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

percent abundance for cu-63 can be shown as:

63 x + 65 (1-x) = 62.9296

65 - 62.9296 = 2 x

x = 1.035

thus, percent abundance for cu-63 is 1.035

percent abundance for cu-65 can be shown as:

63 x + 65 (1-x) = 64.9278

65 - 64.9278 = 2 x

x = 0.0361

thus, percent abundance for cu-63 is 0.0361

the mass spectrum of cu-63 showing the intense peak as, this isotope is found in nature more abundantly around 92.38 % in comparison to cu-65 which is found 62.58 % naturally