Lewis Structures and Molecular Geometry

These flashcards cover key concepts related to Lewis structures, molecular geometry, and bonding relevant to organic chemistry.

Molecular formula

A notation that shows the type and number of atoms in a molecule.

Lone pair

A pair of valence electrons that are not shared with another atom.

Pi bond

A bond that results from the side-to-side overlap of p orbitals.

VSEPR theory

A model used to predict the geometry of individual molecules based on the repulsion between the electron pairs surrounding the central atom.

Formal charge

The charge assigned to an atom in a molecule, calculated by comparing the number of valence electrons with the number of electrons assigned to the atom in the Lewis structure.

Octet rule

The principle that atoms tend to form bonds until they are surrounded by eight valence electrons.

Trigonal bipyramidal geometry

A molecular shape with five bonded atoms around a central atom, with two axial and three equatorial positions.

Equatorial position

In a trigonal bipyramidal structure, positions that minimize lone pair-bond pair repulsion.

Valence electrons

The electrons in the outermost shell of an atom that can participate in forming bonds.

Electron-pair geometry

The spatial arrangement of all electron pairs (bonding and lone pairs) around a central atom.