A neutral atom will have the lowest ionizatio | vedclass

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(D) The ionization potential is the energy required to remove the most loosely bound electron from an isolated gaseous atom.Ionization potential gener

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$1s^2, 2s^2, 2p^6, 3s^1$

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(D) The ionization potential is the energy required to remove the most loosely bound electron from an isolated gaseous atom.Ionization potential generally decreases down a group as the atomic size increases and the valence electron is further from the nucleus.Among the given options,$1s^1$ is Hydrogen,$1s^2, 2s^2, 2p^6$ is Neon (a noble gas with very high ionization potential),$1s^2, 2s^2, 2p^2$ is Carbon,and $1s^2, 2s^2, 2p^6, 3s^1$ is Sodium.Sodium $(Na)$ is an alkali metal in the third period,and its valence electron is in the $3s$ orbital,which is much further from the nucleus compared to the valence electrons of the other elements listed.Therefore,the configuration $1s^2, 2s^2, 2p^6, 3s^1$ corresponds to the lowest ionization potential.

$A$ neutral atom will have the lowest ionization potential when its electronic configuration is

Similar Questions

The ionization energy will be higher when the electron is removed from

If first ionization enthalpies of element $X$ and $Y$ are $419 \ kJ \ mol^{-1}$ and $590 \ kJ \ mol^{-1}$,respectively and second ionization enthalpies of $X$ and $Y$ are $3069 \ kJ \ mol^{-1}$ and $1145 \ kJ \ mol^{-1}$,respectively. Then the correct statement is :-

Which of the following species has the highest ionisation potential?

Which of the following has the highest first ionisation energy?

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