Valence Forces: Fundamental Interactions Governing Chemical Bonding

These flashcards cover key concepts related to valence forces and chemical bonding, providing definitions and explanations to aid in exam preparation.

Valence Forces

Attractive interactions between atoms resulting from the sharing or transfer of valence electrons.

Ionic Bonds

Bonds formed through the complete transfer of electrons from one atom to another, typically between metals and nonmetals, resulting in oppositely charged ions.

Covalent Bonds

Chemical bonds formed when two atoms share one or more pairs of electrons.

Metallic Bonds

Bonds where electrons are delocalized and shared across a lattice of metal ions, resulting in properties like electrical conductivity.

Coordinate (Dative) Bonds

A type of covalent bond where both electrons in the bond originate from the same atom.

Electronegativity

A measure of the tendency of an atom to attract a bonding pair of electrons, influencing the polarity of bonds.

Hybridization

The mixing of atomic orbitals to form new hybrid orbitals for bonding, explaining molecular geometry.

VSEPR Theory

A model used to predict the three-dimensional shapes of molecules based on the repulsion between electron pairs.

Resonance

A concept in chemistry where a molecule cannot be represented by a single Lewis structure but is a hybrid of multiple structures.

Intermolecular Forces

Forces that occur between molecules; typically weaker than valence forces, including van der Waals forces.