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Chapter 10: Problem 139

The greatest bond length is found in (a) \(\mathrm{O}_{2} ;\) (b) \(\mathrm{N}_{2}\) (c) \(\mathrm{Br}_{2} ;\) (d) BrCl.

Short Answer

Expert verified
The compound with the greatest bond length is BrCl.

Step by step solution

01

Identifying atomic sizes

The first step involves identifying which atoms are larger. Oxygen, Nitrogen and Bromine. Bromine being in the 4th period of the periodic table is larger than Nitrogen and Oxygen which are in the 2nd period of the periodic table.
02

Identify nature of bond

Next, look at the nature of the bonds in the compounds. \(\mathrm{O}_{2}\) and \(\mathrm{N}_{2}\) both have double and triple bonds respectively making them shorter. \(\mathrm{Br}_{2}\) has a single bond and BrCl involves two different larger atoms, possibly leading to a longer bond length.
03

Compare and conclude

Comparing the bond lengths, the single bond between two larger bromine atoms in \(\mathrm{Br}_{2}\) and between bromine and chlorine in BrCl would be generally longer than the double bond in \(\mathrm{O}_{2}\) and the triple bond in \(\mathrm{N}_{2}\). However, between \(\mathrm{Br}_{2}\) and BrCl, the bond length of BrCl would likely be larger as bond lengths tend to increase with the increase in atomic size difference. Hence, BrCl has the greatest bond length among the given compounds.

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Most popular questions from this chapter

One reaction involved in the sequence of reactions leading to the destruction of ozone is $$\mathrm{NO}_{2}(\mathrm{g})+\mathrm{O}(\mathrm{g}) \longrightarrow \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})$$ Calculate \(\Delta H^{\circ}\) for this reaction by using the thermodynamic data in Appendix D. Use your \(\Delta H^{\circ}\) value, plus data from Table \(10.3,\) to estimate the nitrogenoxygen bond energy in \(\mathrm{NO}_{2}\). [Hint: The structure of nitrogen dioxide, \(\mathrm{NO}_{2}\), is best represented as a resonance hybrid of two equivalent Lewis structures.]

What is the formal charge of the indicated atom in each of the following structures? (a) the central \(\mathrm{O}\) atom in \(\mathrm{O}_{3}\) (b) \(\mathrm{Al}\) in \(\mathrm{AlH}_{4}^{-}\) (c) \(\mathrm{Cl}\) in \(\mathrm{ClO}_{3}^{-}\) (d) \(\sin \sin ^{2} \theta^{-}\) (e) \(\mathrm{Cl}\) in \(\mathrm{Cl} \mathrm{F}_{3}\)

If you have four electron pairs around a central atom, under what circumstances can you have a pyramidal molecule? Similarly, how can you have a bent molecule? What are the expected bond angles in each case?

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

Sketch the propyne molecule, \(\mathrm{CH}_{3} \mathrm{C} \equiv \mathrm{CH}\). Indicate the bond angles in this molecule. What is the maximum number of atoms that can be in the same plane?
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