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Q6.

Expert-verified
Organic Chemistry
Found in: Page 17

Short Answer

Answer

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-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.

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