The correct order of atomic radii of N,F,Al,a | vedclass

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Question

(D) In the periodic table,atomic radii decrease from left to right across a period and increase from top to bottom down a group.$N$ and $F$ belong to

Vedclass · Accepted Answer

$Al > Si > N > F$

Vedclass · Answer

(D) In the periodic table,atomic radii decrease from left to right across a period and increase from top to bottom down a group.$N$ and $F$ belong to period $2$,while $Al$ and $Si$ belong to period $3$.Since period $3$ elements have a larger principal quantum number $(n=3)$ than period $2$ elements $(n=2)$,$Al$ and $Si$ are larger than $N$ and $F$.Within period $3$,atomic radius decreases from left to right: $Al > Si$.Within period $2$,atomic radius decreases from left to right: $N > F$.Therefore,the correct order of atomic radii is $Al > Si > N > F$.

The correct order of atomic radii of $N$,$F$,$Al$,and $Si$ is:

Similar Questions

Choose the correct order of atomic radii of fluorine and neon (in $pm$) out of the options given below and justify your answer.

The radii of $F$,$F^{-}$,$O$ and $O^{2-}$ are in the order of:

$Na^{+}$,$Mg^{2+}$,$Al^{3+}$,and $Si^{4+}$ are isoelectronic. Their ionic size follows the order:

Consider the following species: $N^{3-}, O^{2-}, F^{-}, Na^{+}, Mg^{2+}, Al^{3+}$
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In $K^{+} F^{-}$ ionic,the ionic radius of $F^{-}$ is more,while the atomic radius of $K^{+}$ is:

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