A-level Chemistry/OCR (Salters)/Molecular geometry
The shapes of molecules is the title of Section 3.3 in Chemical Ideas and it covers the topic of molecular geometry.
Introductory examplesEdit
Methane moleculeEdit
Ammonia moleculeEdit
Water moleculeEdit
Hydrogen fluoride moleculeEdit
PolyhedraEdit
TetrahedraEdit
You have probably come across tetrahedra before in maths, although you most likely called them triangle-based pyramids. Tetrahedra have four vertices (corners), four faces and six edges. Each face is an equilateral triangle.
The tetrahedron is one of the most important shapes in chemistry because a very great many molecules contain them. Tetrahedral molecules don't actually contain little pyramids. What they do contain is a central atom bonded to four other atoms. The four atoms surrounding the central atom occupy positions that you can imagine as the vertices of a tetrahedron.
In the image gallery below, the central atom is coloured magenta and the surrounding atoms are coloured white.
The angle between any two bonds in a tetrahedral molecule is approximately 109.5°. The tetrahedral angle can be calculated as accurately as required because it is equal to cos^{−1}(–⅓).
OctahedraEdit
You may or may not have met an octahedron before. Octahedra have six vertices (corners), eight faces and twelve edges. Each face is an equilateral triangle.
Octahedra are very important in chemistry because many transition metal-based molecules are octahedral.
Common molecular geometriesEdit
Further examplesEdit
Example moleculesEdit
Example ionsEdit
Molecular geometry and lone pairsEdit
You can use the so-called AXE method to calculate the shape of a molecule. It is based on molecules that have a central atom, which we label A. Atoms or groups bonded to A are labelled X. Lone pairs are labelled E. A molecule with three lone pairs and two atoms/groups bonded to it would be denoted AX_{2}E_{3}. The table below shows how X and E and molecular shape are related.
Valence shell electron pair repulsion theory (VSEPR) is used to predict the shape of a molecule once X and E are known. This sounds more complicated than it is. You consider any X's and E's to be regions of charge that position themselves as far apart from each other as possible, in order to minimize the forces of electrostatic repulsion between each other.
AXE label | X (substituents) |
E (lone pairs) |
Shape | 2D diagram lone pairs shown |
2D diagram lone pairs not shown |
3D model lone pairs shown |
3D model lone pairs not shown |
Examples |
---|---|---|---|---|---|---|---|---|
AX_{1}E_{0} | Linear | H_{2} | ||||||
AX_{1}E_{1} | Linear | CN^{−} | ||||||
AX_{1}E_{2} | Linear | O_{2} | ||||||
AX_{1}E_{3} | Linear | HCl | ||||||
AX_{2}E_{0} | Linear | BeCl_{2} HgCl_{2} CO_{2} | ||||||
AX_{2}E_{1} | Bent | NO_{2}^{−} SO_{2} O_{3} | ||||||
AX_{2}E_{2} | Bent | H_{2}O H_{2}S OF_{2} | ||||||
AX_{2}E_{3} | Linear | XeF_{2} I_{3}^{−} | ||||||
AX_{3}E_{0} | Trigonal planar | BF_{3} CO_{3}^{2−} NO_{3}^{−} SO_{3} | ||||||
AX_{3}E_{1} | Trigonal pyramidal | NH_{3} PCl_{3} | ||||||
AX_{3}E_{2} | T-shaped | ClF_{3} BrF_{3} | ||||||
AX_{4}E_{0} | Tetrahedral | CH_{4} NH_{4}^{+} PO_{4}^{3−} SO_{4}^{2−} ClO_{4}^{−} | ||||||
AX_{4}E_{1} | Seesaw | SF_{4} | ||||||
AX_{4}E_{2} | Square Planar | XeF_{4} | ||||||
AX_{5}E_{0} | Trigonal Bipyramidal | PCl_{5} | ||||||
AX_{5}E_{1} | Square pyramidal | ClF_{5} BrF_{5} | ||||||
AX_{5}E_{2} | Pentagonal planar | XeF_{5}^{-} | ||||||
AX_{6}E_{0} | Octahedral | SF_{6} | ||||||
AX_{6}E_{1} | Pentagonal pyramidal | IF_{6}^{-} | ||||||
AX_{7}E_{0} | Pentagonal bipyramidal | IF_{7} | ||||||
AX_{8}E_{0} | Square antiprismatic | IF_{8}^{-} | ||||||
AX_{8}E_{1} | Distorted square antiprismatic | XeF_{8}^{2-} | ||||||
AX_{9}E_{0} | Tricapped trigonal prismatic OR capped square antiprismatic | ReH_{9}^{2-} (tricapped trigonal prismatic) |