1. Interpret the options

The option text is clearly garbled, but from the topic and the visible ionic species, option A appears to represent the common isoelectronic set:

$Mg^{2+},\ Na^+,\ F^-,\ N^{3-}$

This is a standard periodicity question asking for the increasing order of ionic radii.

2. Use the isoelectronic principle

All these ions have 10 electrons:

• $Mg^{2+}$: $12 - 2 = 10$
• $Na^+$: $11 - 1 = 10$
• $F^-$: $9 + 1 = 10$
• $N^{3-}$: $7 + 3 = 10$

So they are isoelectronic.

For an isoelectronic series, ionic radius decreases as nuclear charge increases.

Their nuclear charges are:

• $Mg^{2+}$: $Z=12$
• $Na^+$: $Z=11$
• $F^-$: $Z=9$
• $N^{3-}$: $Z=7$

Thus, the smallest ion is the one with highest $Z$, and the largest is the one with lowest $Z$.

So the order of increasing ionic radii is:

$Mg^{2+} < Na^+ < F^- < N^{3-}$

3. Match with the options

This sequence corresponds to Option A.

4. Final answer

The correct increasing order is:

$Mg^{2+} < Na^+ < F^- < N^{3-}$

Hence, Option A is correct.