THE COMPLETE QUESTION IS HERE Use the following information to determine the formal charges on the atoms and the overall bestresonance structure.NOTE that brackets and charges are not shown, please use the iformation below!Atom information:A: 5 valence electrons, CAN exceed the octet. Further from fluorine on the periodic tablethan X.X: 6 valence electrons, CANNOT exceed the octet. Closer to fluorine on the periodic tablethan A.Molecule information: AX1)*:汉:2)3):X:4)Formal charge on A in Structure 1[Choose]Formal charge on A in Structure 2( Choose]Formal charge on A in Structure 3[Choose ]:X::X: :X:::3)4)Formal charge on A in Structure 1[ Choose ]Formal charge on A in Structure 2[ Choose ]Formal charge on A in Structure 3[Choose ]Formal charge on A in Structure 4[Choose]Formal charge on single bonded X[ Choose]Formal charge on double bonded X[Choose]Best overall structure[Choose]

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:X: :X: 3) 4) A=X Formal charge on A in Structure 1 [ Choose ] Formal charge on A in Structure 2 [ Choose ] Formal charge on A in Structure 3 [ Choose ] Formal charge on A in Structure 4 [Choose] Formal charge on single bonded X [Choose ] Formal charge on double bonded X [ Choose ] Best overall structure [ Choose ] :X:

:X: :X: 3) 4) A=X Formal charge on A in Structure 1 [ Choose ] Formal charge on A in Structure 2 [ Choose ] Formal charge on A in Structure 3 [ Choose ] Formal charge on A in Structure 4 [Choose] Formal charge on single bonded X [Choose ] Formal charge on double bonded X [ Choose ] Best overall structure [ Choose ] :X:

Pushing Electrons

4th Edition

ISBN:9781133951889

Author:Weeks, Daniel P.

Publisher:Weeks, Daniel P.

Chapter1: Lewis Structures

Section: Chapter Questions

Problem 35EQ: In the Lewis structure for chloromethane, the chlorine atom is sharing _____ electron pair and...

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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 ____.
the formal charges on all the atoms in the following Lewis diagrams. Which one would best represent bonding in the molecule Cl2O ?
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.
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.
A complete Lewis structure must show all nonzero formal charges. Complete each of thefollowing Lewis structures by adding any missing formal charges.
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.
Two possible Lewis diagrams for sulfine (H2CSO) are (a) Compute the formal charges on all atoms. (b) Draw a Lewis diagram for which all the atoms in sulfine have formal charges of zero.
Carbon monoxide (CO) is an example of an overall neutral molecule (netcharge=0) that hasnon-zero formal charges. Draw a Lewis structure of carbon monoxide (CO).
The Lewis structure of acetone is Circling the carbonyl carbon, i.e., the carbon atom attached to oxygen, and its octet gives Circling the oxygen atom and its octet gives Thus, atoms share electrons in making bonds, and a pair of electrons may be included in the octet of two different atoms. When computing the formal charge on an atom, the number of electrons that belong to that atom is compared with the number of electrons the atom would have in the unbonded and neutral state. If the two numbers are the same, the formal charge on the atom is zero. In a Lewis structure both electrons in an unshared pair belong to the atom, and one of every pair of shared (bonding) electrons belongs to the atom.
White phosphorus (P4) consists of four phosphorus atoms arranged at the corners of a tetrahedron. Draw the valence electrons on this structure to give a Lewis diagram that satisfies the octet rule.
Write all possible resonance structures for the following species. Assign a formal charge to each atom. In each case, which resonance structure is the most important? (a) NO2 (nitrogen is central) (b) ClCN
Determine the formal charge for the atom indicated in the structures below. ASSUME that the structures are drawn correctly and that you do not have to change them due to formal charge issues. The external atom in this structure. :O: :O! Ar 11 :0: The central atom in this structure. = :0: (1 Si = : 0: 2- 1. +1 2. +2 3. +3 4. 0 5. -3 6.-2 7. -1