Questions: S = C - O S = C = O S - C = O A B C Formal Charge S C O

S = C - O S = C = O S - C = O A B C Formal Charge S C O
Transcript text: S = C - O S = C = O S - C = O A B C Formal Charge S C O
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Solution

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Solution Steps

Step 1: Understanding Formal Charge Calculation

The formal charge (FC) of an atom in a molecule can be calculated using the formula: \[ \text{FC} = V - (L + \frac{B}{2}) \] where \( V \) is the number of valence electrons in the free atom, \( L \) is the number of lone pair electrons, and \( B \) is the number of bonding electrons.

Step 2: Calculate Formal Charge for Each Atom in Each Structure
Structure A: \( \text{S} = \text{C} - \text{O} \)

  • Sulfur (S):

    • Valence electrons (\( V \)) = 6
    • Lone pairs (\( L \)) = 2
    • Bonding electrons (\( B \)) = 6 (double bond with C) \[ \text{FC}_S = 6 - (2 + \frac{6}{2}) = 6 - 5 = +1 \]

  • Carbon (C):

    • Valence electrons (\( V \)) = 4
    • Lone pairs (\( L \)) = 0
    • Bonding electrons (\( B \)) = 8 (double bond with S and single bond with O) \[ \text{FC}_C = 4 - (0 + \frac{8}{2}) = 4 - 4 = 0 \]

  • Oxygen (O):

    • Valence electrons (\( V \)) = 6
    • Lone pairs (\( L \)) = 6
    • Bonding electrons (\( B \)) = 2 (single bond with C) \[ \text{FC}_O = 6 - (6 + \frac{2}{2}) = 6 - 7 = -1 \]
Structure B: \( \text{S} = \text{C} = \text{O} \)

  • Sulfur (S):

    • Valence electrons (\( V \)) = 6
    • Lone pairs (\( L \)) = 2
    • Bonding electrons (\( B \)) = 4 (double bond with C) \[ \text{FC}_S = 6 - (2 + \frac{4}{2}) = 6 - 4 = +2 \]

  • Carbon (C):

    • Valence electrons (\( V \)) = 4
    • Lone pairs (\( L \)) = 0
    • Bonding electrons (\( B \)) = 8 (double bond with S and double bond with O) \[ \text{FC}_C = 4 - (0 + \frac{8}{2}) = 4 - 4 = 0 \]

  • Oxygen (O):

    • Valence electrons (\( V \)) = 6
    • Lone pairs (\( L \)) = 4
    • Bonding electrons (\( B \)) = 4 (double bond with C) \[ \text{FC}_O = 6 - (4 + \frac{4}{2}) = 6 - 6 = 0 \]
Structure C: \( \text{S} - \text{C} = \text{O} \)

  • Sulfur (S):

    • Valence electrons (\( V \)) = 6
    • Lone pairs (\( L \)) = 6
    • Bonding electrons (\( B \)) = 2 (single bond with C) \[ \text{FC}_S = 6 - (6 + \frac{2}{2}) = 6 - 7 = -1 \]

  • Carbon (C):

    • Valence electrons (\( V \)) = 4
    • Lone pairs (\( L \)) = 0
    • Bonding electrons (\( B \)) = 8 (single bond with S and double bond with O) \[ \text{FC}_C = 4 - (0 + \frac{8}{2}) = 4 - 4 = 0 \]

  • Oxygen (O):

    • Valence electrons (\( V \)) = 6
    • Lone pairs (\( L \)) = 4
    • Bonding electrons (\( B \)) = 4 (double bond with C) \[ \text{FC}_O = 6 - (4 + \frac{4}{2}) = 6 - 6 = 0 \]

Final Answer

  • Structure A:

    • \( \text{FC}_S = +1 \)
    • \( \text{FC}_C = 0 \)
    • \( \text{FC}_O = -1 \) \[ \boxed{\text{Structure A: } \text{FC}_S = +1, \text{FC}_C = 0, \text{FC}_O = -1} \]

  • Structure B:

    • \( \text{FC}_S = +2 \)
    • \( \text{FC}_C = 0 \)
    • \( \text{FC}_O = 0 \) \[ \boxed{\text{Structure B: } \text{FC}_S = +2, \text{FC}_C = 0, \text{FC}_O = 0} \]

  • Structure C:

    • \( \text{FC}_S = -1 \)
    • \( \text{FC}_C = 0 \)
    • \( \text{FC}_O = 0 \) \[ \boxed{\text{Structure C: } \text{FC}_S = -1, \text{FC}_C = 0, \text{FC}_O = 0} \]
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