A bond angle is the geometric angle between two adjacent bonds. Some common shapes of simple molecules include:
* Linear: In a linear model, atoms are connected in a straight line. The bond angles are set at 180°. For example, carbon dioxide and nitric oxide have a linear molecular shape.
* Trigonal planar: Molecules with the trigonal planar shape are somewhat triangular and in one plane (flat).  Consequently, the bond angles are set at 120°. For example, boron trifluoride.
* Angular: Angular molecules (also called bent or V-shaped) have a non-linear shape. For example, water (HO), which has an angle of about 105°. A water molecule has two pairs of bonded electrons and two unshared lone pairs.
* Tetrahedral: Tetra- signifies four, and -hedral relates to a face of a solid, so "tetrahedral" literally means "having four faces".  This shape is found when there are four bonds all on one central atom, with no extra unshared electron pairs.  In accordance with the VSEPR (valence-shell electron pair repulsion theory), the bond angles between the electron bonds are arccos(−) = 109.47°. For example, methane (CH) is a tetrahedral molecule. 
* Octahedral: Octa- signifies eight, and -hedral relates to a face of a solid, so "octahedral" means "having eight faces". The bond angle is 90 degrees. For example, sulfur hexafluoride (SF) is an octahedral molecule.
* Trigonal pyramidal: A trigonal pyramidal molecule has a pyramid-like shape with a triangular base.  Unlike the linear and trigonal planar shapes but similar to the tetrahedral orientation, pyramidal shapes require three dimensions in order to fully separate the electrons.  Here, there are only three pairs of bonded electrons, leaving one unshared lone pair. Lone pair – bond pair repulsions change the bond angle from the tetrahedral angle to a slightly lower value. For example, ammonia (NH).