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Chapter 9: Problem 118

The \(\mathrm{N}-\mathrm{O}\) bond distance in nitric oxide is \(115 \mathrm{pm}\) which is intermediate between a triple bond (106 pm) and a double bond (120 pm). (a) Draw two resonance structures for \(\mathrm{NO}\) and comment on their relative importance. (b) Is it possible to draw a resonance structure having a triple bond between the atoms?

Short Answer

Expert verified
Yes, it is possible to draw resonance structures for Nitric Oxide, one with a double bond and one with a triple bond between the Nitrogen and Oxygen atoms. However, the structure with a triple bond, though possible, is less important due to the charge separation and its discordance with the given bond length.

Step by step solution

01

Draw Resonance Structures

To begin, let's draw two resonance structures for nitric oxide. The nitrogen atom can either form a double bond or a triple bond with the oxygen atom because nitrogen has five valence electrons while oxygen has six. Therefore, in the first resonance structure, nitrogen forms a double bond with oxygen and also has a lone pair, while oxygen has two lone pairs. In the second resonance structure, nitrogen and oxygen form a triple bond and nitrogen has a lone pair while oxygen has only one lone pair.
02

Comment On Importance Of Resonance Structures

After drawing the resonance structures, let's comment on their relative importance. Resonance structures portray a molecule's electronic structure more accurately because they show all possible arrangements of electrons. However, the second resonance structure with a triple bond is less important because it leads to charge separation and it follows from the principle that structures with minimum charges are more stable. Moreover, given the bond distance, the actual structure is likely to lean more towards the double bond since its length is nearer to the given value (120 pm).
03

Consider Triple Bond Resonance Structure

Now let's consider if we can draw a resonance structure with a triple bond between the atoms. Though the triple bond structure is possible, it is less important as explained earlier because it leads to charge separation and structures with minimum charges are more stable. Furthermore, the bond length for a triple bond structure is shorter (106 pm) in comparison to the actual bond length of NO. Hence, the triple bond structure is not in alignment with the given properties.

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Most popular questions from this chapter

Describe some characteristics of an ionic compound such as \(\mathrm{KF}\) that would distinguish it from a covalent compound such as benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\).

Use Lewis dot symbols to show the transfer of electrons between the following atoms to form cations and anions: (a) \(\mathrm{Na}\) and \(\mathrm{F},(\mathrm{b}) \mathrm{K}\) and \(\mathrm{S},\) (c) \(\mathrm{Ba}\) and \(\mathrm{O},\) (d) Al and N.

The chlorine nitrate molecule (ClONO \(_{2}\) ) is believed to be involved in the destruction of ozone in the Antarctic stratosphere. Draw a plausible Lewis structure for this molecule.

A new allotrope of oxygen, \(\mathrm{O}_{4}\), has been reported. The exact structure of \(\mathrm{O}_{4}\) is unknown, but the \(\operatorname{sim}-\) plest possible structure would be a four-member ring consisting of oxygen-oxygen single bonds. The report speculated that the \(\mathrm{O}_{4}\) molecule might be useful as a fuel "because it packs a lot of oxygen in a small space, so it might be even more energy-dense than the liquefied ordinary oxygen used in rocket fuel." (a) Draw a Lewis structure for \(\mathrm{O}_{4}\) and write a balanced chemical equation for the reaction between ethane, \(\mathrm{C}_{2} \mathrm{H}_{6}(g),\) and \(\mathrm{O}_{4}(g)\) to give carbon dioxide and water vapor. (b) Estimate \(\Delta H^{\circ}\) for the reaction. (c) Write a chemical equation illustrating the standard enthalpy of formation of \(\mathrm{O}_{4}(g)\) and estimate \(\Delta H_{\mathrm{f}}^{\circ}\) (d) Assuming the oxygen allotropes are in excess, which will release more energy when reacted with ethane (or any other fuel): \(\mathrm{O}_{2}(g)\) or \(\mathrm{O}_{4}(g) ?\) Explain using your answers to parts (a)-(c).

Explain how the lattice energy of an ionic compound such as \(\mathrm{KCl}\) can be determined using the Born-Haber cycle. On what law is this procedure based?
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