How many resonance structures can be drawn for the perbromate ion (BrO4) in which the central bromine atom bears a -1 formal charge and theoxygens bear formal charges of either zero or-1? Enter your answer as a whole number.AnswerInstrucEnter ValueCQueQues

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Answered: How many resonance structures can be…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter9: Chemical Bonds

Section: Chapter Questions

Problem 9.17QE

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Write the correct Lewis structure and assign a formal charge to each atom in fulminate ion, CNO.
Consider the pyrosulfate ion, S2O72-. It has no sulfurâ€“sulfur nor oxygenâ€“oxygen bonds. (a) Write a Lewis structure for the pyrosulfate ion using only single bonds. (b) What is the formal charge on the sulfur atoms for the Lewis structure you drew in part (a)? (c) Write another Lewis structure using six bonds and two Oâ€”S bonds. (d) What is the formal charge on each atom for the structure you drew in part (c)?
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
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.
Draw a Lewis diagram for BrO4- in which the central Br atom has a formal charge of zero and show all NONZERO formal charges on all atoms. Note that the overall charge on this ion is -1.
How many resonance structures can be drawn for the hydrogen tellurate ion (HTeO4–) in which the central tellurium atom bears a –1 formal charge and the oxygens bear formal charges of either zero or –1? Enter your answer as a whole number.
The Lewis structure for the chlorate ion is :0: Calculate the formal charge on the chlorine (Cl ) atom. Express your answer as an integer. • View Available Hint(s) formal charge on Cl = Submit Part B Calculate the formal charge on each of the oxygen (O) atoms labeled a, b, and c in the following Lewis structure. :0: Express your answers as integers separated by commas. • View Available Hint(s) formal charge on Oa , Ob , Oc = Submit ormal charges to predict the most stable structure he interactive activity shows how to calculate the formal charge of atoms in a structure. These formal charges can be used to predict the resonance structure that contributes most to the stability of a molecule or ion. The struc enerally the most stable. Part C What are the formal charges on the sulfur (S), carbon (C ), and nitrogen (N ) atoms, respectively, in the resonance structure that contributes most to the stability of the thiocyanate ion, SCN¯ ? The possible resonance structures for the thiocyanate…
Calculating Formal Charge: Formal charge is calculated for each atom in a structure. It provides information about the stability and reactivity of the atom in the molecule. Formal Charge = Valence Electrons - 1/2 Bonding Electrons - Non-bonding Electrons For example, the formal charge on the carbon of methane is calculated here. Carbon has 4 valence electrons. There are 8 bonding electrons around it. Formal Charge4- 12 (8) -0 Calculate the formal charge on the circled atoms in the following structures. formal charge: Incorect formal charge: formal charge: 1 Incomect
The carbonate anion, CO32- , is a resonance hybrid. Draw all of the important resonance structures for this molecule. If an atom has a nonzero formal charge, be sure the formal charge is shown clearly in the structure. Use the resonance structures to calculate the average formal charge on each O atom (which are all equivalent in the "true" structure). [Note: all of the important contributing resonance structures have octets around each atom that desires an octet.]
Consider the incomplete structure shown. Determine the formal charge on the bromine atom in the structure. If the atom is formally neutral, indicate a charge of zero.
Draw a Lewis structure for IO4- in which the octet rule is satisfied on all atoms and show all NONZERO formal charges on all atoms. Note that the overall charge on this ion is -1.
For the phosphoric acid molecule (H3PO4), all four oxygen atoms are bonded to the central phosphorus atom and the three hydrogen atoms are bonded to different oxygen atoms. Several resonance structures can be drawn for H3PO4 but one structure is more important than the others. In the most important structure, the phosphorus atom has: a formal charge of +1 and a complete octet a formal charge of zero and a complete octet a formal charge of −1 and an expanded octet a formal charge of +5 and an expanded octet a formal charge of zero and an expanded octet

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How many resonance structures can be drawn for the perbromate ion (BrO4) in which the central bromine atom bears a -1 formal charge and the oxygens bear formal charges of either zero or-1? Enter your answer as a whole number. Answer Instruc Enter Value C Que Ques