Which of the following electronic configurati | vedclass

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(D) Ionization energy decreases down a group and increases across a period. Alkali metals have the lowest ionization energy in their respective period

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

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(D) Ionization energy decreases down a group and increases across a period. Alkali metals have the lowest ionization energy in their respective periods due to their large atomic size and stable noble gas core configuration plus one valence electron $(ns^1)$. Among the given options,$1s^2 2s^2 2p^6 3s^1$ represents Sodium $(Na)$,which is an alkali metal and has the lowest ionization energy compared to the other elements listed (which are non-metals or metalloids in the second period).

Which of the following electronic configurations represents the element with the lowest ionization energy?

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