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For each of the following structures,1. Draw a Lewis

Organic Chemistry | 8th Edition | ISBN: 9780321768414 | Authors: L.G. Wade Jr ISBN: 9780321768414 33

Solution for problem 34SP Chapter 1

Organic Chemistry | 8th Edition

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Organic Chemistry | 8th Edition | ISBN: 9780321768414 | Authors: L.G. Wade Jr

Organic Chemistry | 8th Edition

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Problem 34SP

For each of the following structures,

1. Draw a Lewis structure; fill in any nonbonding electrons.

2. Calculate the formal charge on each atom other than hydrogen. All are electrically neutral except as noted.

Step-by-Step Solution:

Solution 34SP :

Step 1:

Here, we have to draw a Lewis structure and fill in any nonbonding electrons and also calculate the formal charge on each atom other than hydrogen.

Formal charge is calculated using the formula :

        Formal charge = Valence electrons - Nonbonding electrons -

It is also calculated using a shortcut formula :

        Formal charge = Valence electrons - (Number of bonds + Number of dots)

Step 2:

The given compound is Diazomethane(CH2N2). This compound has resonance forms. The lewis structure and the formal charge of the atoms are as shown below :

Now, let’s calculate the formal charge for the atoms in the 1st structure :

Formal charge = Valence electrons - ( Number of bonds + Number of dots)

Now, let’s calculate the formal charge for C :

        C = 4 - (4 + 0)= 0

Now, let’s calculate the formal charge for 1st N atom :

        N = 5 - (4 + 0) = +1

Thus 1st nitrogen atom in the chain has formal charge of +1 and it is represented in the diagram above.

Now, let’s calculate the formal charge for 2nd N atom :

N = 5 - (2 + 4 ) = -1.    

Hence, 2nd nitrogen atom in the chain has formal charge of -1 and it is represented in the diagram above.

Now, let’s calculate the formal charge for the atoms in the 2nd structure :

Formal charge = Valence electrons - ( Number of bonds + Number of dots)

Now, let’s calculate the formal charge for C :

        C = 4 - (3 + 2)= -1

Thus carbon atom in the chain has formal charge of -1 and it is represented in the diagram above.

Now, let’s calculate the formal charge for 1st N atom :

        N = 5 - (4 + 0) = +1

Thus 1st nitrogen atom in the chain has formal charge of +1 and it is represented in the diagram above.

Now, let’s calculate the formal charge for 2nd N atom :

N = 5 - (3 + 2 ) = 0.    

Step 3 :

The lewis structure and the formal charge of the atoms are as shown below :

Now, let’s calculate the formal charge for the atoms here :

Formal charge = Valence electrons - ( Number of bonds + Number of dots)

Now, let’s calculate the formal charge for  1st C atom :

        C = 4 - (4 + 0)= 0

Now, let’s calculate the formal charge for 2nd C atom :

        C = 4 - (4 + 0) = 0

Now, let’s calculate the formal charge for 3rd C atom :

        C = 4 - (4 + 0) = 0

Now, let’s calculate the formal charge for N atom :

        N = 5 - (4 + 0) = +1

Now, let’s calculate the formal charge for O atom :

O = 6 - (1 + 6 ) = -1.    

Hence, oxygen atom in the chain has formal charge of -1 and it is represented in the diagram above.

Step 4 of 6

Chapter 1, Problem 34SP is Solved
Step 5 of 6

Textbook: Organic Chemistry
Edition: 8
Author: L.G. Wade Jr
ISBN: 9780321768414

This textbook survival guide was created for the textbook: Organic Chemistry, edition: 8. Since the solution to 34SP from 1 chapter was answered, more than 320 students have viewed the full step-by-step answer. Organic Chemistry was written by and is associated to the ISBN: 9780321768414. This full solution covers the following key subjects: any, atom, calculate, Charge, draw. This expansive textbook survival guide covers 25 chapters, and 1336 solutions. The answer to “For each of the following structures,1. Draw a Lewis structure; fill in any nonbonding electrons.2. Calculate the formal charge on each atom other than hydrogen. All are electrically neutral except as noted.” is broken down into a number of easy to follow steps, and 32 words. The full step-by-step solution to problem: 34SP from chapter: 1 was answered by , our top Chemistry solution expert on 05/06/17, 06:41PM.

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