NCERT Solution
Class 11
Chemistry
Classification of Elements and Periodicity in Properties
the size of isoelectronic species mdash f ndash...

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:

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^-

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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.

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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.

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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.