In a neutral compound, what does the number of bonds formed by an oxygen atom typically indicate?

• A. The formal charge of the oxygen atom
• B. The total number of electrons in the molecule
• C. The atomic number of oxygen
• D. The number of lone pairs present on the oxygen atom

Answer: (A)

Verified step by step guidance

1. Recall that oxygen typically has 6 valence electrons and tends to form bonds to complete its octet in neutral compounds.
2. Understand that the number of bonds an oxygen atom forms affects its formal charge, which is calculated by comparing the number of valence electrons in the free atom to the electrons assigned in the molecule.
3. Use the formal charge formula: \(\text{Formal Charge} = \text{Valence Electrons} - (\text{Nonbonding Electrons} + \frac{1}{2} \times \text{Bonding Electrons})\) to see how bonding influences the charge on oxygen.
4. Recognize that the number of bonds does not directly indicate the total number of electrons in the molecule, the atomic number of oxygen, or the number of lone pairs, but it is closely related to the formal charge on the oxygen atom.
5. Conclude that in a neutral compound, the number of bonds formed by oxygen typically indicates its formal charge, helping to understand the distribution of electrons and stability of the molecule.