3. What are the formal charges, if any, on atoms other than carbon and hydrogen inthe following molecule?H H:S=C=N-C-C-H|H H

Formal charge of an atom in a molecule is the difference of electrons around the atom in a moluclue…

Answered: 3. What are the formal charges, if any,…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter6: Covalent Bonding

Section: Chapter Questions

Problem 98QRT

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Similar questions

Based on the concept of formal charge, what is the central atom in (a) HCN (do not include H as a possibility)? b) NOCI (Cl is always a terminal atom)?
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).
Three known isomers exist of N2CO, with the atoms in these sequences: NOCN; ONNC; and ONCN. Write resonance structures for each isomer and use formal charge to predict which isomer is the most stable.
Given the bonds C N, C H, C Br, and S O, (a) which atom in each is the more electronegative? (b) which of these bonds is the most polar?
Write the correct Lewis structure and assign a formal charge to each atom in fulminate ion, CNO.
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.
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
Iodine forms a series of fluorides (listed here). Write Lewis structures for each of the four compounds and determine the formal charge of the iodine atom in each molecule: (a) IF (b) IF3 (c) IF5 (d) IF7
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.
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.
Acrylonitrile is the building block of the synthetic fiber Orlon. Acrylonitrile Which carbon-carbon bond is shorter? Which carbon-carbon bond is stronger? Which bond is the most polar? What is the partial negative end of that bond?
What is the formal charge on the indicated atom in each of the following species? (a) sulfur in SO2 (b) nitrogen in N2H4 (c) each oxygen atom in ozone, O3

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3. What are the formal charges, if any, on atoms other than carbon and hydrogen in the following molecule? H H :S=C=N-C-C-H | H H