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.

Question

Philoid · Accepted Answer

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^-(Z=9) < Ne(Z=10) < Na⁺(Z=11)

Therefore, the order of the increasing size of F^-, Ne and Na⁺ is as follows:

Na⁺ < Ne < F^-

Hence, the correct option is - (a) nuclear charge (Z).

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.

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.