Molecular Orbital Theory

These flashcards cover the key concepts of Molecular Orbital Theory, including bond order, bond length, bond strength, and magnetic properties.

Molecular Orbital Theory

A theory that describes the combination of atomic orbitals to form molecular orbitals, which can predict molecular properties.

Bond Order (BO)

The difference between the number of bonding electrons and the number of antibonding electrons, indicating the strength and stability of a bond.

Bond Length (BL)

The average distance between the nuclei of two bonded atoms; typically decreases with increasing bond order.

Bond Strength (BS)

The amount of energy required to break a bond; generally increases with higher bond order.

Magnetic Properties

Characteristics of a molecule that determine its response to a magnetic field, classified as paramagnetic (unpaired electrons present) or diamagnetic (all electrons paired).

Bond Order Formula

Calculated as (number of bonding electrons) - (number of antibonding electrons); used to assess bond strength.

Paramagnetic

A property of substances that have unpaired electrons and are attracted to a magnetic field.

Diamagnetic

A property of substances that have all paired electrons and are not attracted to a magnetic field.

Examples of Molecular Orbitals

Diagrams that represent how atomic orbitals combine, such as H-H (single bond), N-N (double bond), and triple bonds.

Energy Levels in Molecular Orbitals

The arrangement of electrons in molecular orbitals reflects their energy; higher energy corresponds to higher bond order.