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Found in: Page 17

### Organic Chemistry

Book edition 5th
Author(s) Janice Gorzynski Smith
Pages 1256 pages
ISBN 9780078021558

# Question: Calculate the formal charge on each second-row atoma. b. c.

a. +1

b. 0, +1, -1 (from left to right)

c. 0, +1, -1 (from left to right)

See the step by step solution

## Step-by-Step Solution Step 1:  Determination of formal charge

The formal charge is determined using the given formula:

## Step 2: Calculation of formal charge

a. The formal charge of N (second-row element) is calculated as follows:

• The total count of valence electrons of nitrogen is five.
• The number of lone pair of electrons is 0.
• The total count of bonding pair electrons is eight as all the electrons of nitrogen are used.

Therefore, the formal charge of N is +1.

b. The formal charge of C (methyl carbon) is calculated as follows:

• The total number of valence electrons of C is four.
• The number of lone pair of electrons is 0.
• The total number of bonding pair electrons is eight as all the electrons of N are used.

Therefore, the formal charge of C is -1.

c. The formal charge of O (extreme left) is calculated as follows:

• The total valence electrons of O are six.
• The number of lone pairs of electrons is four.
• The total number of bonding pair electrons is four as all the electrons of O are used.

Therefore, the formal charge of O is 0.

c. The formal charge of O (middle) is calculated as follows:

• The total valence electrons of O are six.
• The number of lone pairs of electrons is two.

The total number of bonding pair electrons is six as all the electrons of O are used

Therefore, the formal charge of O is +1.

d. The formal charge of O (extreme right) is calculated as follows:

• The total valence electrons of O are six.
• The number of lone pairs of electrons is six.
• The total number of bonding pair electrons is two as all the electrons of O are used.

Therefore, the formal charge of O is -1.