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Chapter 11: Problem 91

A molecule in which \(s p^{2}\) hybrid orbitals are used by the central atom in forming covalent bonds is (a) \(\mathrm{PCl}_{5}\) (b) \(\mathrm{N}_{2} ;\) (c) \(\mathrm{SO}_{2} ;\) (d) \(\mathrm{He}_{2}\)

Short Answer

Expert verified
The molecule in which \(sp^{2}\) hybrid orbitals are used by the central atom in forming covalent bonds is \(\mathrm{SO}_{2}\).

Step by step solution

01

Structure of PCl5

The central atom in \(\mathrm{PCl}_{5}\) is Phosphorus (P). It has 5 valence electrons, and it forms 5 sigma bonds with 5 Chlorine (Cl) atoms. There are no lone pairs on Phosphorus. So, the hybridization is \(sp^{3}d\), not \(sp^{2}\).
02

Structure of N2

The molecule \(\mathrm{N}_{2}\) is composed of two Nitrogen (N) atoms. Each Nitrogen atom forms one sigma bond with the other Nitrogen atom and two pi bonds. So, no \(sp^{2}\) hybridization here. The hybridization is \(sp\).
03

Structure of SO2

The central atom in \(\mathrm{SO}_{2}\) is Sulphur (S). It forms two sigma bonds with two Oxygen (O) atoms and has one lone pair. Hence, it's hybridization is \(sp^{2}\). Therefore, \(\mathrm{SO}_{2}\) is the molecule in which \(sp^{2}\) hybrid orbitals are used by the central atom in forming covalent bonds.
04

Structure of He2

The molecule \(\mathrm{He}_{2}\) does not exist because Helium (He) is a noble gas and it does not form covalent bonds with other atoms. So, it doesn't undergo hybridization.

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Most popular questions from this chapter

Delocalized molecular orbitals are found in (a) \(\mathrm{H}_{2}\) (b) \(\mathrm{HS}^{-} ;\) (c) \(\mathrm{CH}_{4} ;\) (d) \(\mathrm{CO}_{3}^{2-}\) .

Match each of the following species with one of these hybridization schemes: \(s p, s p^{2}, s p^{3}, s p^{3} d, s p^{3} d^{2} .\) (a) \(\mathrm{PF}_{6}^{-}\) (b) \(\operatorname{COS} ;\) (c) \(\operatorname{SiCl}_{4} ;\) (d) \(\mathrm{NO}_{3}^{-}\);(e) AsF \(_{5}\)

Why does the hybridization \(s p^{3} d\) not account for bonding in the molecule BrF \(_{5} ?\) What hybridization scheme does work? Explain.

Draw a Lewis structure(s) for the nitrite ion, \(\mathrm{NO}_{2}^{-}\) Then propose a bonding scheme to describe the \(\sigma\) and the bonding in this ion. What conclusion can you reach about the number and types of \(\pi\) molecular orbitals in this ion? Explain.

Represent bonding in the carbon dioxide molecule, \(\mathrm{CO}_{2},\) by \((\mathrm{a})\) a Lewis structure and \((\mathrm{b})\) the valencebond method. Identify \(\sigma\) and \(\pi\) bonds, the necessary hybridization scheme, and orbital overlap.
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