Please correct answer and don't use hand rating Draw two resonance structures for the selenite anion (SeO3¾3-). Include nonbonding electrons and formal charges where necessary.

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Answered: Draw two resonance structures for the…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter6: Covalent Bonding

Section: Chapter Questions

Problem 8QRT

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Similar questions

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.
Write all resonance structures of chlorobenzene, C6H5Cl, a molecule with the same cyclic structure as benzene. In all structures, keep the CCl bond as a single bond. Which resonance structures are the most important?
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)?
Carbon monoxide (CO) is an example of an overall neutral molecule (netcharge=0) that hasnon-zero formal charges. Draw a Lewis structure of carbon monoxide (CO).
A complete Lewis structure must show all nonzero formal charges. Complete each of thefollowing Lewis structures by adding any missing formal charges.
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.]
The hypochlorite ion, ClO-, is the active ingredient inbleach. The perchlorate ion, ClO4-, is a main componentof rocket propellants. Draw Lewis structures for both ions. (a) What is the formal charge of Cl in the hypochlorite ion?(b) What is the formal charge of Cl in the perchlorate ion, assumingthe Cl—O bonds are all single bonds? (c) What is theoxidation number of Cl in the hypochlorite ion? (d) Whatis the oxidation number of Cl in the perchlorate ion, assumingthe Cl—O bonds are all single bonds? (e) In a redox reaction,which ion would you expect to be more easily reduced?
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For the next compounds/ions, draw two (2) appropriate Lewis structures. One structure must obey the octet rule and the other structure must be a non-octet obeying structure (octet deficient or octet expansion). Be sure to indicate which structure is the “best” structure and explain your choice formal charge arguments and any other points you deem important. (a) BeCl2 (b) POF3 (c) SO42−
Compare the electron dot structures of the carbonate</o:p> (CO32- ) and borate (BO33- ) ions.</o:p> (a) Are these ions isoelectronic?</o:p> (b) How many resonance structures does each ion have?</o:p> (c) What are the formal charges of each atom in these ions?</o:p> (d) If an H+ ion attaches to CO32- to form the bicarbonate ion, HCO3- , does it attach to an O atom or to the C atom?</o:p> </o:p>
Draw two electron-dot resonance structures that obey the octet rule for trichloronitromethane, CCl3NO2, and show the formal charges on N and O in both structures. (Carbon is connected to the chlorines and to nitrogen; nitrogen is also connected to both oxygens.)

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