Covalent Bonding and Molecular Geometry

These flashcards cover key concepts related to covalent bonding, molecular geometry, and intermolecular forces (IMFs) that are essential for understanding molecular interactions and properties.

Covalent Bond

A bond formed when two atoms share electrons due to similar electronegativity.

Electronegativity (EN)

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

Polar Covalent Bond

A bond where one atom is more electronegative, creating partial charges.

Nonpolar Covalent Bond

A bond where atoms share electrons equally.

Single Bond

A covalent bond where two electrons are shared; longest and weakest.

Double Bond

A covalent bond where four electrons are shared.

Triple Bond

A covalent bond where six electrons are shared; shortest and strongest.

VSEPR Theory

A model used to determine the 3D shape of molecules based on electron repulsion.

Lewis Structure

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

Bonding Domain

A region in a molecule occupied by bonded electron pairs.

Lone Pair

A pair of valence electrons that are not shared between atoms.

Polar Molecule

A molecule that has a net dipole moment due to the presence of polar bonds.

Intermolecular Forces (IMFs)

Forces of attraction between molecules; determine physical properties.

Hydrogen Bonding

A strong type of intermolecular force occurring between molecules containing H bonded to F, O, or N.

Dipole-Dipole Interaction

An intermolecular force occurring between polar molecules.

London Dispersion Forces (LDF)

The weakest intermolecular force, present in all molecules, especially nonpolar.

Binary Covalent Compound

A compound formed from two different nonmetals.

Naming Acids

Rules for naming acids based on the presence of oxygen and the type of ions involved.

Molecular Geometry

The three-dimensional arrangement of atoms in a molecule.