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

Which among the following isoelectronic species has the smallest size?
$O^{2-}, F^{-}, Ne, Na^{+}, Mg^{2+}, Al^{3+}, Si^{4+}$

$A$ trend common to both groups $I$ and $VII$ elements in the periodic table as atomic number increases is

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

Which of the following orders of atomic radius is correct?

The ionic radii of $F^{-}$ and $O^{2-}$ respectively are $1.33 \ \mathring{A}$ and $1.40 \ \mathring{A}$,while the covalent radius of $N$ is $0.74 \ \mathring{A}$. The correct statement for the ionic radius of $N^{3-}$ from the following is: