Chemical Bonding and Molecular Geometry

These flashcards cover key concepts and terms related to chemical bonding and molecular geometry, including VSEPR theory and various molecular shapes.

Valence Shell Electron Pair Repulsion Theory (VSEPR)

A theory that states electron pairs in the outermost energy level try to get as far apart from each other as possible, determining the shape of the molecule.

Linear Shape

A molecular geometry shape with 2 atoms; Examples include H2 and CO2 with approximate bond angles of ~180˚.

Bent Shape

A molecular geometry with 3 atoms; Example includes H2O, where the central atom can have one or two unshared pairs of electrons, with an approximate bond angle of ~104.5˚.

Trigonal Planar Shape

A molecular geometry with 4 atoms such as CH2O, where the central atom has NO unshared pairs, with an approximate bond angle of ~120˚.

Pyramid Shape

A molecular geometry with 4 atoms like NH3, where the central atom has one unshared pair of electrons, with an approximate bond angle of ~107.5˚.

Tetrahedral Shape

A molecular geometry shape with 5 atoms, example CH4, where the central atom has NO unshared pairs, with an approximate bond angle of ~109.5˚.

Trigonal Bipyramidal Shape

A molecular geometry with 6 atoms, such as PF5; the central atom has NO unshared pairs, with bond angles of ~90˚ and ~120˚.