Problem 8.64

(a)Describe the molecule chlorine dioxide, ClO₂, in terms of three possible resonance structures. (b)Do any of these structures obey the octet rule for every atom in the molecule? Why or why not(c) Using formal charges, select the resonance form(s) that is (are) most important.

The resonance structures and formal charges are shown below:

Notice that the chlorine dioxide molecule has an odd number of electrons (19). None of these resonance structures satisfies the octet rule; in each of these resonance structures, one of the atoms has an odd number of electrons around it. Formal charge arguments predict that the two resonance structures with the odd electron on O are most important (these give the lowest formal charges.) This is a little counterintuitive - we would expect the more electronegative element (oxygen) to have the full octet.

If you have any questions or comments, reply to chapman@sou.edu

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Doug Chapman chapman@sou.edu 6/25/08

Problem 8.64

(a)Describe the molecule chlorine dioxide, ClO2, in terms of three possible resonance structures. (b)Do any of these structures obey the octet rule for every atom in the molecule? Why or why not(c) Using formal charges, select the resonance form(s) that is (are) most important.

(a)Describe the molecule chlorine dioxide, ClO₂, in terms of three possible resonance structures. (b)Do any of these structures obey the octet rule for every atom in the molecule? Why or why not(c) Using formal charges, select the resonance form(s) that is (are) most important.