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Draw the Lewis structure of [tex](HCONCH_3)[/tex] and calculate the formal charge of nitrogen (N) and oxygen (O). (4 points)

Draw the Lewis structure of [tex](CH_3NO_2)[/tex] and calculate the formal charge of nitrogen (N) and oxygen (O). (4 points)

Draw resonance forms and the hybrid structure of the molecule below. (4 points)

Answer :

The Lewis structures and formal charges of (HCONCH3) and CH_NO2 have been calculated. The resonance forms and hybrid structure of a given structure are also provided.

The Lewis structure of (HCONCH3) has the following arrangement:

H

|

H-C

|

H-N-CH3

|

H

The formal charge of N in this structure can be calculated using the formula:

Formal charge = Group number - (Unshared electrons + (1/2)×Shared electrons)

For N, the calculation would be:

Formal charge = 5 - (2 + (1/2)×6) = 0

The formal charge of N is 0. The formal charge of I cannot be determined as there is no I in the given structure.

Similarly, the Lewis structure of CH_NO2 can be represented as:

H

|

C-N-O

|

The formal charge of N can be calculated as:

Formal charge = 5 - (2 + (1/2)×6) = 0

The formal charge of O can be calculated as:

Formal charge = 6 - (2 + (1/2)×6) = 0

The resonance forms and hybrid structure of the given structure can be shown as:

H H O

| | |

C–N–O

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