What is the formal charge of carbon in carbon monoxide (CO) when the Lewis structure is drawn with a triple bond between carbon and oxygen?

• A. +1
• B. +2
• C. -1
• D. 0

Answer: (A)

Verified step by step guidance

1. Draw the Lewis structure of carbon monoxide (CO) with a triple bond between carbon and oxygen. This means carbon and oxygen share three pairs of electrons, and each atom has lone pairs to complete their octets.
2. Recall the formula for formal charge: \(\text{Formal Charge} = \text{Valence Electrons} - \text{Nonbonding Electrons} - \frac{1}{2} \times \text{Bonding Electrons}\).
3. Determine the number of valence electrons for carbon, which is 4, since carbon is in group 14 of the periodic table.
4. Count the number of nonbonding (lone pair) electrons on the carbon atom in the Lewis structure. Also, count the number of bonding electrons shared by carbon in the triple bond (each bond has 2 electrons).
5. Substitute these values into the formal charge formula to calculate the formal charge on carbon without simplifying the final number.