Atomic radii of fluorine and neon in mathring | vedclass

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Question

(A) The atomic radius of fluorine is determined by its covalent radius,which is approximately $0.72 \ \mathring{A}$.Neon is a noble gas and does not f

Vedclass · Accepted Answer

$0.72, 1.60$

Vedclass · Answer

(A) The atomic radius of fluorine is determined by its covalent radius,which is approximately $0.72 \ \mathring{A}$.Neon is a noble gas and does not form covalent bonds under normal conditions,so its atomic radius is measured as the Van der Waal's radius,which is approximately $1.60 \ \mathring{A}$.Since the Van der Waal's radius is always larger than the covalent radius,the atomic radius of neon is significantly larger than that of fluorine.Therefore,the values are $0.72 \ \mathring{A}$ and $1.60 \ \mathring{A}$ respectively.

Atomic radii of fluorine and neon in $\mathring{A}$ units are respectively given by

Similar Questions

Which of the following ions has the smallest radius?

Largest in size out of $Na^{+}$,$Ne$,and $F^{-}$ is

What is atomic radius in reality?

In $K^{+} F^{-}$ ionic,the ionic radius of $F^{-}$ is more,while the atomic radius of $K^{+}$ is:

The correct sequence which shows the decreasing order of the ionic radii of the elements is:

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