Chemical Bonding and Molecular Structure

These flashcards cover key terms and definitions related to chemical bonding, molecular structure, and intermolecular forces.

Lewis Model

A method that emphasizes valence electrons to explain chemical bonding.

Agonist

A molecule that binds to a receptor and activates it.

Antagonist

A molecule that binds to a receptor but does not activate it.

Chemical Bond

A lasting attraction between atoms, ions, or molecules that enables the formation of chemical compounds.

Ionic Bond

A type of bond that involves the transfer of electrons from one atom to another, typically between metals and nonmetals.

Covalent Bond

A bond formed when two atoms share electrons.

Metallic Bond

A bond characterized by a sea of delocalized electrons around metal cations.

Valence Electrons

Electrons in the outermost shell of an atom that are involved in forming bonds.

Octet Rule

Atoms tend to bond in such a way that they each have eight electrons in their valence shell.

Lone Pairs

Pairs of valence electrons that are not involved in bonding.

Polar Covalent Bond

A type of bond where electrons are shared unequally between atoms, resulting in a dipole.

Hybridization

The process of mixing atomic orbitals to form new hybrid orbitals.

Dipole-Dipole Forces

Attractive forces between polar molecules caused by the presence of permanent dipoles.

Hydrogen Bonding

A strong type of intermolecular force that occurs between molecules when hydrogen is covalently bonded to a highly electronegative atom.

Ion-Dipole Forces

Forces that occur between an ion and a polar molecule.

Resonance Structures

Different Lewis structures that represent the same molecule, differing only in the positions of electrons.

Boiling Point

The temperature at which the vapor pressure of a liquid equals the external pressure surrounding the liquid.

Lattice Energy

The energy required to separate one mole of an ionic solid into gaseous ions.

Dynamic Equilibrium

A state of balance in which the rates of two opposing processes are equal.

Dispersion Forces

Weak intermolecular forces resulting from temporary shifts in electron density, also known as London dispersion forces.

Vapor Pressure

The pressure exerted by a vapor in equilibrium with its liquid or solid phase.