Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 8: Problem 55

Compare the \(\mathrm{O}-\mathrm{O}\) bond length in \(\mathrm{O}_{2}\) versus \(\mathrm{H}_{2} \mathrm{O}_{2}\). Which bond is shorter? Why?

Short Answer

Expert verified
The O-O bond length in \(O_2\) is shorter than in \(H_2O_2\) because of the stronger double bond in \(O_2\), which results from a greater number of shared electrons between the oxygen atoms. This stronger bonding leads to a shorter bond length as the oxygen atoms are pulled closer together.

Step by step solution

01

Identify the molecular structures for O₂ and H₂O₂

Both O₂ and H₂O₂ contain an O-O bond. Let's first understand the molecular structure for both molecules. \(O_2\) is a diatomic molecule consisting solely of two oxygen atoms bonded together. The O-O bond in O₂ can be represented in Lewis structures as a double bond: O = O \(H_2O_2\) (hydrogen peroxide) is a molecule consisting of two oxygen atoms and two hydrogen atoms. It has the following molecular structure: H - O - O - H It is essential to notice that in this molecule, the O-O bond is a single bond.
02

Understand the electronic configuration and bonding in oxygen atoms

The electronic configuration of each oxygen atom is: 1s² 2s² 2p⁴ This means that each oxygen atom has six valence electrons - two in the 2s orbital and four in the 2p orbitals. In O₂, two oxygen atoms form a double bond, which means they share four electrons between them. This contributes to a stronger and shorter bond. In H₂O₂, the two oxygen atoms are connected via a single bond, sharing only two electrons, which results in a weaker and longer bond.
03

Compare the bond length in O₂ and H₂O₂

Now that we understand the electronic configuration and bonding in oxygen atoms for both molecules, we can conclude which bond is shorter. The O-O double bond in O₂ is stronger than the O-O single bond in H₂O₂ because more electrons are shared between the two oxygen atoms in O₂. Due to this strong connection and the higher number of shared electrons, the double bond in O₂ will be shorter as the atoms are pulled closer together due to stronger electrostatic forces between the oxygen atoms.
04

Conclusion

In conclusion, the O-O bond length in O₂ is shorter than the O-O bond length in H₂O₂ due to the greater number of shared electrons and stronger bonding in the O₂ molecule.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

(a) Construct a Lewis structure for hydrogen peroxide, $\mathrm{H}_{2} \mathrm{O}_{2}$, in which each atom achieves an octet of electrons. (b) How many bonding electrons are between the two oxygen atoms? (c) Do you expect the \(\mathrm{O}-\mathrm{O}\) bond in \(\mathrm{H}_{2} \mathrm{O}_{2}\) to be longer or shorter than the \(\mathrm{O}-\mathrm{O}\) bond in \(\mathrm{O}_{2} ?\) Explain.

For Group 13-17 elements in the third row of the periodic table and beyond, the octet rule is often not obeyed. A friend of yours says this is because these heavier elements are more likely to make double or triple bonds. Another friend of yours says that this is because the heavier elements are larger and can make bonds to more than four atoms at a time. Which friend is more correct?

Consider the lattice energies of the following Group \(2 \mathrm{~A}\) compounds: $\mathrm{BeH}_{2}, 3205 \mathrm{~kJ} / \mathrm{mol} ; \mathrm{MgH}_{2}, 2791 \mathrm{~kJ} / \mathrm{mol} ;\( \)\mathrm{CaH}_{2}, 2410 \mathrm{~kJ} / \mathrm{mol} ; \mathrm{SrH}_{2}, 2250 \mathrm{~kJ} / \mathrm{mol} ; \mathrm{BaH}_{2}, 2121 \mathrm{~kJ} / \mathrm{mol}$ (a) What is the oxidation number of H in these compounds? (b) Assuming that all of these compounds have the same three-dimensional arrangement of ions in the solid, which of these compounds has the shortest cation-anion distance? (c) Consider BeH \(_{2}\). Does it require \(3205 \mathrm{~kJ}\) of energy to break one mole of the solid into its ions, or does breaking up one mole of solid into its ions release \(3205 \mathrm{~kJ}\) of energy? (d) The lattice energy of \(\mathrm{ZnH}_{2}\) is \(2870 \mathrm{~kJ} / \mathrm{mol}\). Considering the trend in lattice enthalpies in the Group 2 compounds, predict which Group 2 element is most similar in ionic radius to the \(\mathrm{Zn}^{2+}\) ion.

Draw the Lewis structures for each of the following ions or molecules. Identify those in which the octet rule is not obeyed; state which atom in each compound does not follow the octet rule; and state, for those atoms, how many electrons surround them: $(\mathbf{a}) \mathrm{HCl},(\mathbf{b}) \mathrm{ICl}_{5},\( (c) \)\mathrm{NO}\( (d) \)\mathrm{CF}_{2} \mathrm{Cl}_{2},(\mathbf{e}) \mathrm{I}_{3}^{-}$

Which of the following trends in lattice energy is due to differences in ionic radii? (a) $\mathrm{LiF}>\mathrm{NaF}>\mathrm{CsF},(\mathbf{b}) \mathrm{CaO}>\mathrm{KCl}\( (c) \)\mathrm{PbS}>\mathrm{Li}_{2} \mathrm{O}$
See all solutions

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Read Explanation

Kinetics

Read Explanation

Chemical Analysis

Read Explanation

The Earths Atmosphere

Read Explanation

Inorganic Chemistry

Read Explanation

Organic Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free