A newly discovered element Bm has 7 valence electrons. It is found to form the following molecular ion. :CI: :CI – Bm-Cl: (click here e if you cannot see the image) :Cl: The formal charge on the central Bm atom is [Select] Based on the Lewis structure for BmCl4* given above, the VSEPR predicted molecular geometry (i.e., molecular shape) is [ Select] Based on the Lewis structure for BmCl4* given above, there are [ Select ] pi bonds in this molecule. The hybrization of the central Bm atom is predicted to be [ Select ] . (Because of a formatting issue, the numbers could not be superscripted) The bond angles between Cl atoms surrounding the central Bm atom is predicted to be [ Select ] degrees.

A newly discovered element Bm has 7 valence electrons. It is found to form the following molecular ion. :CI: :CI – Bm-Cl: (click here e if you cannot see the image) :Cl: The formal charge on the central Bm atom is [Select] Based on the Lewis structure for BmCl4* given above, the VSEPR predicted molecular geometry (i.e., molecular shape) is [ Select] Based on the Lewis structure for BmCl4* given above, there are [ Select ] pi bonds in this molecule. The hybrization of the central Bm atom is predicted to be [ Select ] . (Because of a formatting issue, the numbers could not be superscripted) The bond angles between Cl atoms surrounding the central Bm atom is predicted to be [ Select ] degrees.

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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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.
Consider the following flat drawing of methane (CH4) . a. What is HCH bond angle implied by this drawing if you assume it is flat? b. Are the electron domains of this flat CH4 spread out as much as possible? c. Use model materials to make a model of CH4 (methane). If you assembled it correctly, thefour bonds (bonding electron domains) of your model will be 109.5° apart. d. In which representation, the drawing above or the model in your hand (circle one) are theH’s of CH4 more spread out around the central carbon? e. Confirm that your model looks like the following drawing. The wedgebond represents a bond coming out of the page, and the dash bondrepresents a bond going into the page f. You will often see methane drawn as if it were flat (like on the previous page). Why is thismisleading, and what is left to the viewer’s imagination when looking at such a drawing?
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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 ____.
These are NOTlegitimate Lewisstructures (and aremissing formalcharges). Show (as inthe example) how apair of electrons canbe moved to make theLewis structurelegitimate.
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Chloromethane has the Lewis structure _______________________________ The carbon atom is sharing 4 electron pairs. In each shared pair the carbon atom “owns” 1 electron. The number of electrons that “belong” to carbon is ___. Carbon, being a Group ___ element would have 4 , outer shell electrons in the unbonded, neutral state. Therefore, the carbon atom in chloromethane has a formal charge of zero.
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).
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