Molecular Geometry

Flashcards covering key concepts in Molecular Geometry based on VSEPR theory.

VSEPR Theory

Valence Shell Electron Pair Repulsion theory, which states that electron pairs around a central atom will arrange themselves to minimize repulsions.

Linear Geometry

A molecular shape where atoms are arranged in a straight line, typically with bond angles of 180 degrees.

Trigonal Planar Geometry

A molecular shape with three bonded atoms and no lone pairs around the central atom, with bond angles of 120 degrees.

Bent Geometry

A molecular shape that occurs when there are lone pairs on the central atom, causing the bonded atoms to be at an angle less than 120 degrees.

Tetrahedral Geometry

A molecular shape where four atoms are bonded to a central atom, typically with bond angles around 109.5 degrees.

Trigonal Pyramidal Geometry

A molecular shape similar to tetrahedral but with one lone pair, resulting in bond angles less than 109.5 degrees.

Effect of Lone Pairs

Lone pairs of electrons take up more space than bonding pairs, resulting in smaller bond angles due to increased repulsion.