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Chapter 11: Problem 11

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 \(_{5}\)

Short Answer

Expert verified
The hybridizations for the given species are - (a) \(PF_{6}^{-}\) is \(sp^{3}d^{2}\), (b) \(COS\) is \(sp\), (c) \(SiCl_{4}\) is \(sp^{3}\), (d) \(NO_{3}^{-}\) is \(sp^{2}\), (e) \(AsF_{5}\) is \(sp^{3}d\).

Step by step solution

01

PF6-

Look at the central atom (P). The number of atoms bonded to Phosphorus is 6 and there are no lone pairs. This implies an octahedral shape, leading to hybridization of \(sp^{3}d^{2}\).
02

COS

In \(COS\), C is the central atom. It is bonded to two other atoms and there are no lone pairs. This indicates a straight-line structure with bond angles of 180°. This implies \(sp\) hybridization.
03

SiCl4

For \(SiCl_{4}\), the central atom is Si. The number of atoms Si is bonded to is 4 and there are no lone pairs. This corresponds to a Tetrahedral shape and hence the hybridisation is \(sp^{3}\).
04

NO3-

For \(NO_{3}^{-}\), the central atom is N. It is bonded to 3 atoms (oxygen atoms) and there is one resonance bond. This implies a Trigonal Planar shape and hence the hybridisation is \(sp^{2}\).
05

AsF5

Finally, in \(AsF_{5}\), As is the central atom. The number of atoms As is bonded to is 5 and there are no lone pairs. This implies a trigonal Bi-Pyramidal shape and hence the hybridisation is \(sp^{3}d\).

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Most popular questions from this chapter

Think of the reaction shown here as involving the transfer of a fluoride ion from \(\mathrm{ClF}_{3}\) to \(\mathrm{AsF}_{5}\) to form the ions \(\mathrm{ClF}_{2}^{+}\) and \(\mathrm{AsF}_{6}^{-}\). As a result, the hybridization scheme of each central atom must change. For each reactant molecule and product ion, indicate (a) its geometric structure and (b) the hybridization scheme for its central atom. $$ \mathrm{ClF}_{3}+\mathrm{AsF}_{5} \longrightarrow\left(\mathrm{ClF}_{2}^{+}\right)\left(\mathrm{AsF}_{6}^{-}\right) $$

The compound potassium sesquoxide has the empirical formula $\mathrm{K}_{2} \mathrm{O}_{3}$. Show that this compound can be described by an appropriate combination of potassium, peroxide, and superoxide ions. Write a Lewis structure for a formula unit of the compound.

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.

Explain why the molecular structure of \(\mathrm{BF}_{3}\) cannot be adequately described through overlaps involving pure \(s\) and \(p\) orbitals.

The paramagnetism of gaseous \(\mathrm{B}_{2}\) has been established. Explain how this observation confirms that the \(\pi_{2 p}\) orbitals are at a lower energy than the \(\sigma_{2 p}\) orbital for \(\mathrm{B}_{2}\)
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