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Chapter 10: Problem 88

In which of the following molecules would you expect the oxygen-to-oxygen bond to be the shortest: (a) \(\mathrm{H}_{2} \mathrm{O}_{2},\) (b) \(\mathrm{O}_{2},\) (c) \(\mathrm{O}_{3} ?\) Explain.

Short Answer

Expert verified
The shortest oxygen-to-oxygen bond should be in \(\mathrm{O}_{2}\) because it has the highest bond order (2), which means it has the strongest bond and thus the shortest bond length.

Step by step solution

01

Understand the Molecules

First, we need to understand the structure of the given molecules. Hydrogen peroxide (\(\mathrm{H}_{2} \mathrm{O}_{2}\)) is a simple molecule where each oxygen is single-bonded to another oxygen and two hydrogen atoms. Dioxygen (\(\mathrm{O}_{2}\)) is a molecule in which two oxygen atoms are double-bonded to each other. Ozone (\(\mathrm{O}_{3}\)) is a polyatomic molecule in which one oxygen atom is double-bonded to a second oxygen atom, which is in turn single-bonded to a third oxygen atom.
02

Determine Bond Order

Now we need to determine the bond order of the oxygen-to-oxygen bonds in each molecule. In hydrogen peroxide, there is a single bond between the oxygen atoms, so the bond order is 1. In dioxygen, there is a double bond, so the bond order is 2. In ozone, there are 1.5 bonds on average between each pair of oxygen atoms (one double bond and one single bond shared among three atoms), so the bond order is 1.5.
03

Determine Bond Length

We know that bond length decreases as bond order increases. Therefore, we should expect the shortest oxygen-oxygen bond to occur in the molecule with the highest oxygen-oxygen bond order. This is dioxygen (\(\mathrm{O}_{2}\)) with the bond order of 2, so the bond in \(\mathrm{O}_{2}\) would be expected to be the shortest.

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Most popular questions from this chapter

Write plausible Lewis structures for the following odd-electron species: (a) \(\mathrm{CH}_{3} ;\) (b) \(\mathrm{ClO}_{2} ;\) (c) \(\mathrm{NO}_{3}\).

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In your own words, define the following terms: (a) valence electrons; (b) electronegativity; (c) bonddissociation energy; (d) double covalent bond;(e) coordinate covalent bond.

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The species \(\mathrm{PBr}_{4}^{-}\) has been synthesized and has been described as a tetrahedral anion. Comment on this description.
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