Use the drawing of MO energy diagram for CO to predict the bond order.
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To predict the bond order using the molecular orbital (MO) energy diagram for CO, you can follow these steps:
1. Draw the molecular orbital energy diagram for CO by filling in the atomic orbitals according to the Aufbau principle. The diagram will consist of the atomic orbitals of carbon (C) and oxygen (O) and the corresponding molecular orbitals.
2. Start by drawing the atomic orbitals for carbon and oxygen. Carbon has the electronic configuration of 1s^2 2s^2 2p^2, while oxygen has the electronic configuration of 1s^2 2s^2 2p^4.
3. Combine the atomic orbitals to form molecular orbitals. The bonding molecular orbitals (σ MOs) are formed by adding the corresponding atomic orbitals, while the antibonding molecular orbitals (σ* MOs) are formed by subtracting the corresponding atomic orbitals.
4. Fill the molecular orbitals with electrons according to the Pauli exclusion principle and Hund's rule. Start with the lowest-energy orbital and continue filling up until reaching the total number of valence electrons for the molecule.
5. Calculate the bond order by subtracting the number of electrons in the antibonding orbitals from the number of electrons in the bonding orbitals, and then dividing by 2. The bond order represents the stability of the molecule and indicates the strength of the bond.
In the case of CO, the molecular orbital diagram should show that two electrons occupy the σ bonding orbital, and there are two electrons in the σ* antibonding orbital. The bond order is calculated as follows:
Bond order = (number of bonding electrons - number of antibonding electrons) / 2
In this case, the bond order will be:
Bond order = (2 - 2) / 2 = 0
Hence, the bond order of CO is zero. A bond order of zero indicates that there is no net bonding between the carbon and oxygen atoms.