Chapter 6: Chemical Bonding II - Valence Bond and Molecular Orbital Theory

Set of flashcards on the key concepts and vocabulary related to Chapter 6 on Chemical Bonding, focusing on Valence Bond and Molecular Orbital Theory.

Bonding Electron Pairs

Pairs of electrons that are shared between two atoms in a chemical bond.

Nonbonding Electron Pairs

Pairs of valence electrons that are not involved in bonding.

Valence Bond Theory

A theory that explains how atomic orbitals overlap to form chemical bonds.

Paramagnetic

A property of materials that have unpaired electrons and are attracted to magnetic fields.

Lewis Theory

A model that uses Lewis structures to represent molecules and predict their properties, but is limited in accuracy.

Hybridization

The mixing of atomic orbitals to create new hybrid orbitals suitable for bonding.

Sigma (σ) Bond

A type of bond formed when orbitals overlap along the internuclear axis.

Pi (π) Bond

A type of bond formed when orbitals overlap side-by-side, resulting in less strength than sigma bonds.

Molecular Orbital Theory

A theory that considers electrons in a molecule to be delocalized, belonging to the molecule as a whole.

Bond Order

The difference between the number of bonding electrons and antibonding electrons divided by two, indicating bond stability.

Hybrid Orbitals

Orbitals that result from the hybridization of standard atomic orbitals, used to form chemical bonds.

Cis and Trans Isomers

Isomers that differ in the arrangement of groups around a double bond, affecting properties.

Delocalization

The phenomenon of electrons being shared over multiple atoms, as described in molecular orbital theory.

Antibonding Orbital

Molecular orbitals that have higher energy than bonding orbitals and can destabilize a bond.

Linear Combination of Atomic Orbitals (LCAO)

A method in molecular orbital theory where atomic orbitals combine to form molecular orbitals.

Quantum Mechanics

The branch of physics that describes the behavior and interactions of energy and matter at very small scales.

Trigonal Planar

A molecular geometry with three bonding pairs arranged at 120° angles.

Tetrahydral Geometry

A molecular shape where a central atom is surrounded by four bonds, resulting in bond angles of approximately 109.5°.

VSEPR Theory

A model used to predict the geometry of molecules based on electron pair repulsion.

Molecular Orbital Energy Diagram

A graphical representation of the energies of molecular orbitals in a molecule.

Lewis Structure

A diagram representing the valence electrons of atoms within a molecule, showing how they are arranged among the atoms.

Electronegativity

The tendency of an atom to attract electrons in a chemical bond.