Lecture 12 – Molecular Geometry and Electronegativity with Lewis Structures

These flashcards cover key concepts and vocabulary from Lecture 12 regarding molecular geometry and electronegativity with Lewis structures.

Lewis Structures

Diagrams that show the bonding between atoms of a molecule and the lone pairs of electrons that may exist.

Molecular Geometry

The three-dimensional arrangement of the atoms that constitute a molecule.

Electronegativity

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

Bond Angle

The angle formed by three adjacent atoms in a molecule.

Polar Covalent Bond

A bond where electrons are attracted more strongly by one atom than by the other.

Non-Polar Covalent Bond

A bond where electrons are attracted equally to two atoms.

Valence-Shell Electron-Pair Repulsion (VSEPR)

A model used to predict the geometry of individual molecules based on the number of electron charge clouds surrounding their central atoms.

Charge Cloud

A region around a central atom in a molecule where electrons are likely to be found.

Ionic Bond

A bond formed by the electrostatic attraction between oppositely charged ions.

Polyatomic Ion

An ion composed of two or more atoms that are covalently bonded and that carries a net charge.