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Chapter 10: Problem 48

Which of the following species requires a resonance hybrid for its Lewis structure: (a) \(\mathrm{CO}_{2},\) (b) \(\mathrm{OCl}^{-}\) (c) \(\mathrm{CO}_{3}^{2-},\) or \((\mathrm{d}) \mathrm{OH}^{-} ?\) Explain.

Short Answer

Expert verified
Out of the four species given, only \(\mathrm{CO}_{3}^{2-}\) requires a resonance hybrid for its Lewis structure.

Step by step solution

01

Draw the Lewis Structure for CO2

The Lewis structure for CO2 includes one carbon atom and two oxygen atoms. Carbon has four valence electrons and each oxygen atom has six, giving a total of 16 valence electrons. Four electrons are used to form two double bonds (one with each of the oxygen atoms), while the remaining 12 are arranged as lone pairs around the oxygen atoms. No matter how these electrons are shifted, we always end up with the same structure, so we conclude that CO2 has only one valid Lewis structure and hence does not have resonance.
02

Draw the Lewis Structure for OCl-

The Lewis structure for OCl- includes one oxygen atom and one chlorine atom, and additionally one electron because of the -1 charge. Oxygen has six valence electrons, chlorine has seven, and there is one extra electron, giving a total of 14 valence electrons. The oxygen and chlorine atoms are bonded with a single bond, using two electrons. The remaining 12 electrons form six lone pairs: three on the oxygen atom, and three on the chlorine atom. No matter how these electrons are rearranged, we can't get another valid Lewis structure, so OCl- also doesn't have resonance.
03

Draw the Lewis Structure for CO3 2-

The Lewis structure for CO3 2- includes one carbon atom and three oxygen atoms, and additionally two electrons because of the -2 charge. Carbon has four valence electrons, each oxygen has six, and there are two extra electrons, giving a total of 24 valence electrons. We arrange these electrons to form double bonds with one of the oxygen atoms, and single bonds with the other two. The remaining electrons form lone pairs. There are three ways we can arrange these bonds, with the double bond being at a different position in each arrangement, so CO3 2- does have resonance.
04

Draw the Lewis Structure for OH-

The Lewis structure for OH- includes one oxygen atom and one hydrogen atom, and additionally one electron because of the -1 charge. Oxygen has six valence electrons, hydrogen has one, and there is one extra electron, giving a total of 8 valence electrons. The oxygen and hydrogen atoms are bonded with a single bond, using two electrons. The remaining electrons are on the oxygen atom. There is only one way we can arrange the bonds and lone pairs, so OH- does not have resonance.

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Most popular questions from this chapter

A pair of isoelectronic species for \(C\) and \(N\) exist with the formula \(\mathrm{X}_{2} \mathrm{O}_{4}\) in which there is an \(\mathrm{X}-\mathrm{X}\) bond. \(\mathrm{A}\) corresponding fluoride of boron also exists. Draw Lewis structures for these species and describe their shapes.

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) \(\mathrm{C}_{2} \mathrm{H}_{6}\) \(\left(\mathrm{H}_{3} \mathrm{CCH}_{3}\right) ;(\mathrm{d}) \mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\left(\mathrm{H}_{3} \mathrm{COCH}_{3}\right)\).

Construct a concept map illustrating the connections between Lewis dot structures, the shapes of molecules, and polarity.

In certain polar solvents, \(\mathrm{PCl}_{5}\) undergoes an ionization reaction in which a \(\mathrm{Cl}^{-}\) ion leaves one \(\mathrm{PCl}_{5}\) molecule and attaches itself to another. The products of the ionization are \(\mathrm{PCl}_{4}^{+}\) and \(\mathrm{PCl}_{6}^{-}\). Draw a sketch showing the changes in geometric shapes that occur in this ionization (that is, give the shapes of \(\mathrm{PCl}_{5}\), \(\mathrm{PCl}_{4}^{+},\) and \(\mathrm{PCl}_{6}^{-}\) ). $$2 \mathrm{PCl}_{5} \rightleftharpoons \mathrm{PCl}_{4}^{+}+\mathrm{PCl}_{6}^{-}$$

Represent the following ionic compounds by Lewis structures: (a) barium hydroxide; (b) sodium nitrite; (c) magnesium iodate; (d) aluminum sulfate.
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