Using the molecular orbital model, write electron...

Using the molecular orbital model, write electron configurations for the following diatomic species and calculate the bond orders. Which ones are paramagnetic?
a. $\mathrm{Li}_{2}$
b. $\mathrm{C}_{2}$
c. $\mathrm{S}_{2}$

Key Concepts

Paramagnetism and Diamagnetism in Molecules

Molecules exhibit paramagnetism when they contain unpaired electrons in their molecular orbitals, which causes them to be attracted to magnetic fields. In contrast, molecules with all electrons paired are diamagnetic and are weakly repelled by magnetic fields. This magnetic behavior can be predicted by analyzing the electron configuration in the molecular orbitals.

Bond Order

Bond order is calculated as half the difference between the number of electrons in bonding orbitals and antibonding orbitals. It quantifies the strength of a bond; a higher bond order indicates a stronger, more stable bond, while a lower bond order suggests a weaker bond.

Molecular Orbital Theory

Molecular orbital theory explains how atomic orbitals combine to form molecular orbitals that are spread over the entire molecule. This framework allows us to analyze bonding and antibonding interactions between electrons, yielding insights into overall molecular stability and electronic configurations.

Electron Configuration in Molecular Orbitals

Determining the electron configuration in molecular orbitals involves placing electrons into molecular orbitals according to their energy levels while adhering to the Pauli exclusion principle and Hund’s rule. This process shows the distribution of electrons between bonding and antibonding orbitals, which is key for assessing molecular properties.

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