Which of the following sets has the atoms and/or ions in correct order of increasing size?

N e < F^{-} < O^{2 -}

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B r^{-} < C l^{-} < F^{-}

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N a^{+} < M g^{2 +} < A l^{3 +}

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P < S < C l

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Solution

The correct option is B $N e < F^{-} < O^{2 -}$
$N e < F^{-} < O^{2 -}$ have the atoms and/or ions in correct order of increasing size.
All these species are isoelectronic with 10 electrons. Anion with greater negative charge will have larger ionic radius. The net repulsion of the electrons will outweigh the nuclear charge and the ion will expand in size.

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Similar questions

i) N e i i) O^{2 -} i i i) M g^{2 +} i v) F

v) A l^{3 +} v i) C l^{-} v i i) K v i i i) N a

Arrange the following in increasing order of the atomic sizes and give reasons

Na⁺ , Mg²⁺ , Al³⁺ , F^- , O^2- , C^4-

I

A l > S i > P > C l

I I

B e < M g < C a < S r

I I I

I < B r < C l < F

I V

{N a}^{+} < {M g}^{2 +} < {A l}^{3 +} < {S i}^{4 +}

In which of the following option the order of arrangement does not agree with the variation of property indicated against it

a) Li<Na<K<Rb(increasing metallic radius)

b) B<C<N<O(increasing 1st ionisation enthalpy)

c)I<Br<Cl<F(increasing electron gain enthalpy)

d) Al³⁺<Mg²⁺<Na⁺<F^-(increasing ionic size)

F^{-}, O^{2 -}, N a^{+}, M g^{2 +}

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