Question

The size of isoelectronic species - $F^{-}$, Ne and $Na^{+}$ is affected by: (a) nuclear charge (Z) (b) valence principal quantum number (n) (c) electron–electron interaction in the outer orbitals (d) none of the factors because their size is the same

Answer 1

Isoelectronic species are the species belonging to different atoms or ions which have same number of electrons but different magnitudes of nuclear charges.
The size of an isoelectronic species increases with a decrease in the nuclear charge ( Z ). For example, the order of the increasing nuclear charge of F – , Ne, and Na + is as follows:
F – < Ne < Na +
Z 9 10 11
Therefore, the order of the increasing size of F – , Ne and Na + is as follows:
Na + < Ne < F

Answer 2

"Isoelectronic species are “different atoms” or “ions” with the “same number” of “electrons” but “different magnitudes” of “nuclear charges”.

The “size” of an “isoelectronic species increases” as the “nuclear charge (Z) decreases”.

For example, the “order” of the “increasing nuclear charge” of ${ F }^{ - }$, Ne and ${ Na }^{ + }$is as follows.

${ F }^{ - }\quad <\quad Ne\quad <\quad N{ a }^{ + }$

Therefore, the order of the increasing size of ${ F }^{ - }, Ne, and { Na }^{ + }$is as follows.

$N{ a }^{ + }\quad <\quad Ne\quad <\quad { F }^{ - }$"