We would like to show you a description here but the site won’t allow us. To determine the bond order of the carbon monoxide (CO) molecule, we can follow these steps: - Carbon (C) has 6 electrons, and Oxygen (O) has 8 electrons. - Therefore, the total number of electrons in CO = 6 (from C) + 8 (from O) = 14 electrons. - The bond order of the CO molecule is 3, not 2.5 as stated in the question. --- Hint: The molecular orbital theory helps us find out the bond order on the basis of molecular order diagrams. The Atomic no, of C = 6 and O = 8 Complete answer: The electronic configuration of C is 1 s 2 2 s 2 2 p 2 and that of O + is 1 s 2 2 s 2 2 p 4. Steps for drawing the Molecular Orbital Diagram Since C O is a heteronuclear atom, the atom with more electronegativity will be placed lower in the energy level. So For the 1s degenerate orbital, 2 electrons will go to σ 1 s and 2 electrons ... In short: The bond order of $\ce {CO}$ is not exactly 3 and removing an electron will not increase the bond order to 3.5. In both cases, the observed bond order is probably closer to 2.5, while experiments suggest that the bond is stronger in $\ce {CO+}$.
