To determine the formal charges of each atom in the structure [tex]\(O=C=O\)[/tex], we should use the formal charge formula:
[tex]\[ \text{Formal charge} = \text{valence electrons} - \text{non-bonding electrons} - \frac{\text{bonding electrons}}{2} \][/tex]
Let's analyze each atom in the molecule:
### Carbon Atom (C)
1. Valence Electrons:
- Carbon has 4 valence electrons.
2. Non-bonding Electrons:
- Carbon has no lone pairs.
3. Bonding Electrons:
- Carbon is involved in two double bonds, so it shares a total of 4 pairs of electrons (8 bonding electrons).
Applying the formal charge formula for Carbon:
[tex]\[ \text{Formal charge of C} = 4 - 0 - \frac{8}{2} = 4 - 4 = 0 \][/tex]
### Each Oxygen Atom (O)
Each oxygen in the structure is doubly bonded to the carbon atom.
1. Valence Electrons:
- Oxygen has 6 valence electrons.
2. Non-bonding Electrons:
- Each oxygen has two lone pairs, so there are 4 non-bonding electrons.
3. Bonding Electrons:
- Each oxygen is involved in one double bond with the carbon atom, which means 2 pairs of bonding electrons (4 bonding electrons).
Applying the formal charge formula for each Oxygen:
[tex]\[ \text{Formal charge of O} = 6 - 4 - \frac{4}{2} = 6 - 4 - 2 = 0 \][/tex]
### Summary
So, in the structure [tex]\(O=C=O\)[/tex], the formal charges are:
- The Carbon (C) atom has a formal charge of [tex]\(0\)[/tex].
- Each Oxygen (O) atom has a formal charge of [tex]\(0\)[/tex].
Let's match these calculated charges to the provided options:
- Carbon (C): [tex]\( \boxed{0} \)[/tex]
- Oxygen (O) (both atoms): [tex]\( \boxed{0} \)[/tex]
