We can draw three inequivalent Lewis structures for the arsenite ion , AsO,". The concepts of formal charge and electronegativity can help us choose the structure that is the best representation. 1. Assign formal charges to the elements in each of the structures below. Note: Count oxygen atoms starting from the left for each structure. 3- As. As :0: :O: B Formal Charge As 01 02 03 2. The best Lewis structure for AsO is ot

We can draw three inequivalent Lewis structures for the arsenite ion , AsO,". The concepts of formal charge and electronegativity can help us choose the structure that is the best representation. 1. Assign formal charges to the elements in each of the structures below. Note: Count oxygen atoms starting from the left for each structure. 3- As. As :0: :O: B Formal Charge As 01 02 03 2. The best Lewis structure for AsO is ot

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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These are NOTlegitimate Lewisstructures (and aremissing formalcharges). Show (as inthe example) how apair of electrons canbe moved to make theLewis structurelegitimate.
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.
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?
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.
Explain why this Lewis structure for CO is not as valid as the Lewis structure you drew in theprevious question even though it has no “hot spots” of + or charge (formal charges).
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.
Represent the bonding in SF2 (F-S-F) with Lewis diagrams. Include the formal charges on all atoms. The dimerof this compound has the formula S2F4. It was isolated in1980 and shown to have the structure F3S-SF. Draw apossible Lewis diagram to represent the bonding in thedimer, indicating the formal charges on all atoms. Is it possible to draw a Lewis diagram for S2F4 in which all atomshave valence octets? Explain why or why not
Draw possible Lewis structures and using formal charge determine the best one for [AsSiSe]-. Show FC for ALL structures and then explain why you chose the one that is best.
Represent the bonding in SF2 (FUSUF) with Lewis diagrams. Include the formal charges on all atoms. The dimer of this compound has the formula S2F4. It was isolated in 1980 and shown to have the structure F3SUSF. Draw a possible Lewis diagram to represent the bonding in the dimer, indicating the formal charges on all atoms. Is it possible to draw a Lewis diagram for S2F4 in which all atoms have valence octets? Explain why or why not.
In Lewis theory, we use electron dot formulas and the VSEPR model to determine electron distributionand geometric structure of covalent particles. Two important basic forms are ??5 and ??6 as outlined here: SEE IMAGE. A ) Iodine (?) often forms compounds with other halogens, such as fluorine (?), chlorine (??) and bromine(??). Compare valid Lewis electron structures and VSEPR geometries of the particles: see image Write down the correct VSEPR classification (?????) for each particle and provide a valid geometry
Incomplete Lewis structures for the nitrous acid molecule,HNO2, and the nitrite ion, NO2-, are shown here. (a) Completeeach Lewis structure by adding electron pairs as needed.(b) Is the formal charge on N the same or different in thesetwo species? (c) Would either HNO2 or NO2- be expected toexhibit resonance? (d) Would you expect the N=O bond inHNO2 to be longer, shorter, or the same length as the N¬Obonds in NO2?
Incomplete Lewis structures for the nitrous acid molecule,HNO2, and the nitrite ion, NO2-, are shown here. (a) Completeeach Lewis structure by adding electron pairs as needed.(b) Is the formal charge on N the same or different in thesetwo species? (c) Would either HNO2 or NO2- be expected toexhibit resonance? (d) Would you expect the N“O bond inHNO2 to be longer, shorter, or the same length as the N¬Obonds in NO2-? [Sections 8.5 and 8.6]