key term - Bonding molecular orbitals

Definition

Bonding molecular orbitals are formed when atomic orbitals combine constructively, leading to a region of increased electron density between two nuclei. This increase in electron density stabilizes the molecule, allowing it to form a bond. The presence of bonding molecular orbitals is crucial in understanding the stability and characteristics of both simple diatomic molecules and more complex coordination compounds.

5 Must Know Facts For Your Next Test

1. Bonding molecular orbitals are lower in energy than the atomic orbitals from which they are formed, leading to increased stability for the molecule.
2. In diatomic molecules, such as H$_2$ or O$_2$, bonding molecular orbitals result from the combination of s or p orbitals from each atom.
3. The occupancy of bonding molecular orbitals contributes to the bond order; higher occupancy indicates stronger bonds.
4. In coordination compounds, bonding molecular orbitals can arise from interactions between metal d-orbitals and ligand p-orbitals or other atomic orbitals.
5. The concept of bonding molecular orbitals is essential for predicting magnetic properties; molecules with unpaired electrons in these orbitals exhibit paramagnetism.

Review Questions

• How do bonding molecular orbitals differ from anti-bonding molecular orbitals in terms of energy and stability?
  • Bonding molecular orbitals are lower in energy compared to anti-bonding molecular orbitals, which makes them more stable. When atomic orbitals combine constructively to form bonding molecular orbitals, they create regions of high electron density between nuclei, leading to attractive forces that stabilize the bond. In contrast, anti-bonding molecular orbitals, formed through destructive combination, decrease electron density between nuclei, resulting in repulsion and reduced stability.
• Discuss the significance of bonding molecular orbitals in determining the properties of coordination compounds.
  • Bonding molecular orbitals play a crucial role in coordination compounds by influencing their geometry, stability, and reactivity. The interaction between metal d-orbitals and ligand atomic orbitals forms new bonding molecular orbitals that contribute to the overall electron distribution in the complex. This electron configuration directly affects properties such as color, magnetism, and coordination number, making bonding molecular orbitals essential for understanding coordination chemistry.
• Evaluate how the concept of bond order, derived from bonding molecular orbitals, affects predictions about molecule stability and reactivity.
  • The bond order calculated from bonding molecular orbitals indicates the number of bonds between two atoms; it is defined as half the difference between the number of electrons in bonding and anti-bonding molecular orbitals. A higher bond order suggests stronger bonds and greater stability for molecules. Conversely, a low or zero bond order can indicate weak or non-existent bonds, influencing reactivity. This relationship helps predict how molecules will behave under various conditions, making it a fundamental concept in understanding chemical reactivity.

Related terms

anti-bonding molecular orbitals: Anti-bonding molecular orbitals are created when atomic orbitals combine destructively, resulting in a decrease in electron density between nuclei and destabilizing the bond.

hybridization: Hybridization is the process where atomic orbitals mix to form new hybrid orbitals, which can help explain molecular geometry and bonding in compounds.

ligand field theory:

Ligand field theory describes the interactions between ligands and metal ions in coordination complexes, focusing on the splitting of d-orbitals and the role of bonding molecular orbitals.