In which of the following options are the ele | vedclass

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(A) $1$. 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

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$F < N < P < Si < Na$

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(A) $1$. 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.$2$. 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 $3$)$3$. Across Period $2$: $F $4$. Across Period $3$: $P $5$. Since Period $3$ elements have more shells than Period $2$ elements, they are larger.$6$. Combining these, the increasing order of atomic radius is $F < N < P < Si < Na$.

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

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