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

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

1. O atom = -1

2 H atoms and atoms C = 0

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

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

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

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

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⁻)

formal charge

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adding electron dots as needed

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ionic bonding

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Keywords: formal charge, the valence electron, Lewis structure

the answer is c. nacl

i think tornado but not 100%