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Chapter 9: Problem 104

Several resonance structures for the molecule \(\mathrm{CO}_{2}\) are shown. Explain why some of them are likely to be of little importance in describing the bonding in this molecule.

Short Answer

Expert verified
Some resonance structures for the molecule \(\mathrm{CO}_{2}\) are of little importance in describing the bonding in this molecule because they lead to increased formal charges on the atoms, which makes these structures less stable. The \(\mathrm{CO}_{2}\) molecule is most stable and correctly described by a structure where carbon is double bonded to each oxygen, resulting in a formal charge of zero for all atoms.

Step by step solution

01

Understanding Resonance Structures

Resonance structures are a combination of multiple Lewis structures that exist for some molecules where the bonding can't be accurately depicted by a single structure but instead exists as a hybrid of these structures. Lewis structures are diagrams that depict the bonding between atoms of a molecule, as well as any unbonded electron pairs.
02

Understanding Formal Charge

Formal charge is a useful way to predict the most likely structure of a molecule. It's calculated by comparing the number of valence electrons in an isolated atom against the number of electrons assigned to it in a molecule. In general, structures with lower formal charges are more significant contributers to the overall structure of the molecule. Structures with formal charges closest to zero are typically the most stable and hence are the major contributors.
03

Analyzing \(\mathrm{CO}_{2}\) Resonance Structures

In the case of \(\mathrm{CO}_{2}\), the molecule is linear with carbon in the center, and carries no net charge, thus the molecule is most stable when the formal charges of all atoms are zero. The major resonance structure of \(\mathrm{CO}_{2}\) places double bonds between the carbon atom and the oxygen atoms. Any other resonance structures that might place a formal charge on the atoms, for example by creating single or triple bonds, would increase the formal charges on these atoms and thus are less stable and contribute little to the actual bonding in the molecule.

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Most popular questions from this chapter

What is lattice energy and what role does it play in the stability of ionic compounds?

Most organic acids can be represented as \(\mathrm{RCOOH}\) where \(\mathrm{COOH}\) is the carboxyl group and \(\mathrm{R}\) is the rest of the molecule. (For example, \(\mathrm{R}\) is \(\mathrm{CH}_{3}\) in acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH} .\) ) (a) Draw a Lewis structure for the carboxyl group. (b) Upon ionization, the carboxyl group is converted to the carboxylate group, \(\mathrm{COO}^{-}\). Draw resonance structures for the carboxylate group.

Draw reasonable resonance structures for the following ions: (a) \(\mathrm{HSO}_{4}^{-},\) (b) \(\mathrm{PO}_{4}^{3-},\) (c) \(\mathrm{HSO}_{3}^{-}\) (d) \(\mathrm{SO}_{3}^{2-}\). (Hint: See comment on Example \(\left.9.11 .\right)\)

Summarize the essential features of the Lewis octet rule.

What is bond enthalpy? Bond enthalpies of polyatomic molecules are average values, whereas those of diatomic molecules can be accurately determined. Why?
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