The Lewis electron-pair approach described previously can be used to predict the number and types of bonds between the atoms in a substance, and it indicates which atoms have lone pairs of electrons. This approach gives no information about the actual arrangement of atoms in space, however. Molecular Geometry The specific three dimensional arrangement of atoms in molecules is referred to as molecular geometry . We also define molecular geometry as the positions of the atomic nuclei in a molecule. There are various instrumental techniques such as X-Ray crystallography and other experimental techniques which can be used to tell us where the atoms are located in a molecule. Using advanced techniques, very complicated structures for proteins, enzymes, DNA , and RNA have been determined. Molecular geometry is associated with the chemistry of vision, smell, taste, drug reactions, and enzyme controlled reactions to name a few. Example \(\PageIndex{1}\): Carbon Tetrachloride The Lewis structure of carbon tetrachloride provides information about connectivities, provides information about valence orbitals, and provides information about bond character. However, the Lewis structure provides no information about the shape of the molecule, which is defined by t he bond angles and the bond lengths . For carbon tetrachloride, each C-Cl bond length is 1.78Å and each Cl-C-Cl bond angle is 109.5°. Hence, carbon tetrachloride is tetrahedral in structure: Molecular Geometries of \(AB_n\) molecules Molecular geometry is associated with the specific orientation of bonding atoms. A careful analysis of electron distributions in orbitals will usually result in correct molecular geometry determinations. In addition, the simple writing of Lewis diagrams can also provide important clues for the determination of molecular geometry. Molecular shapes, or geometries, are critical to molecular recognition and function. Table \(\PageIndex{1}\) shows some examples of geometries where a central atom \(A\) is bonded to two or more \(X\) atoms. As indicated in several of the geometries below, non-bonding electrons \(E\) can strongly influence the molecular geometry of the molecule; this is discussed in more details in VSEPR Model" data-cke-saved-href="/Bookshelves/General_Chemistry/Map:_Chemistry_-_The_Central_Science_(Brown_et_al.)/09:_Molecular_Geometry_and_Bonding_Theories/9.02:_The_VSEPR_Model" href="/Bookshelves/General_Chemistry/Map:_Chemistry_-_The_Central_Science_(Brown_et_al.)/09:_Molecular_Geometry_and_Bonding_Theories/9.02:_The_VSEPR_Model" data-quail-id="26">Section 9.2. 6 5 4 3 2 AX6 octahedral AX5 trigonal bipyramidal AX4 tetrahedral AX3 trigonal planar AX2 linear 1 lone pair of electrons 1 lone pair of electrons 1 lone pair of electrons 1 lone pair of electrons 1 lone pair of electrons AX5E square pyramidal AX4E distorted tetrahedron AX3E pyramidal AX2E nonlinear AXE linear 2 lone pairs of electrons 2 lone pairs of electrons 2 lone pairs of electrons 2 lone pairs of electrons NaN AX4E2 square planar AX3E2 T-shaped AX2E2 bent AXE2 linear NaN These structures can generally be predicted, when A is a nonmetal, using the "valence-shell electron-pair repulsion model (VSEPR) discussed in the next section.