# How do you draw the Lewis structures of carbon dioxide and carbon monoxide?

$O = C = O$, and ""^+O-=C^-
For carbon dioxide there are $6 + 6 + 4 = 16 \text{ valence electrons}$, i.e. 8 electron pairs. There are 2 lone pairs around each oxygen atom, and with the 8 electrons involved in the double bonds, this accounts for the 16 electrons.
For carbon monoxide, there are $6 + 4 = 10 \text{ valence electrons}$. A representation of ""^+:O-=C:^- is typical. This involves formal charge separation, but inorganic chemists tend to like this representation in that carbon monoxide typically coordinates thru the carbon.