Which of the following is the correct representation of $O_{2}$ ?

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Solution

The correct option is A

The electronic configuration of oxygen is 2,6. Oxygen has 6 electrons in its outermost shell. So, each of the two ‘O’ atoms contributes two electrons so as to have two shared pairs of electrons between them. Both atoms attain octet structure which results in the formation of a double covalent bond [O=O] between them.

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Similar questions

C

O

C O_{2} (: ¨ O = C = ¨ O :)

C a O

C a : [A r] 4 s^{2} ⟶ C a^{2 +} [A r] O : 1 s^{2} 2 s^{2} 2 p^{4} ⟶ O^{2 -} 1 s^{2} 2 s^{2} 2 p^{6} C a^{2 +} [: ¨ O \cdot \cdot :]^{2 -}

{[: ¨ O = N = ¨ O :]}^{+}

N

O

Question 20

Which of the following options represents the correct bond order?

(a) $O_{2}^{-} > O_{2} > O_{2}^{+}$

(b) $O_{2}^{-} < O_{2} < O_{2}^{+}$

(d) $O_{2}^{-} < O_{2} > O_{2}^{+}$

[: ¨ O = N = ¨ O :]^{+}

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