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Chapter 11: Problem 93

The hybridization scheme for the central atom includes a \(d\) orbital contribution in (a) \(\mathrm{I}_{3}^{-} ;\) (b) \(\mathrm{PCl}_{3}\) (c) \(\mathrm{NO}_{3}^{-} ;\) (d) \(\mathrm{H}_{2}\) Se.

Short Answer

Expert verified
Only \( \mathrm{I}_{3}^{-} \) involves a d orbital in its hybridization scheme.

Step by step solution

01

Identify the Central Atom and Electron Pairs for \( \mathrm{I}_{3}^{-} \)

The central atom for \( \mathrm{I}_{3}^{-} \) is iodine (I), with two other iodine atoms and one lone pair of electrons. This gives it a total of 3 electron pairs.
02

Identify the Central Atom and Electron Pairs for \( \mathrm{PCl}_{3} \)

The central atom for \( \mathrm{PCl}_{3} \) is phosphorus (P), with three other chlorine atoms and one lone pair of electrons. This gives it a total of 4 electron pairs.
03

Identify the Central Atom and Electron Pairs for \( \mathrm{NO}_{3}^{-} \)

The central atom for \( \mathrm{NO}_{3}^{-} \) is nitrogen (N), with three other oxygen atoms. This gives it a total of 3 electron pairs.
04

Identify the Central Atom and Electron Pairs for \( \mathrm{H}_{2} Se \)

The central atom for \( \mathrm{H}_{2} Se \) is selenium (Se), with two hydrogen atoms and two pairs of lone electrons. This gives it a total of 4 electron pairs.
05

Identify Which Molecules Involve a d Orbital

Looking at the total number of electron pairs, the only molecule with more than four electron pairs is \( \mathrm{I}_{3}^{-} \). Therefore, \( \mathrm{I}_{3}^{-} \) involves a d orbital in its hybridization scheme.

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Most popular questions from this chapter

Which of these diatomic molecules do you think has the greater bond energy, \(\mathrm{Li}_{2}\) or \(\mathrm{C}_{2} ?\) Explain.

In your own words, define the following terms or symbols: (a) \(s p^{2} ;\) (b) \(\sigma_{2 p}^{*} ;\) (c) bond order; (d) \(\pi\) bond.

Show that both the valence-bond method and molecular orbital theory provide an explanation for the existence of the covalent molecule \(\mathrm{Na}_{2}\) in the gaseous state. Would you predict \(\mathrm{Na}_{2}\) by the Lewis theory?

The structure of the molecule allene, \(\mathrm{CH}_{2} \mathrm{CCH}_{2}\), is shown here. Propose hybridization schemes for the \(C\) atoms in this molecule.

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