CHEMISTRY · Single correct · A Level · Chemistry · Bonding · Bonding
Problem
Consider two possible Lewis structures for CO2.
Structure A: O=C=O with each oxygen bearing two lone pairs.
Structure B: −O–C≡O+ where the left oxygen is single-bonded to carbon, the right oxygen is triple-bonded, and all atoms possess an octet.
Which choice correctly identifies the more plausible structure and the primary reason?
(a) Structure B, because all atoms satisfy the octet rule.
(b) Structure A, because all formal charges are zero.
(c) Structure B, because it places the negative charge on the more electronegative oxygen atom.
(d) Structure A, because carbon cannot form more than four bonds.