Concept explainers
(a)
Interpretation:
The curve arrow should be drawn for contributing structure and all formal charges have to be shown.
Concept introduction:
Resonance: The delocalization of electrons which is characterized as several structural changes.
(b)
Interpretation:
The curve arrow should be drawn for contributing structure and all formal charges has to be shown.
Concept introduction:
Resonance: The delocalization of electrons which is characterized as several structural changes.
(c)
Interpretation:
The curve arrow should be drawn for contributing structure and all formal charges has to be shown.
Concept introduction:
Resonance: The delocalization of electrons which is characterized as several structural changes.
(d)
Interpretation:
The curve arrow should be drawn for contributing structure and all formal charges has to be shown.
Concept introduction:
Resonance: The delocalization of electrons which is characterized as several structural changes.
(e)
Interpretation:
The curve arrow should be drawn for contributing structure and all formal charges has to be shown.
Concept introduction:
Resonance: The delocalization of electrons which is characterized as several structural changes.
(e)
Interpretation:
The curve arrow should be drawn for contributing structure and all formal charges has to be shown.
Concept introduction:
Resonance: The delocalization of electrons which is characterized as several structural changes.
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Chapter 1 Solutions
Organic Chemistry
- Assign formal charges to all atoms in the following Lewis diagrams. (a) SO42 (b) S2O32 (c) SbF3 (d) SCNarrow_forwardDraw the contributing structure indicated by the curved arrow(s). Assign formal charges as appropriate.arrow_forwardCalculate the formal charge on each of the atoms in the Lewis structure given. Be sure to answer all parts. H: N: O (of OH): O: Nitrous acidarrow_forward
- Keeping the same atomic connections and moving only electrons, write a more stable Lewis structure for each of the following. Be sure to specify formal charges, if any, in the new structure. (g) (h) (i)arrow_forwardDraw ALL THREE (3) possible Lewis structures for FNO (N is the central atom) and identify the dominant structure using formal charges.arrow_forwardThe two compounds nitrogen dioxide and dinitrogentetraoxide are introduced in Section 3.13.(a) NO2 is an odd-electron compound. Draw the bestLewis diagrams possible for it, recognizing that oneatom cannot achieve an octet configuration. Use formal charges to decide whether that should be the(central) nitrogen atom or one of the oxygen atoms.(b) Draw resonance forms for N2O4 that obey the octetrule. The two N atoms are bonded in this molecule.arrow_forward
- 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>arrow_forwardAssign formal charges for all the atoms in the sulphate ion, SO.arrow_forwardWrite Lewis structures for these ions. Show all valence electrons and all formal charges. (Q)Nitrate ion, NO3 -arrow_forward
- In an ammonium, nitrogen has a valence of 4, and zero nonbonding electrons. What is the correct formal charge of nitrogen with 4 covalent bonds?arrow_forward(a) Determine the formal charge of oxygen in the following structure. If the atom is formally neutral, indicate a charge of zero. (b) Draw an alternative Lewis (resonance) structure for the compound given in part (a). Show the unshared pairs and nonzero formal charges in your structure. Don't use radicals. Formal charge on O 0arrow_forward12. Draw 2 resonance structures for each of the following two molecules/ions. Make sure you include formal charges on all atoms. Indicate which of the 2 resonance structures is preferred. (a) N2O (b) SCN-arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningPrinciples of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning