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Chapter 10: Problem 57

In which of the following species is it necessary to employ an expanded valence shell to represent the Lewis structure: $\mathrm{PO}_{4}^{3-}, \mathrm{PI}_{3}, \mathrm{ICl}_{3}, \mathrm{OSCl}_{2}, \mathrm{SF}_{4}, \mathrm{ClO}_{4} ?$ Explain your choices.

Short Answer

Expert verified
The species where it is necessary to employ an expanded valence shell to represent the Lewis structure are \(PO_{4}^{3-}\), \(PI_{3}\), \(ICl_{3}\), \(SF_{4}\), and \(ClO_{4}\)

Step by step solution

01

Labeling Central Atoms

The first step deals with identifying the central atom in the species \(PO_{4}^{3-}\), \(PI_{3}\), \(ICl_{3}\), \(OSCl_{2}\), \(SF_{4}\), \(ClO_{4}\). These are P, P, I, O, S and Cl, respectively.
02

Determining Valence Electrons

Next, determine the number of valence electrons for each central atom. Phosphorus has 5 valence electrons, Iodine has 7, Oxygen has 6, Sulfur has 6, and Chlorine has 7.
03

Establishing Bonds and Lone Pairs

Now, establish how many bonds each atom tends to form and whether it typically carries any lone pairs of electrons. Phosphorus in \(PO_{4}^{3-}\) forms 4 bonds and carries no lone pairs, Phosphorus in \(PI_{3}\) forms 3 bonds and has one lone pair, Iodine in \(ICl_{3}\) forms 3 bonds and has two lone pairs, Oxygen in \(OSCl_{2}\) forms 2 bonds and carries two lone pairs, Sulfur in \(SF_{4}\) forms 4 bonds and has one lone pair, and Chlorine in \(ClO_{4}\) forms 4 bonds and carries no lone pairs.
04

Understanding Expanded Valence Shells

Atoms in the second period (n=2) of the periodic table, such as carbon, nitrogen, and oxygen, cannot have more than four groups around them because they only have four orbitals in which to place their valence electrons. Phosphorus, sulfur, and chlorine atoms can hold more than eight electrons when they form hypervalent compounds. These include elements such as sulfur, phosphorus, silicon, and chlorine, which can expand their valence shell to include the 3d orbitals.
05

Determining Expanded Valance Shells

All the central atoms, except Oxygen in \(OSCl_{2}\), have more than 8 electrons around them in the given molecular species, exhibiting an expanded valence shell. Therefore, the species requiring the use of an expanded valence shell to represent their Lewis structures are \(PO_{4}^{3-}\), \(PI_{3}\), \(ICl_{3}\), \(SF_{4}\), and \(ClO_{4}\).

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Most popular questions from this chapter

Predict the shapes of the following molecules, and then predict which would have resultant dipolemoments: (a) \(\mathrm{SO}_{2} ;\) (b) \(\mathrm{NH}_{3} ;\) (c) \(\mathrm{H}_{2} \mathrm{S} ;\) (d) \(\mathrm{C}_{2} \mathrm{H}_{4} ;\) (e) \(\mathrm{SF}_{6}\); (f) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\).

What is the percent ionic character of each of the following bonds: (a) \(\mathrm{S}-\mathrm{H} ;\) (b) \(\mathrm{O}-\mathrm{Cl} ;\) (c) \(\mathrm{Al}-\mathrm{O}\) (d) As - O?

Estimate the lengths of the following bonds and indicate whether your estimate is likely to be too high or too low: (a) I \(-\mathrm{Cl} ;\) (b) \(\mathrm{C}-\mathrm{F}\).

Explain why it is not necessary to find the Lewis structure with the smallest formal charges to make a successful prediction of molecular geometry in the VSEPR theory. For example, write Lewis structures for \(S O_{2}\) having different formal charges, and predict the molecular geometry based on these structures.

Acetone \(\left(\mathrm{CH}_{3}\right) \mathrm{C}=\mathrm{O},\) a ketone, will react with a strong base \((\mathrm{A})\) to produce the enolate anion, \(\mathrm{CH}_{3}(\mathrm{C}=\mathrm{O}) \mathrm{CH}_{2}^{-} .\) Draw the Lewis structure of the enolate anion, and describe the relative contributions of any resonance structures.
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