Question

The carbon-oxygen bond in CO has a higher bond dissociation enthalpy than a carbon-oxygen bond in CO2. Which is the best explanation for this difference? Group of answer choices CO has a triple bond while each carbon-oxygen bond in CO2 is a double bond. CO has a lone pair on carbon while CO2 does not. CO is a polar molecule while CO2 is a nonpolar molecule. CO contains one carbon-oxygen bond while CO2 contains two carbon-oxygen bonds.

Answer 1

CO HAS A TRIPLE BOND WHILE C-O BOND IN CO2 IS A DOUBLE BOND

CO HAS A LONE PAIR ON CARBON WHILE CO2 DOES NOT

Step-by-step explanation:

Bond dissociation bond enthalpy or energy is the energy needed to break 1 mole of a divalent molecule into separate atoms mostly in the gaseous state.

The carbon and oxygen in carbon monoxide form a triple bond as carbon monoxide has 10 electrons in their outermost shell which results into six shared electrons in 3 bonding orbitals as against the double bond formed by other carbon compounds. Four electrons come from oxygen and the remaining two from carbon and due to this, two electrons from oxygen will occupy one orbital and this forms a dative bond. Also because of the triple bond, carbon monoxide is often regarded as a more stable compound than carbon dioxide with a double bond. This gives it its higher bond dissociation enthalpy value and more energy is needed to break it into its separate atoms. This is in conjunction with a larger bond length similar to the bong length in a triple bond. This makes it more stronger than the bond dissociation enthalpy of carbon dioxide having a double bond.