Covalent Bonding and Molecular Structure

Flashcards for reviewing key concepts in covalent bonding and molecular structure.

Covalent Bond

A bond formed by the sharing of electrons between nonmetal atoms.

Bond Dissociation Energy (BDE)

The energy required to break a covalent bond; larger BDE indicates a stronger bond.

Single Bond

A covalent bond involving one shared pair of electrons.

Double Bond

A covalent bond involving two shared pairs of electrons.

Triple Bond

A covalent bond involving three shared pairs of electrons.

Intermolecular Forces (IMF)

Attractions between molecules that are much weaker than covalent bonds.

Molecular Formula (MF)

A formula that shows the actual count of each element in a molecular compound.

Empirical Formula (EF)

A formula representing the simplest whole number ratio of elements in a compound.

Octet Rule

A rule stating that atoms tend to form bonds until they are surrounded by eight valence electrons.

Lewis Dot Diagram

A diagram that shows the bonding between atoms and the lone pairs of electrons in a molecule.

Coordinate Covalent Bond

A bond where one atom contributes both electrons to a shared pair.

Resonance

A phenomenon in which a molecule can be represented by two or more valid Lewis structures.

Valence Shell Electron Pair Repulsion (VSEPR) Theory

A theory used to predict the 3D shape of molecules based on the repulsion between electron pairs.

Polarity of Bonds

Determined by the electronegativity difference between bonded atoms, affecting how equally electrons are shared.

Hydrogen Bond

A strong type of dipole-dipole attraction occurring between molecules that have hydrogen bonded to highly electronegative atoms.

Isomers

Compounds that have the same molecular formula but different arrangements of atoms.

Intra molecular Bonds

Bonds that occur within a molecule.

Intermolecular Attractions

Forces that occur between molecules.

London Dispersion Forces (LDF)

Weak intermolecular forces arising from temporary dipoles in atoms or molecules.