The formal charge is the "charge" an element would have in a molecule or ion if all of thebonding electrons were shared equally between atoms.We can draw three inequivalent Lewis structures for carbonyl sulfide, SCO. The concepts of formalcharge and electronegativity can help us choose the structure that is the most significant representation.1. Assign formal charges to the elements in each of the structures below...:S=C O:S-C=0:S=CAFormal ChargeSCBC2. The structure that contributes most significantly to the overall electronic structure of SCO is We can draw three inequivalent Lewis structures for the selenite ion, SeO3². The concepts of formalcharge 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.Formal ChargeSe010203.SeSeSeO::0::0::0:CBA2. The best Lewis structure for SeO3²- isPreviouNext

Answered: The formal charge is the "charge" an…

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter3: Bonding: General Concepts

Section: Chapter Questions

Problem 101E: A common trait of simple organic compounds is to have Lewis structures where all atoms have a formal...

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A common trait of simple organic compounds is to have Lewis structures where all atoms have a formal charge of zero. Consider the following incomplete Lewis structure for an organic compound called methyl cyanoacrylate, the main ingredient in Super Glue. Draw a complete Lewis structure for methyl cyanoacrylate in which all atoms have a formal charge of zero.
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.
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?
Write Lewis formulas for the BF molecule (two with a single BF bond, two with a double BF bond, and one with a triple BF bond) in which the octet rule is satisfied for at least one of the atoms. Obtain the formal charges of the atoms. Based on the information you have, is there one formula that you think best describes the molecule? Explain. For this best Lewis formula, give the valence bond description of the bonding.
Draw the structure of hydroxylamine, H3NO, and assign formal charges; look up the structure. Is the actual structure consistent with the formal charges?
Define the term lattice energy. Why, energetically, do ionic compounds form? Fig. 3-8 illustrates the energy changes involved in the formation of MgO(s) and NaF(s). Why is the lattice energy of MgO(s) so different from that of NaF(s)? The magnesium oxide is composed of Mg2+ and O2 ions. Energetically, why does Mg2+O2 form and not Mg+O? Why doesnt Mg3+O3 form?
Think of forming an ionic compound as three steps (this is a simplification, as with all models): (I) removing an electron from the metal; (2) adding an electron to the nonmetal; and (3) allowing the metal cation and nonmetal anion to come together. a. What is the sign of the energy change for each of these three processes? b. In general, what is the sign of the sum of the first two processes? Use examples to support your answer. c. What must be the sign of the sum of the three process d. Given your answer to part c, why do ionic bonds occur? e. Given your above explanations, why is NaCl stable but not Na2Cl? NaCl2? What about MgO compared to MgO2? Mg2O?
The chemistry of the nitrite ion and HNO2: (a) Two resonance structures are possible for NO2. Draw these structures, and then find the formal charge on each atom in each resonance structure. (b) In forming the acid HNO2 an H+ ion attaches to the O atom and not the N atom of NO2. Explain why you would predict this result. (c) Two resonance structures are possible for HNO2. Draw these structures, and then find the formal charge on each atom in each resonance structure. Is either of these structures strongly preferred over the other?
These are NOTlegitimate Lewisstructures (and aremissing formalcharges). Show (as inthe example) how apair of electrons canbe moved to make theLewis structurelegitimate.
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?
number 2 asks A B or C
Give a clear handwritten answer with explanation

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