This is an example of a octahedral molecule that contains no lone pairs. This is a Sulfur hexaflouride molecule, SF6, which contains 48 valence electrons to use for the lewis dot structure. When the lewis dot structure is drawn there are six bonding locations and no lone pairs on the central atom. This type of configuration would give you a octahedral geometry. The angles are 90 degrees all around except for opposite atoms, which would be 180 degrees. Other octahedral molecules would be SCl6, SeF6, and SeBr6. Click on the top picture to see the rotation of the molecule.