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Chapter 10: Problem 20

Although the notion that a Lewis structure in which formal charges are zero or held to a minimum seems to apply in most instances, describe several significant situations in which this appears not to be the case.

Short Answer

Expert verified
Exceptions to minimizing formal charges in Lewis structures occur in cases of hypervalent molecules, free radicals, and resonance structures.

Step by step solution

01

Examples of Exceptions to the Rule

1. Hypervalent Molecules: These refer to molecules that have more than an octet of electrons around the central atom, like PCl5, SF6 etc. In these instances, the central atom has formal charge of zero but still violates the octet rule.2. Free Radicals: Molecules where an unpaired electron exists, such as the nitric oxide (NO). Here the N atom cannot have a formal charge of zero unless it violates the octet rule.3. Resonance Structures: In instances of resonance where the molecule is better represented by a blend of structures rather than a single one, as in the case of Ozone (O3) or Benzene (C6H6), the minimization of formal charges doesn't always apply.
02

Conclusions

While it's generally a good rule of thumb to create Lewis Structures where formal charges are held to a minimum, there are certain situations where this is not the case. Understanding these exceptions will provide a greater understanding of molecular geometry and make predictions about chemical behavior more accurate.

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Most popular questions from this chapter

If you have four electron pairs around a central atom, under what circumstances can you have a pyramidal molecule? Similarly, how can you have a bent molecule? What are the expected bond angles in each case?

The molecular shape of \(\mathrm{BF}_{3}\) is planar (see Table 10.1 ). If a fluoride ion is attached to the \(B\) atom of \(B F_{3}\) through a coordinate covalent bond, the ion \(\mathrm{BF}_{4}^{-}\) results. What is the shape of this ion?

Without referring to tables or figures in the text other than the periodic table, indicate which of the following atoms, \(\mathrm{Bi}, \mathrm{S}, \mathrm{Ba}, \mathrm{As},\) or \(\mathrm{Mg},\) has the intermediate value when they are arranged in order of increasing electronegativity.

Briefly describe each of the following ideas: (a) formal charge; (b) resonance; (c) expanded valence shell; (d) bond energy.

Which of the following molecules would you expect to be polar: (a) \(\mathrm{HCN} ;\) (b) \(\mathrm{SO}_{3} ;\) (c) \(\mathrm{CS}_{2} ;\) (d) OCS; (e) \(\operatorname{SOCl}_{2} ;\) (f) \(\operatorname{SiF}_{4} ;\) (g) \(\operatorname{POF}_{3}\) ? Give reasons for your conclusions.
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