To determine the formal charge of each atom in the structure [tex]\( \ddot{O}=C= \ddot{O} \)[/tex], we will follow these steps:
1. Identify the number of valence electrons for each atom:
- Carbon (C) has 4 valence electrons.
- Oxygen (O) has 6 valence electrons.
2. Determine the bonding and non-bonding electrons in the structure:
- For the carbon atom in the center:
- It forms two double bonds with the two oxygen atoms.
- This means it is involved in 4 bonding pairs of electrons but has no lone pairs.
- For each oxygen atom:
- Each oxygen forms one double bond with the carbon atom.
- This means each oxygen is involved in 2 bonding pairs (4 bonding electrons).
- Each oxygen also has 2 lone pairs of electrons (4 non-bonding electrons).
3. Use the formal charge formula:
[tex]\[
\text{Formal Charge} = \text{Valence Electrons} - \text{Non-bonding Electrons} - \frac{\text{Bonding Electrons}}{2}
\][/tex]
4. Apply the formal charge formula for each atom:
- For the carbon atom (C):
[tex]\[
\text{Formal Charge of C} = 4 - 0 - \frac{8}{2} = 4 - 0 - 4 = 0
\][/tex]
- For each oxygen atom (O):
[tex]\[
\text{Formal Charge of O} = 6 - 4 - \frac{4}{2} = 6 - 4 - 2 = 0
\][/tex]
Based on these formal charge calculations:
- The formal charge of the central carbon atom (C) is [tex]\(0\)[/tex].
- The formal charge of each oxygen atom (O) is [tex]\(0\)[/tex].
Thus, the correct sentence completions are:
- The formal charge of the carbon atom in the structure [tex]\( \ddot{O}=C= \ddot{O} \)[/tex] is [tex]\(0\)[/tex].
- The formal charge of each oxygen atom in the structure [tex]\( \ddot{O}=C= \ddot{O} \)[/tex] is [tex]\(0\)[/tex].
