Question 5 Consider the following incomplete structures. On your rough sheet, complete their Lewis structures (including minimizing formal charge) by adding electrons/bonds where necessary. Which statement below is true of the completed Lewis structures? Hint: Consider the potential for multiple bonds on the molecules and be sure to account for all valence electrons. The second Lewis structure has both nonzero formal charges and resonance structures, while the first Lewis structure has resonance structures but no nonzero formal charges. The first Lewis structure has non-zero formal charges but does not have resonance structures, while the second exhibits both resonance structures and nonzero formal charges O None of these O The formal charges on all the atoms are zero, and the molecules have no resonance structures. O The second Lewis structure has nonzero formal charges but no resonance structures, while the first has resonance structures but no nonzero formal charges. The first Lewis structure has nonzero formal charges and resonance structures, while the second exhibits nonzero formal charges but no resonance structures.

Question 5 Consider the following incomplete structures. On your rough sheet, complete their Lewis structures (including minimizing formal charge) by adding electrons/bonds where necessary. Which statement below is true of the completed Lewis structures? Hint: Consider the potential for multiple bonds on the molecules and be sure to account for all valence electrons. The second Lewis structure has both nonzero formal charges and resonance structures, while the first Lewis structure has resonance structures but no nonzero formal charges. The first Lewis structure has non-zero formal charges but does not have resonance structures, while the second exhibits both resonance structures and nonzero formal charges O None of these O The formal charges on all the atoms are zero, and the molecules have no resonance structures. O The second Lewis structure has nonzero formal charges but no resonance structures, while the first has resonance structures but no nonzero formal charges. The first Lewis structure has nonzero formal charges and resonance structures, while the second exhibits nonzero formal charges but no resonance structures.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter3: Atomic Shells And Classical Models Of Chemical Bonding

Section: Chapter Questions

Problem 99AP: A stable triatomic molecule can be formed that contains one atom each of nitrogen, sulfur, and...

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Similar questions

A complete Lewis structure must show all nonzero formal charges. Complete each of thefollowing Lewis structures by adding any missing formal charges.
Chloromethane has the Lewis structure _______________________________ The carbon atom is sharing 4 electron pairs. In each shared pair the carbon atom “owns” 1 electron. The number of electrons that “belong” to carbon is ___. Carbon, being a Group ___ element would have 4 , outer shell electrons in the unbonded, neutral state. Therefore, the carbon atom in chloromethane has a formal charge of zero.
These are NOTlegitimate Lewisstructures (and aremissing formalcharges). Show (as inthe example) how apair of electrons canbe moved to make theLewis structurelegitimate.
The molecular ion S3N3 has the cyclic structure All SN bonds are equivalent. (a) Give six equivalent resonance hybrid Lewis diagrams for this molecular ion. (b) Compute the formal charges on all atoms in the molecular ion in each of the six Lewis diagrams. (c) Determine the charge on each atom in the polyatomic ion, assuming that the true distribution of electrons is the average of the six Lewis diagrams arrived at in parts (a) and (b). (d) An advanced calculation suggests that the actual charge resident on each N atom is 0.375 and on each S atom is +0.041 . Show that this result is consistent with the overall +1 charge on the molecular ion.
In the Lewis structure for chloromethane, the chlorine atom is sharing _____ electron pair and “owns” _____ of those electrons. Also, the chlorine atom possesses two electrons from each of _____ unshared pairs. The total number of electrons that belong to chlorine is 7 . Chlorine is a Group ____ element. The formal charge on chlorine in chloromethane is ____.
A stable triatomic molecule can be formed that contains one atom each of nitrogen, sulfur, and fluorine. Three bonding structures are possible, depending on which is the central atom: NSF, SNF, and SFN. (a) Write a Lewis diagram for each of these molecules, indicating the formal charge on each atom. (b) Often, the structure with the least separation of formal charge is the most stable. Is this statement consistent with the observed structure for this molecule—namely, NSF, which has a central sulfur atom? (c) Does consideration of the electronegativities of N, S, and F from Figure 3.18 help rationalize this observed structure? Explain.