Answer
See the explanation
Work Step by Step
To answer this question, we need to write the electron configurations for CO and O2 using the molecular orbital model, and then identify two property differences between them.
Electron Configuration for CO:
The carbon monoxide (CO) molecule has the following electron configuration:
1s^2 2s^2 2p^2 (C) + 1s^2 2s^2 2p^4 (O)
= 1s^2 2s^2 2p^6
Using the molecular orbital model, the electron configuration of CO can be represented as:
1σ^2 2σ^2 3σ^2 1π^4 2π^2
Electron Configuration for O2:
The oxygen (O2) molecule has the following electron configuration:
1s^2 2s^2 2p^4 (O) + 1s^2 2s^2 2p^4 (O)
= 1s^2 2s^2 2p^8
Using the molecular orbital model, the electron configuration of O2 can be represented as:
1σ^2 2σ^2 3σ^2 1π^4 2π^2 3σ^2
Two Property Differences between CO and O2:
1. Bond Order:
- The bond order of CO is 3, as it has one sigma (σ) bond and two pi (π) bonds.
- The bond order of O2 is 2, as it has one sigma (σ) bond and one pi (π) bond.
2. Magnetic Properties:
- CO is a diamagnetic molecule, as it has no unpaired electrons.
- O2 is a paramagnetic molecule, as it has two unpaired electrons in its 2π molecular orbitals.
These differences in bond order and magnetic properties lead to other differences in the properties and behavior of CO and O2 molecules.
