Write the molecular orbital configurationsof O2 and–22O . Also calculate their bondorders

To determine the molecular orbital configurations of O2 and O2^2-, we need to follow these steps:

Step 1: Write the electron configuration of the oxygen atom (O).

The electron configuration of oxygen (O) is 1s^2 2s^2 2p^4.

Step 2: Determine the total number of valence electrons.

Oxygen has 6 valence electrons.

Step 3: Construct the molecular orbital diagram for O2.

In the molecular orbital diagram, we start by filling the lower energy orbitals first and then move to higher energy orbitals. The molecular orbital diagram for O2 is as follows:

σ2s* (antibonding) σ2s (bonding) σ2p* (antibonding) π2p* (antibonding) π2p (bonding) σ2p* (antibonding) σ2p (bonding)

Step 4: Fill the molecular orbitals with the valence electrons.

Oxygen has 6 valence electrons, so we fill the molecular orbitals starting from the lowest energy level. The electron configuration for O2 is:

σ2s* (2 electrons) σ2s (2 electrons) σ2p* (2 electrons) π2p* (0 electrons) π2p (0 electrons) σ2p* (0 electrons) σ2p (0 electrons)

Step 5: Calculate the bond order.

The bond order is calculated by subtracting the number of antibonding electrons from the number of bonding electrons and dividing the result by 2.

For O2, the bond order is:

Bond order = (Number of bonding electrons - Number of antibonding electrons) / 2 = (4 - 2) / 2 = 2 / 2 = 1

For O2^2-, the bond order is:

Bond order = (Number of bonding electrons - Number of antibonding electrons) / 2 = (4 - 4) / 2 = 0 / 2 = 0

So, the bond order for O2 is 1, indicating a single bond, and the bond order for O2^2- is 0, indicating no bond.