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(C) $1$. Atomic radius decreases across a period from left to right due to an increase in effective nuclear charge $(Z_{	ext{eff}})$.$2$. As we move

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group $17$

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(C) $1$. Atomic radius decreases across a period from left to right due to an increase in effective nuclear charge $(Z_{	ext{eff}})$.$2$. As we move from $Group \ 1$ to $Group \ 17$, the atomic radius decreases.$3$. $Group \ 18$ elements (noble gases) have larger atomic radii than $Group \ 17$ elements because their radii are defined as van der Waals radii, which are significantly larger than covalent radii.$4$. Therefore, $Group \ 17$ elements (halogens) possess the smallest covalent atomic radii in their respective periods.

Which group elements have the smallest atomic radii in their respective periods?

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Assertion $(A)$: The ionic radii of $Na^{+}$ and $F^{-}$ are same.
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