How do you calculate formal charge of CO?

Answer 1

The formal charge of carbon monoxide gas is #"ZERO"#.

In some representations, we depict charge separation in the carbon monoxide molecule: #""^(-):C-=O^+#, and of course, here, the formal charge of the #"molecule"# is still zero. I tend to like this representation because it suggests that carbon monoxide binds thru the carbon nucleus, which is what is typically observed.

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Answer 2

Xavier Avery

To calculate the formal charge of CO:

[ \text{Formal Charge} = \text{Valence Electrons} - \frac{1}{2}(\text{Bonding Electrons}) - \text{Unshared Electrons} ]

For CO (( \text{Carbon Monoxide} )):

Carbon has 4 valence electrons.
Oxygen has 6 valence electrons.

The Lewis structure of CO involves a triple bond between C and O.

[ \text{Formal Charge of C} = 4 - \frac{1}{2}(6) - 0 = 1 ]

[ \text{Formal Charge of O} = 6 - \frac{1}{2}(6) - 0 = -1 ]

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.