Which group elements have the smallest atomic | vedclass

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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?

Similar Questions

$O^{2-}, F^-, Na^+, Mg^{2+},$ and $Al^{3+}$ are isoelectronic ions. What do their ionic radii represent?

Which of the following ions has the maximum ionic radius?

Which of the following represents the correct order of ionic radii?

The ionic radii of $N^{3-}$,$O^{2-}$,$F^{-}$,and $Na^{+}$ follow the order:

In the isoelectronic species,the ionic radii in $\mathring{A}$ of $N^{3-}$,$O^{2-}$,and $F^{-}$ are respectively given by:

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