Identify the element with the lowest electron | vedclass

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(B) Electronegativity generally increases across a period from left to right and decreases down a group.Comparing the given elements: $O$ and $F$ are

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$S$

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(B) Electronegativity generally increases across a period from left to right and decreases down a group.Comparing the given elements: $O$ and $F$ are in the $2^{nd}$ period,while $S$ and $Cl$ are in the $3^{rd}$ period.Since electronegativity decreases down a group,the elements in the $3^{rd}$ period ($S$ and $Cl$) have lower electronegativity than those in the $2^{nd}$ period ($O$ and $F$).Between $S$ and $Cl$,$S$ is to the left of $Cl$ in the $3^{rd}$ period,therefore $S$ has the lowest electronegativity among the given options.

Identify the element with the lowest electronegativity.

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