Question

Which of the following species have the same shape?

(i) \[\ce{CO2}\]

(ii) \[\ce{CCl4}\]

(iii) \[\ce{O3}\]

(iv) \[\ce{NO^{-}3}\]

Answer 1

(iii) \[\ce{O3}\]

(iv) \[\ce{NO^{-}3}\]

Explanation:

(i) The number of valence electrons in \[\ce{CO2}\] is 14. The oxygen atom attached to the carbon atom forms a double bond. Therefore, the hybridization of the structure is sp². Thus, carbon dioxide is linear in shape.

(ii) The number of valence electrons in \[\ce{CCl4}\] is 32. The structure of \[\ce{CCl4}\] is arranged in a tetrahedral manner. The chlorine atoms are arranged such that the hybridization is sp³.

(iii) The number of valence electrons in \[\ce{O3}\] is 24. The hybridization of the molecule is sp² and due to the presence of lone pair of electrons on the central oxygen atom and due to the effect of resonance, ozone molecule has a bent shape.

(iv) The number of valence electrons in \[\ce{NO^{-}2}\] is 24. The hybridization of the molecule is sp² and due to the presence of lone pair on the nitrogen atom it attains a bent shape.