molecular shapes

VSEPR Theory

A model predicting molecular geometry based on the principle that electron pairs around a central atom repel each other and position themselves as far apart as possible.

Linear molecular geometry

The molecular geometry formed by 2 bonding pairs and 0 lone pairs around a central atom, resulting in a bond angle of $180^\circ$ (e.g., $CO_2$).

Trigonal planar molecular geometry

The molecular geometry formed by 3 bonding pairs and 0 lone pairs around a central atom, producing bond angles of $120^\circ$ (e.g., $BF_3$).

Bent molecular geometry (3 electron domains)

The shape formed by 2 bonding electron domains and 1 lone pair on a central atom, resulting in a bond angle of slightly less than $120^\circ$ (e.g., $SO_2$).

Tetrahedral molecular geometry

The molecular geometry formed by 4 bonding pairs and 0 lone pairs around a central atom, yielding bond angles of $109.5^\circ$ (e.g., $CH_4$).

Trigonal pyramidal molecular geometry

The molecular geometry formed by 3 bonding pairs and 1 lone pair on a central atom, producing bond angles of approximately $107^\circ$ (e.g., $NH_3$).

Bent molecular geometry (4 electron domains)

The molecular geometry formed by 2 bonding pairs and 2 lone pairs on a central atom, resulting in bond angles of approximately $104.5^\circ$ (e.g., $H_2O$).

Trigonal bipyramidal molecular geometry

The molecular geometry formed by 5 bonding pairs and 0 lone pairs around a central atom, featuring equatorial bond angles of $120^\circ$ and axial bond angles of $90^\circ$ (e.g., $PCl_5$).

Octahedral molecular geometry

The molecular geometry formed by 6 bonding pairs and 0 lone pairs around a central atom, where all adjacent bond angles measure $90^\circ$ (e.g., $SF_6$).