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Chapter 10: Problem 85

Without referring to tables in the text, indicate which of the following bonds you would expect to have the greatest bond length, and give your reasons. (a) \(\mathrm{O}_{2}\); (b) \(\mathrm{N}_{2} ;\) (c) \(\mathrm{Br}_{2} ;\) (d) \(\mathrm{BrCl}\).

Short Answer

Expert verified
Among \(\mathrm{O}_{2}\), \(\mathrm{N}_{2}\), \(\mathrm{Br}_{2}\) and \(\mathrm{BrCl}\), the \(\mathrm{BrCl}\) bond is expected to have the greatest length. This is due to it being composed of larger atoms (compared to O and N) and it being a single bond (longer than double or triple bonds).

Step by step solution

01

Understand Elements' Properties

To start with, recognize the periodic table properties of the elements involved. Oxygen (O) and Nitrogen (N) are Period 2 elements, while Bromine (Br) and Chlorine (Cl) are Period 4 and 3 elements respectively. This means Bromine and Chlorine are larger than Oxygen and Nitrogen.
02

Determine Bond Types

Next, identify the type of bond present in the given molecules. In \(\mathrm{O}_{2}\) and \(\mathrm{N}_{2}\), they are double and triple bonds respectively while in \(\mathrm{Br}_{2}\) and \(\mathrm{BrCl}\), they are single bonds. Single bonds are generally longer than double and triple bonds.
03

Compare Bond lengths

Now compare the bond lengths based on the above information. Given that single bonds are typically longer and Period 4/3 elements are larger, it can be expected that \(\mathrm{BrCl}\) and \(\mathrm{Br}_{2}\) will have greater bond lengths than \(\mathrm{O}_{2}\) and \(\mathrm{N}_{2}\). Between \(\mathrm{BrCl}\) and \(\mathrm{Br}_{2}\), \(\mathrm{BrCl}\) is likely to have a slightly longer bond because mixing different elements often increases bond length.

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Most popular questions from this chapter

Write a plausible Lewis structure for \(\mathrm{C}_{3} \mathrm{O}_{2},\) a substance known as carbon suboxide.

Levulinic acid has the formula $\mathrm{CH}_{3}(\mathrm{CO}) \mathrm{CH}_{2} \mathrm{CH}_{2}$ COOH. Sketch the levulinic acid molecule, and indicate the various bond angles.

Sketch the probable geometric shape of a molecule of (a) \(\mathrm{N}_{2} \mathrm{O}_{4}\left(\mathrm{O}_{2} \mathrm{NNO}_{2}\right) ;\) (b) \(\mathrm{C}_{2} \mathrm{N}_{2}(\mathrm{NCCN}) ;\) (c) \(\mathrm{C}_{2} \mathrm{H}_{6}\) \(\left(\mathrm{H}_{3} \mathrm{CCH}_{3}\right) ;(\mathrm{d}) \mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\left(\mathrm{H}_{3} \mathrm{COCH}_{3}\right)\).

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.]

Write Lewis symbols for the following atoms. (a) \(\mathrm{Kr}\); (b) Ge; (c) \(\mathrm{N} ;\) (d) Ga; (e) As; (f) Rb.
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