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Chapter 10: Problem 23

The concept of formal charge helped us to choose the more plausible of the I ewis structures for \(\mathrm{NO}_{2}^{+}\) given in expressions (10.14) and \((10.15) .\) Can it similarly help us to choose a single Lewis structure as most plausible for \(\mathrm{CO}_{2} \mathrm{H}^{+} ?\) Explain.

Short Answer

Expert verified
By drawing the possible Lewis structures for \(\mathrm{CO}_{2} \mathrm{H}^{+}\) and assessing the formal charges on each atom within these structures, one can identify the most plausible structure as the one where the formal charges on individual atoms are lowest and closest to zero.

Step by step solution

01

Draw Possible Structures

First, start by drawing all possible Lewis structures for \(\mathrm{CO}_{2} \mathrm{H}^{+}\). This molecule has 13 total valence electrons, so these electrons need to be distributed in such a way that every atom has a complete octet (apart from hydrogen, which only requires two electrons).
02

Calculate Formal Charges

Calculate the formal charges for each atom in each structure. The formal charge is calculated using the formula: Formal charge = [No. of valence electrons in the free atom] – [No. of non-bonding electrons + 1/2 the number of bonding electrons]. Apply this formula to each atom in the structures.
03

Evaluate Structures Based on Formal Charges

The most plausible Lewis structure will be the one in which the atoms bear the least formal charge possible, because formal charge is an indication of the electron distribution in a molecule. Structures in which formal charges are closest to zero will be more plausible.

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Most popular questions from this chapter

Use VSEPR theory to predict the geometric shapes of the following molecules and ions: (a) \(\mathrm{N}_{2}\); (b) HCN; (c) \(\mathrm{NH}_{4}^{+} ;\) (d) \(\mathrm{NO}_{3}^{-} ;\) (e) NSF.

Sketch the propene molecule, \(\mathrm{CH}_{3} \mathrm{CH}=\mathrm{CH}_{2}\). Indicate the bond angles in this molecule. What is the maximum number of atoms that can be in the same plane?

One of the allotropes of sulfur is a ring of eight sulfur atoms. Draw the Lewis structure for the \(S_{8}\) ring. Is the ring likely to be planar? The \(S_{8}\) ring can be oxidized to produce \(S_{8}\) O. In \(S_{8} O,\) the oxygen atom is bonded to one of the S atoms and the Sg ring is still intact. Draw the Lewis structure for \(\mathrm{S}_{8} \mathrm{O}\).

Which of the following species would you expect to be diamagnetic and which paramagnetic: (a) \(\mathrm{OH}^{-} ;\) (b) \(\mathrm{OH} ;(\mathrm{c}) \mathrm{NO}_{3} ;(\mathrm{d}) \mathrm{SO}_{3} ;(\mathrm{e}) \mathrm{SO}_{3}^{2-} ;(\mathrm{f}) \mathrm{HO}_{2} ?\)

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