2} & 4. & Element shows maximum electron gain enthalpy (most exothermic) \end{matrix}

Join BYJU'S Learning Program