Complete the table. Number of electron groups Bond angle Outer atoms/Lone pairs 2 ? 2/0 3 ? ? bond angle in a two electron group molecule: bond angle in a three electron group molecule: bond angle in a four electron group molecule: 3/0 2/1 4/0 3/1 2/2 Shape ? trigonal planar (planar triangular) ? tetrahedral ? bent The shape of a two electron group molecule is The shape of a three electron group molecule with two outer atoms and one lone pair is The shape of a four electron group molecule with three outer atoms and one lone pair is

Complete the table. Number of electron groups Bond angle Outer atoms/Lone pairs 2 ? 2/0 3 ? ? bond angle in a two electron group molecule: bond angle in a three electron group molecule: bond angle in a four electron group molecule: 3/0 2/1 4/0 3/1 2/2 Shape ? trigonal planar (planar triangular) ? tetrahedral ? bent The shape of a two electron group molecule is The shape of a three electron group molecule with two outer atoms and one lone pair is The shape of a four electron group molecule with three outer atoms and one lone pair is

Pushing Electrons

4th Edition

ISBN:9781133951889

Author:Weeks, Daniel P.

Publisher:Weeks, Daniel P.

Chapter1: Lewis Structures

Section: Chapter Questions

Problem 34EQ: Chloromethane has the Lewis structure _______________________________ The carbon atom is sharing 4...

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Acrolein is the starting material for certain plastics. (a) Which bonds in the molecule are polar and which are nonpolar? (b) Which is the most polar bond in the molecule? Which atom is the partial negative end of this bond?
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.
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.
For each of the following molecules, complete the Lewis structure and use the VSEPR model to determine the bond angles around each central atom. Note that the drawings are only skeleton structures and may depict the angles incorrectly.
Fill in the blanks in each line of the following table that involves characteristics of various bonds between nonmetals. The first line is already completed as an example.
Predict the molecular structure and bond angles for each molecule or ion in Exercises 81 and 87 from Chapter 3
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Vitamin B6 is an organic compound whose deficiency in the human body can cause apathy, irritability, and an increased susceptibility to infections. Below is an incomplete Lewis structure for vitamin B6. Complete the Lewis structure and answer the following questions. Hint: Vitamin B6 can be classified as an organic compound (a compound based on carbon atoms). The majority of Lewis structures for simple organic compounds have all atoms with a formal charge of zero. Therefore, add lone pairs and multiple bonds to the structure below to give each atom a formal charge of zero. a. How many bonds and bonds exist in vitamin B6? b. Give approximate values for the bond angles marked a through g in the structure. c. How many carbon atoms are sp2 hybridized? d. How many carbon, oxygen, and nitrogen atoms are sp3 hybridized? e. Does vitamin B6 exhibit delocalized bonding? Explain.
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 ____.
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