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? Place the species in order of increasing bond length and bond energy. a. $\mathrm{CN}^{+}$ b. $\mathrm{CN}$ c. $\mathrm{CN}^{-}$

Using the molecular orbital model, write electron configurations for the following diatomic species and calculate the bond orders. Which ones are paramagnetic? Place the species in order of increasing bond length and bond energy.
a. $\mathrm{CN}^{+}$
b. $\mathrm{CN}$
c. $\mathrm{CN}^{-}$

Key Concepts

Molecular Orbital Theory

Molecular Orbital Theory explains how atomic orbitals combine to form molecular orbitals that extend over the entire molecule. This framework allows the prediction of electron distributions, bonding interactions, and the overall stability of a molecule by considering both bonding and antibonding orbitals.

Electron Configuration in Molecular Orbitals

When using Molecular Orbital Theory, electron configuration involves filling the molecular orbitals in order of increasing energy. Electrons fill lower-energy bonding orbitals before occupying higher-energy antibonding orbitals, following fundamental principles such as the Pauli Exclusion Principle and Hund’s Rule.

Bond Order

Bond order is calculated using the formula (number of electrons in bonding orbitals minus the number in antibonding orbitals) divided by two. It serves as a quantitative measure of bond strength and stability; higher bond orders indicate stronger, shorter bonds, while lower bond orders imply weaker, longer bonds.

Paramagnetism

Paramagnetism in molecules arises when there are unpaired electrons in the molecular orbitals. The presence of these unpaired electrons results in the molecule being attracted to a magnetic field, a key property that can be predicted using the electron configuration in the MO model.

Relationship Between Bond Length and Bond Energy

Bond length and bond energy are inversely related properties; typically, as bond order increases, the bond becomes shorter and the bond energy higher, indicating a stronger bond. This relationship helps in comparing the physical characteristics of molecules with different electron configurations.

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