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Calculate the formal charge on each of the oxygen (O) atoms labeled a, b, and c in the following Lewis structure.
Express your answers as integers separated by commas

To calculate the formal charge on each oxygen atom in the given Lewis structure, we use the formal charge formula:

\[
\text{Formal Charge} = \text{Valence electrons} - (\text{Non-bonding electrons} + \frac{1}{2} \times \text{Bonding electrons})
\]

### Step-by-step Calculation:

1. **Oxygen atom \( a \):**
   - Valence electrons for oxygen = 6
   - Non-bonding electrons on oxygen \( a \) = 6 (three lone pairs)
   - Bonding electrons (shared with chlorine) = 2 (one single bond)
   
   \[
   \text{Formal Charge of \( a \)} = 6 - (6 + \frac{1}{2} \times 2) = 6 - (6 + 1) = -1
   \]

2. **Oxygen atom \( b \):**
   - Valence electrons for oxygen = 6
   - Non-bonding electrons on oxygen \( b \) = 4 (two lone pairs)
   - Bonding electrons (shared with chlorine) = 4 (two double bonds)
   
   \[
   \text{Formal Charge of \( b \)} = 6 - (4 + \frac{1}{2} \times 4) = 6 - (4 + 2) = 0
   \]

3. **Oxygen atom \( c \):**
   - Valence electrons for oxygen = 6
   - Non-bonding electrons on oxygen \( c \) = 6 (three lone pairs)
   - Bonding electrons (shared with chlorine) = 2 (one single bond)
   
   \[
   \text{Formal Charge of \( c \)} = 6 - (6 + \frac{1}{2} \times 2) = 6 - (6 + 1) = -1
   \]

### Formal Charges:

- Oxygen atom \( a \) = -1
- Oxygen atom \( b \) = 0
- Oxygen atom \( c \) = -1

So, the formal charges on the oxygen atoms \( a \), \( b \), and \( c \) are:

\[
-1, 0, -1
\]

Let me know if you'd like further details or clarifications! 

Here are 5 related questions:
1. How does the concept of formal charge help in determining the most stable Lewis structure?
2. What are the general rules to assign formal charges in complex molecules?
3. Why does oxygen atom \( b \) have a formal charge of 0?
4. How do resonance structures affect the formal charges in molecules like this one?
5. Can a formal charge differ across equivalent resonance structures?

**Tip:** Always check the sum of formal charges; it should equal the total charge on the molecule or ion.

Calculate the formal charge on each of the oxygen (O) atoms labeled a, b, and c in the following Lewis structure. Express your answers as integers separated by commas.

Learn how to calculate the formal charge on each oxygen atom in a Lewis structure. This example covers the step-by-step calculation for atoms labeled a, b, and c. Suitable for students in Grades 10-12.

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