Questions: HC==CH / a N N c :O: b=C :O: C6H5

Transcript text: HC==CH / \ a N N c :O: b=C :O: | C_6H_5

Solution

Solution Steps

Step 1: Identify the structure and valence electrons

First, we need to identify the structure and the valence electrons of the atoms labeled a, b, and c. The structure provided is a heterocyclic compound with nitrogen and oxygen atoms.

Step 2: Determine the formal charge formula

The formal charge (FC) can be calculated using the formula: \[ \text{FC} = V - (N + \frac{B}{2}) \] where:

\( V \) is the number of valence electrons in the free atom,
\( N \) is the number of non-bonding (lone pair) electrons,
\( B \) is the number of bonding (shared) electrons.

Step 3: Calculate the formal charge on atom a (Nitrogen)

For nitrogen (N):

Valence electrons (\( V \)) = 5
Non-bonding electrons (\( N \)) = 2 (one lone pair)
Bonding electrons (\( B \)) = 6 (three bonds)

\[ \text{FC}_a = 5 - (2 + \frac{6}{2}) = 5 - (2 + 3) = 5 - 5 = 0 \]

\(\boxed{\text{FC}_a = 0}\)

Step 4: Calculate the formal charge on atom b (Carbon)

For carbon (C):

Valence electrons (\( V \)) = 4
Non-bonding electrons (\( N \)) = 0
Bonding electrons (\( B \)) = 8 (four bonds)

\[ \text{FC}_b = 4 - (0 + \frac{8}{2}) = 4 - (0 + 4) = 4 - 4 = 0 \]

\(\boxed{\text{FC}_b = 0}\)

Step 5: Calculate the formal charge on atom c (Oxygen)

For oxygen (O):

Valence electrons (\( V \)) = 6
Non-bonding electrons (\( N \)) = 4 (two lone pairs)
Bonding electrons (\( B \)) = 4 (two bonds)

\[ \text{FC}_c = 6 - (4 + \frac{4}{2}) = 6 - (4 + 2) = 6 - 6 = 0 \]

\(\boxed{\text{FC}_c = 0}\)

Final Answer

\[ \boxed{\text{FC}_a = 0} \] \[ \boxed{\text{FC}_b = 0} \] \[ \boxed{\text{FC}_c = 0} \]

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