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Chapter 5: Problem 91

Experiments show that it takes more energy to break the bond between oxygen atoms in the \(\mathrm{O}_{2}\) molecule than in the \(\mathrm{O}_{3}\) molecule. How can you explain this?

Short Answer

Expert verified
The energy difference in breaking bonds between oxygen atoms in O2 and O3 molecules can be explained by comparing their molecular structures. In O2, a double covalent bond results in a stronger and shorter bond compared to the single bonds in O3. This double bond involves the sharing of four electrons, making it harder to break. Thus, more energy is required to break the bond between oxygen atoms in O2 than in O3.

Step by step solution

01

Understand molecular structure of O2 and O3

To explain the difference in bond energies, we first need to understand the structure of O2 and O3 molecules. In the O2 molecule, there are two oxygen atoms connected by a double covalent bond. In contrast, in the O3 molecule, three oxygen atoms are connected with single covalent bonds in a bent structure resembling a V-shape.
02

Examine bond strength and lengths

In general, double bonds are stronger than single bonds because they involve the sharing of more electrons between the two atoms. In O2, the double bond between the two oxygen atoms is shorter and stronger than the single bonds between oxygen atoms in O3. This strength difference is because double bonds involve the sharing of four electrons between the two atoms (two in the sigma bond and two in the pi bond), while single bonds share only two electrons (in the sigma bond).
03

Compare the energy required to break bonds

Since double bonds are stronger and shorter than single bonds, it takes more energy to overcome the forces holding the atoms together in O2 than in O3. Hence, it requires more energy to break the bond between oxygen atoms in O2 than in O3.
04

Conclusion

The difference in the energy required to break the bond between oxygen atoms in O2 and O3 molecules can be explained by comparing their molecular structures. Due to the presence of a double bond in O2, the bond is stronger and shorter than the single bonds present in O3. This results in a higher energy requirement to break the bond in O2 compared to that in O3.

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Most popular questions from this chapter

What is a shortcut rule for determining the number of covalent bonds a representative element from group IVA, VA, VIA, VIIA, or VIIIA can form?

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