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Chapter 22: Problem 97

Peroxonitrous acid is an unstable intermediate formed in the oxidation of \(\mathrm{HNO}_{2}\) by \(\mathrm{H}_{2} \mathrm{O}_{2}\). It has the same formula as nitric acid, HNO \(_{3}\). Show how you would expect peroxonitrous and nitric acids to differ in structure.

Short Answer

Expert verified
Nitric acid (HNO3) shows a planar structure, with the N atom in the center, attached to an OH group and two O atoms, with equal bond length, predominantly due to resonance structure. Alternatively, peroxonitrous acid, formed in the oxidation of HNO2 by H2O2, gives a structure where the N atom is connected to one O atom and an O-O group, thus incorporating peroxide in its structure.

Step by step solution

01

Structure of Nitric Acid

First, consider the structure of HNO3 (nitric acid). It forms a planar structure with an N atom at the center attached to an OH group and to two O atoms. The molecule has resonance structures which means the double bond can swap places between the two O atoms and the bond lengths are the same, revealing the equal sharing of electrons.
02

Structure of Peroxonitrous Acid

Next, consider the structure of peroxonitrous acid. In the oxidation of HNO2 by H2O2, the HNO2 gives up an H+ ion, resulting in a nitrite ion (\(NO_{2}^{-}\)). Meanwhile, H2O2 can form O-O with its O atoms, leading to a peroxide (\(O_{2}^{2-}\)) ion. During the reaction, the nitrite ion and the peroxide ion combine, making the N atom to be as above, attached to one O atom and to an O-O group. This results in the formation of peroxonitrous acid.

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Most popular questions from this chapter

Use Lewis structures and other information to explain the observation that (a) the oxygen-to-oxygen bond lengths in \(\mathrm{O}_{2}, \mathrm{O}_{3}\) and \(\mathrm{H}_{2} \mathrm{O}_{2}\) are \(121,128,\) and \(148 \mathrm{pm},\) respectively. (b) the oxygen-to-oxygen bond length of \(\mathrm{O}_{2}\) is \(121 \mathrm{pm}\) and for \(\mathrm{O}_{2}^{+}\) is \(112 \mathrm{pm}\). Why is the bond length for \(\mathrm{O}_{2}^{+}\) so much shorter than for \(\mathrm{O}_{2} ?\)

Fluorine can be prepared by the reaction of hexafluoromanganate(IV) ion, MnF \(_{6}^{2-}\), with antimony pentafluoride to produce manganese(IV) fluoride and \(\mathrm{SbF}_{6}^{-}\) followed by the disproportionation of manganese(IV) fluoride to manganese(III) fluoride and \(\mathrm{F}_{2}(\mathrm{g}) .\) Write chemical equations for these two reactions.

Show by calculation whether the reaction $2 \mathrm{HOCl}(\mathrm{aq}) \longrightarrow \mathrm{HClO}_{2}(\mathrm{aq})+\mathrm{H}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})$ will go essentially to completion as written for standardstate conditions.

Write balanced equations for the following important commercial reactions involving nitrogen and its compounds. (a) the principal artificial method of fixing atmospheric \(\mathrm{N}_{2}\) (b) oxidation of ammonia to \(\mathrm{NO}\) (c) preparation of nitric acid from \(\mathrm{NO}\).

Each of the following compounds produces \(\mathrm{O}_{2}(\mathrm{g})\) when strongly heated: (a) \(\mathrm{HgO}(\mathrm{s}) ;\) (b) \(\mathrm{KClO}_{4}(\mathrm{s})\) (c) \(\mathrm{Hg}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{s}) ;\) (d) \(\mathrm{H}_{2} \mathrm{O}_{2}(\mathrm{aq}) .\) Write a plausible equation for the reaction that occurs in each instance.
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