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Chapter 11: Problem 61

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.

Short Answer

Expert verified
Potassium sesquioxide (\(K_{2}O_{3}\)) can be formed by an appropriate combination of one potassium, one peroxide, and one superoxide ion. The Lewis structure presents two potassium ions (\(K^{+}\)), connected to an oxygen doublet (\(O_{2}^{2-}\)) and an oxygen pair with an additional electron (\(O_{2}^{-}\)).

Step by step solution

01

Understanding different ions

Firstly, it's key to understand the charge and composition of each ion. Potassium ion (\(K^{+}\)), has a charge of +1. Peroxide ion (\(O_{2}^{2-}\)) is composed of 2 oxygen atoms and has a total charge of -2. Likewise, superoxide ion (\(O_{2}^{-}\)) consists of 2 oxygen atoms and has a total charge of -1.
02

Forming the compound

For the compound \(K_{2}O_{3}\) to be neutral, the total charge must be zero. This can be achieved by combining one potassium ion (\(K^{+}\)), one peroxide ion (\(O_{2}^{2-}\)), and one superoxide ion (\(O_{2}^{-}\)). Hence, \(K_{2}O_{3}\) = \(K^{+}\) + \(O_{2}^{2-}\) + \(O_{2}^{-}\). Thus, the compound \(K_{2}O_{3}\) can be described by an appropriate combination of potassium, peroxide, and superoxide ions as required.
03

Drawing the Lewis structure

To draw the Lewis structure, place the potassium ions on the outer side and connect them with oxygen ions inside by lines, which represent shared electrons or ionic bond. For the peroxide ion, draw single bar between the two oxygen atoms indicating the single bond, and then fill in the lone pairs on each oxygen atom. The superoxide ion is drawn similarly. However, it has one extra electron giving it a formal charge of 1-.

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Most popular questions from this chapter

Describe the molecular geometry of \(\mathrm{CCl}_{4}\) suggested by each of the following methods: (a) Lewis theory; (b) valence-bond method using simple atomic orbitals; (c) VSEPR theory; (d) valence-bond method using hybridized atomic orbitals.

Consider the molecules \(\mathrm{NO}^{+}\) and \(\mathrm{N}_{2}^{+}\) and use molecular orbital theory to answer the following: (a) Write the molecular orbital configuration of each ion (ignore the 1 s electrons). (b) Predict the bond order of each ion. (c) Which of these ions is paramagnetic? Which is diamagnetic? (d) Which of these ions do you think has the greater bond length? Explain.

Lewis theory is satisfactory to explain bonding in the ionic compound \(\mathrm{K}_{2} \mathrm{O},\) but it does not readily explain formation of the ionic compounds potassium superoxide, \(\mathrm{KO}_{2}\), and potassium peroxide, \(\mathrm{K}_{2} \mathrm{O}_{2}\) (a) Show that molecular orbital theory can provide this explanation. (b) Write Lewis structures consistent with the molecular orbital explanation.

Is it correct to say that when a diatomic molecule loses an electron, the bond energy always decreases (that is, that the bond is always weakened)? Explain.

Explain why it is necessary to hybridize atomic orbitals when applying the valence-bond method that is, why are there so few molecules that can be described by the overlap of pure atomic orbitals only?
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