In which of the following options,elements ar | vedclass

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(A) The atomic radius decreases across a period from left to right due to an increase in effective nuclear charge,and it increases down a group due to

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$F < N < P < Si < Na$

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(A) The atomic radius decreases across a period from left to right due to an increase in effective nuclear charge,and it increases down a group due to the addition of new shells. Comparing the given elements: $F$ (Fluorine,Group $17$,Period $2$) $N$ (Nitrogen,Group $15$,Period $2$) $P$ (Phosphorus,Group $15$,Period $3$) $Si$ (Silicon,Group $14$,Period $3$) $Na$ (Sodium,Group $1$,Period $3$) Across Period $2$: $F Across Period $3$: $P Since Period $3$ elements have more shells than Period $2$ elements,they are larger. Combining these,the increasing order of atomic radius is $F < N < P < Si < Na$.

In which of the following options,elements are correctly arranged in the increasing order of their atomic radius?

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