What is wrong with the Lewis structure depicted below? [Image description: A Lewis structure with a C atom singly bound to two H atoms and a 0 atom. There are three electron pairs on 0.] :ö: Н—с —н i) Multiple answers: Multiple answers are accepted for this question Select one or more answers and submit. For keyboard navigation... SHOW MORE ♥ a At least one atom has less than an octet b Separation of formal charge persists Formal charges are not minimized d. Row 2 element exceeds octet e Incorrect central atom

What is wrong with the Lewis structure depicted below? [Image description: A Lewis structure with a C atom singly bound to two H atoms and a 0 atom. There are three electron pairs on 0.] :ö: Н—с —н i) Multiple answers: Multiple answers are accepted for this question Select one or more answers and submit. For keyboard navigation... SHOW MORE ♥ a At least one atom has less than an octet b Separation of formal charge persists Formal charges are not minimized d. Row 2 element exceeds octet e Incorrect central atom

Pushing Electrons

4th Edition

ISBN:9781133951889

Author:Weeks, Daniel P.

Publisher:Weeks, Daniel P.

Chapter1: Lewis Structures

Section: Chapter Questions

Problem 35EQ: In the Lewis structure for chloromethane, the chlorine atom is sharing _____ electron pair and...

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Similar questions

These are NOTlegitimate Lewisstructures (and aremissing formalcharges). Show (as inthe example) how apair of electrons canbe moved to make theLewis structurelegitimate.
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.
It is impossible to draw a legitimate Lewis structure of a neutral NH4 molecule. Hypothetically,how many valence electrons would such a neutral NH4 molecule have ifit could exist? a. The +1 cation, NH4+ , does exist. How many valence electrons does one NH4+ ion have? b. Draw the Lewis structure for NH4+
In the Lewis structure for chloromethane, the chlorine atom is sharing _____ electron pair and “owns” _____ of those electrons. Also, the chlorine atom possesses two electrons from each of _____ unshared pairs. The total number of electrons that belong to chlorine is 7 . Chlorine is a Group ____ element. The formal charge on chlorine in chloromethane is ____.
The molecules BH3 and SF6 and the ion SO42 exist and are stable. Draw a Lewis structure of each,and comment on whether they are exceptions to Lewis’ octet rule.
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.
White phosphorus (P4) consists of four phosphorus atoms arranged at the corners of a tetrahedron. Draw the valence electrons on this structure to give a Lewis diagram that satisfies the octet rule.
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 formal charges on all the atoms in the following Lewis diagrams. Which one would best represent bonding in the molecule Cl2O ?