Figure[EN=C-03]A< 1 of 1 >EN-C=O:]BTwo possible electron-dot structures are shown for the cyanate ion, NCO. (Figure 1) What can you conclude about how favorable the structures are?►View Available Hint(s)▶O Structure A is more favored.O Structure B is more favored.O The structures are equally favored.SubmitProvide FeedbackNext > A bonded atom is considered to "own" all its nonbonding electrons but only half of the bonding electrons because these are shared with another atom. Therefore,the formal charge formula can be rewritten as follows:TC▼Part AFC=valence e infree atomnonbonding eshownFormal Charge for H, O, F, O =+12bonding eshown[)]Due to the small and highly electronegative nature of fluorine, the oxyacids of the this element are much less common and less stable than those of the otherhalogens. Bonding theory, however, does allow one to propose structures for these acids and use formal charges for the evaluation of these structures. For almolecule of fluorous acid, the atoms are arranged as HOFO. (Note: In this oxyacid, the placement of fluorine is an exception to the rule of putting the moreelectronegative atom in a terminal position.)What is the formal charge on each of the atoms? Enter the formal charges in the same order as the atoms are listed.Express your answers as charges separated by comma. For example, a positive one charge would be written as +1.▸ View Available Hint(s)

Lewis structure is the representation of valence electrons in a molecule. It is used to show how…

Figure EC-Ö:] :NEC A < 1 of 1 > [EN-C=O: B Two possible electron-dot structures are shown for the cyanate ion, NCO. (Figure 1) What can you conclude about how favorable the structures are? ►View Available Hint(s) O Structure A is more favored. O Structure B is more favored. O The structures are equally favored. Submit Provide Feedback Next >

Figure EC-Ö:] :NEC A < 1 of 1 > [EN-C=O: B Two possible electron-dot structures are shown for the cyanate ion, NCO. (Figure 1) What can you conclude about how favorable the structures are? ►View Available Hint(s) O Structure A is more favored. O Structure B is more favored. O The structures are equally favored. Submit Provide Feedback Next >

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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Distinguish between the terms electronegativity versus electron affinity, covalent bond versus ionic bond, and pure covalent bond versus polar covalent bond. Characterize the types of bonds in terms of electronegativity difference. Energetically, why do ionic and covalcnt bonds form?
The molecule nitrosyl chloride, NOCl, has a skeleton structure of ONCl. Two resonance forms can be written; write them both. Use the formal charge stability rules to predict which form is more stable.
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)?
Define formal charge and explain how to calculate it. What is the purpose of the formal charge? Organic compounds are composed mostly of carbon and hydrogen but also may have oxygen, nitrogen, and/or halogens in the formula. Formal charge arguments work very well for organic compounds when drawing the best Lewis structure. How do C, H, N, O, and Cl satisfy the octet rule in organic compounds so as to have a formula charge of zero?
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?
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.
Draw resonance structures for each of these ions: NSO− and SNO−. (The atoms are bonded in the order given in each case, that is, S is the central atom in NSO−.) Use formal charges to determine which ion is likely to be more stable. Explain why the two ions cannot be considered resonance structures of each other.
Fill in the blanks in each line of the following table that involves characteristics of various bonds between nonmetals. The first line is already completed as an example.
The percent ionic character of a bond can be approximated by the formula 16+3.52 , where is the magnitude of the difference in the electronegativities of the atoms (see Fig. 3.18). Calculate the percent ionic character of HF, HCl, HBr, HI, and CsF, and compare the results with those in Table 3.7.