Please answer question 6 part A and B Formal charge (FC) keeps track of which electrons anatom "owns" in a chemical bond with the equationPart Avalence einvalence e inFC =Due to the small and highly electronegative nature of fluorine, the oxyacids of the this element are much lesscommon and less stable than those of the other halogens. Bonding theory, however, does allow one to proposestructures for these acids and use formal charges for the evaluation of these structures. For a molecule of fluorousacid, the atoms are arranged as HOFO. (Note: In this oxyacid, the placement of fluorine is an exception to the ruleof putting the more electronegative atom in a terminal position.)free atombonded atomWhen more than one valid Lewis structure can be drawnfor a particular molecule, formal charge is used to predictthe most favorable structure.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 writtenas +1.• View Available Hint(s)Formal Charge for H, O, F, O =Part BFigure1 of 1Two possible electron-dot structures are shown for the cyanate ion, NCO¯. (Figure 1) What can you conclude abouthow favorable the structures are?• View Available Hint(s):NEC-Ö::N-c=0:Structure A is more favored.Structure B is more favored.АВThe structures are equally favored.

Formal charge = [ number of valance electron ] -[non bonding electron + number of bonds ]

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 other halogens. Bonding theory, however, does allow one to propose structures for these acids and use formal charges for the evaluation of these structures. For a molecule 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 more electronegative 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) Formal Charge for H, O, F, O = |

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 other halogens. Bonding theory, however, does allow one to propose structures for these acids and use formal charges for the evaluation of these structures. For a molecule 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 more electronegative 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) Formal Charge for H, O, F, O = |

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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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.
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.
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D Lewis strct molecalar iodie, and the dide in
Three compounds that contain an element from Group 18 are XEOF4, XEO2F2, and XeF4. Possible Lewis electron dot diagrams for the compounds are shown below. :ö: :F: :0: || :F-Xe :0: :0: || F: :F-Xe 一X -Xe- 1. E-Xe-F: II. :0: :0: :ö: C :F: A В D E (c) Which structure, B, C, or D, minimizes the formal charges for each atom in XeO2F2 ? Justify your choice. :i:
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Consider the Lewis structure for the polyatomic oxyanionshown here, where X is an element from the third period(Na - Ar). By changing the overall charge, n, from 1- to2- to 3- we get three different polyatomic ions. For each ofthese ions (a) identify the central atom, X; (b) determine theformal charge of the central atom, X; (c) draw a Lewis structurethat makes the formal charge on the central atom equalto zero.
Use the information on the fictious nonmetal elements. to answer the following Element Colomn EN ff 1.9 14 17 3.1 2.3 3.6 15 Nn 16 Shoos one of the followng mokcular compounds and completc the queSTIons: Nn Oyzlshape is benti V) ODraw a leuis Structure Shoudng all lalonce electrons. ) Calculate the electrongativity the bond. State what a paar covalert band, notate the partial difference for Gf bond will form If it is charges d) Detamine if the molecule is polar or polar. non-
N MyLab and Mastering Course Home b Search results for "Which of the At Electronegativity Table of the Ele x + A openvellum.ecollege.com/course.html?courseld=16418591&OpenVellumHMAC=fd2ce09746a2194453c324a109d1a8ec#10001 Scores Part A Pearson eText Part B Study Area Indicate the more electronegative atom in each pair. Match the atoms in the left column to the appropriate blanks in the sentences on the right. Document Sharing User Settings Reset Help Course Tools > B Given the bond P-N, the more electronegative atom in the bond is Given the bond B-F, the more electronegative atom in the bond is Br Given the bond H-Br, the more electronegative atom in the bond is H P N Submit Request Answer P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy. | Permissions | Contact Us | 2:55 AM P Type here to search 4/14/2021
Tap - Cengage Learning vo/index.html?deploymentld%355750828934189288909969212&elSBN=9781305657571&snapshotld%3D2199898&id%31... NDTAP Use the References to access important values if needed for this question. Draw (on paper) Lewis structures for phosphoric acid and the nitrate ion. How many equivalent Lewis structures are necessary to describe the bonding in PO(OH)3? How many equivalent Lewis structures are necessary to describe the bonding in NO3"? Submit Answer 5 question attempts remaining