The electron affinity value are negative for

A. $$\mathrm{Be} \rightarrow \mathrm{Be}^{-}$$

B. $$\mathrm{N} \rightarrow \mathrm{N}^{-}$$

C. $$\mathrm{O} \rightarrow \mathrm{O}^{2-}$$

D. $$\mathrm{Na} \rightarrow \mathrm{Na}^{-}$$

E. $$\mathrm{Al} \rightarrow \mathrm{Al}^{-}$$

Choose the most appropriate answer from the options given below :

Given below are two statements :

Statement I : The metallic radius of $$\mathrm{Na}$$ is $$1.86 \mathrm{~A}^{\circ}$$ and the ionic radius of $$\mathrm{Na}^{+}$$ is lesser than $$1.86 \mathrm{~A}^{\circ}$$

Statement II : Ions are always smaller in size than the corresponding elements.

In the light of the above statements, choose the correct answer from the options given below :

Given below are two statements:

Statement I: In group 13, the stability of +1 oxidation state increases down the group.

Statement II : The atomic size of gallium is greater than that of aluminium.

In the light of the above statements, choose the most appropriate answer from the options given below :

The statement(s) that are correct about the species $$\mathrm{O}^{2-}, \mathrm{F}^{-}, \mathrm{Na}^{+}$$ and $$\mathrm{Mg}^{2+}$$.

(A) All are isoelectronic

(B) All have the same nuclear charge

(C) $$\mathrm{O}^{2-}$$ has the largest ionic radii

(D) $$\mathrm{Mg}^{2+}$$ has the smallest ionic radii

Choose the most appropriate answer from the options given below :