Molecular Geometries under VSEPR Theory

Molecular Geometries under VSEPR Theory

• Linear

  • Geometry with 2 bonds and 0 lone pairs of electrons.

• Bent

  • Geometry resulting from 2 bonds with 1 or 2 lone pairs, leading to a non-linear shape.

• Trigonal Planar

  • Features 3 bonds and no lone pairs, creating a flat, triangular structure.

• Trigonal Pyramidal

  • Comprises 3 bonds plus 1 lone pair, resulting in a pyramidal shape with a central atom at the apex.

• Tetrahedral

  • Consists of 4 bonds with no lone pairs, forming a three-dimensional shape resembling a tetrahedron.

• Trigonal Bipyramidal

  • Characterized by 5 bonds and 0 lone pairs, creating a structure with two triangular bases.

• Octahedral

  • Includes 6 bonds and no lone pairs, resulting in a symmetrical octahedral shape.

• Seesaw

  • Contains 4 bonds and 1 lone pair, producing a structure that resembles a seesaw due to differing electron pair repulsion.

• T-shaped

  • Formed by 3 bonds and 2 lone pairs, creating a "T" shaped configuration.

• Square Pyramidal

  • Comprises 5 bonds and 1 lone pair, leading to a square-based pyramid shape.

• Square Planar

  • Consists of 4 bonds and 2 lone pairs, resulting in a flat square geometry.

VSEPR Theory Overview

• VSEPR Definition

  • Stands for Valence Shell Electron Pair Repulsion, a model that predicts molecular shapes.

• Key Concept of VSEPR

  • Based on the principle that electron pairs around a central atom strive to maximize their spatial separation, minimizing electrostatic repulsion and thus determining the three-dimensional structure of molecules.