Draw an alternative Lewis (resonance) structure for the compound given in part (a). Show the unshared pairs and nonzero formal charges in your structure. Don\'t use radicals for CH2OH

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16-09-2017
Chemistry

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Draw an alternative Lewis (resonance) structure for the compound given in part (a). Show the unshared pairs and nonzero formal charges in your structure. Don\'t use radicals for CH2OH

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meerkat18 meerkat18 · Answer 1 · 2017-09-25T13:13:47+02:00

1. The Lewis structure for CH₃O⁻ or methoxide ion is shown in the picture attached. Each single bond is composed of 2 bonding electrons. The electron dots are lone electrons are the nonbonding electrons.

2. The unshaired pairs are the electrons dots surrounding the oxygen atom. From the picture, there are 3 unpaired electrons or lone pairs.

3. The formal charge of each element has the following equation:
Formal charge = Valence electrons - Nonbonding electrons - (Bonding electrons/2)

C: 4 - 0 - (8/2) = 0
O: 6 - 6 - (2/2) = -1
H: 1 - 0 - (2/2) = 0

Therefore, the nonzero formal charge is -1 for the oxygen atom.

ardni313 ardni313 · Answer 2 · 2019-08-17T03:35:51+02:00

The formal charges of the atoms involved in the CH₃O- the molecule is:

1. O atom = -1

2 H atoms and atoms C = 0

Further explanation

Formal charges are usually used to explain the bonding of the Lewis structure. The structural form of a molecule can have several types based on the Lewis structure. Formal charge calculations can determine which molecule is more stable, by choosing the smallest charge, even though atoms such as C, N, and O the priority is to fulfill the octet rule first.

Formal charges can be formulated:

FC (formal charge) = number of valence electrons - number of free electrons - 1/2 binding electrons

The formal charge on the atoms involved in the CH₃O⁻ the molecule is

1. atom C

formal charge: 4 - 0 - 1 / 2.8 = 0

2. atom O

formal charge: 6-6--1 / 2.2 = -1

(there is 1 electron from the outside which is added to the O atom)

3. atom H

formal charge: 1-0-1 / 2.2 = 0

So that the total formal charge = 0 + -1 + 0 = -1 (corresponding to the molecular charge of CH₃O⁻)

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Keywords: formal charge, the valence electron, Lewis structure