Editing VSEPR theory (section)

==Overview==
VSEPR theory is used to predict the arrangement of electron pairs around central atoms in molecules, especially simple and symmetric molecules. A central atom is defined in this theory as an atom which is bonded to two or more other atoms, while a terminal atom is bonded to only one other atom.<ref name="Petrucci" />{{rp|398}} For example, in the molecule [[methyl isocyanate]] (H<sub>3</sub>C-N=C=O), the two carbons and one nitrogen are central atoms, and the three hydrogens and one oxygen are terminal atoms.<ref name="Petrucci" />{{rp|416}} The geometry of the central atoms and their non-bonding electron pairs in turn determine the geometry of the larger whole molecule.

The number of electron pairs in the valence shell of a central atom is determined after drawing the [[Lewis structure]] of the molecule, and expanding it to show all bonding groups and [[lone pair]]s of electrons.<ref name=Petrucci>{{cite book|last1=Petrucci |first1=R. H. |first2=Harwood |last2=W. S. |first3=Herring |last3=F. G. |title=General Chemistry: Principles and Modern Applications |publisher=Prentice-Hall |edition=8th |year=2002 |isbn=978-0-13-014329-7}}</ref>{{rp|410–417}} In VSEPR theory, a [[double bond]] or [[triple bond]] is treated as a single bonding group.<ref name=Petrucci/> The sum of the number of atoms bonded to a central atom and the number of [[lone pair]]s formed by its nonbonding [[valence electron]]s is known as the central atom's steric number.

The electron pairs (or groups if multiple bonds are present) are assumed to lie on the surface of a sphere centered on the central atom and tend to occupy positions that minimize their mutual repulsions by maximizing the distance between them.<ref name=Petrucci/>{{rp|410–417}}<ref name=Miessler>{{cite book|first1=G. L. |last1=Miessler |first2=D. A. |last2=Tarr |title=Inorganic Chemistry |edition=2nd |publisher=Prentice-Hall |year=1999 |pages=54–62 |isbn=978-0-13-841891-5}}</ref> The number of electron pairs (or groups), therefore, determines the overall geometry that they will adopt. For example, when there are two electron pairs surrounding the central atom, their mutual repulsion is minimal when they lie at opposite poles of the sphere. Therefore, the central atom is predicted to adopt a ''linear'' geometry. If there are 3 electron pairs surrounding the central atom, their repulsion is minimized by placing them at the vertices of an equilateral triangle centered on the atom. Therefore, the predicted geometry is ''[[triangular|trigonal]]''. Likewise, for 4 electron pairs, the optimal arrangement is ''[[tetrahedron|tetrahedral]]''.<ref name=Petrucci/>{{rp|410–417}}

As a tool in predicting the geometry adopted with a given number of electron pairs, an often used physical demonstration of the principle of minimal electron pair repulsion utilizes inflated balloons. Through handling, balloons acquire a slight surface electrostatic charge that results in the adoption of roughly the same geometries when they are tied together at their stems as the corresponding number of electron pairs.  For example, five balloons tied together adopt the ''[[trigonal bipyramidal molecular geometry|trigonal bipyramidal]]'' geometry, just as do the five bonding pairs of a PCl<sub>5</sub> molecule.

===Steric number===
[[Image:Sulfur-tetrafluoride-2D-dimensions.png|thumb|Sulfur tetrafluoride has a steric number of 5.]]
The steric number of a central atom in a molecule is the number of atoms bonded to that central atom, called its [[coordination number]], plus the number of [[lone pair]]s of valence electrons on the central atom.<ref>{{cite book|first1=G. L. |last1=Miessler |first2=D. A. |last2=Tarr |title=Inorganic Chemistry |edition=2nd |publisher=Prentice-Hall |year=1999 |pages=55 |isbn=978-0-13-841891-5}}</ref> In the molecule [[Sulfur tetrafluoride|SF<sub>4</sub>]], for example, the central sulfur atom has four [[ligand]]s; the [[coordination number]] of sulfur is four. In addition to the four ligands, sulfur also has one lone pair in this molecule. Thus, the steric number is 4 + 1 = 5.

===Degree of repulsion===
The overall geometry is further refined by distinguishing between ''bonding'' and ''nonbonding'' electron pairs. The bonding electron pair shared in a [[sigma bond]] with an adjacent atom lies further from the central atom than a nonbonding (lone) pair of that atom, which is held close to its positively charged nucleus. VSEPR theory therefore views repulsion by the lone pair to be greater than the repulsion by a bonding pair. As such, when a molecule has 2 interactions with different degrees of repulsion, VSEPR theory predicts the structure where lone pairs occupy positions that allow them to experience less repulsion. Lone pair–lone pair (lp–lp) repulsions are considered stronger than lone pair–bonding pair (lp–bp) repulsions, which in turn are considered stronger than bonding pair–bonding pair (bp–bp) repulsions, distinctions that then guide decisions about overall geometry when 2 or more non-equivalent positions are possible.<ref name=Petrucci/>{{rp|410–417}} For instance, when 5 valence electron pairs surround a central atom, they adopt a ''trigonal bipyramidal'' molecular geometry with two collinear ''axial'' positions and three ''equatorial'' positions. An electron pair in an axial position has three close equatorial neighbors only 90° away and a fourth much farther at 180°, while an equatorial electron pair has only two adjacent pairs at 90° and two at 120°. The repulsion from the close neighbors at 90° is more important, so that the axial positions experience more repulsion than the equatorial positions; hence, when there are lone pairs, they tend to occupy equatorial positions as shown in the diagrams of the next section for steric number five.<ref name=Miessler/>

The difference between lone pairs and bonding pairs may also be used to rationalize deviations from idealized geometries. For example, the H<sub>2</sub>O molecule has four electron pairs in its valence shell: two lone pairs and two bond pairs.  The four electron pairs are spread so as to point roughly towards the apices of a tetrahedron.  However, the bond angle between the two O–H bonds is only 104.5°, rather than the 109.5° of a regular tetrahedron, because the two lone pairs (whose density or probability envelopes lie closer to the oxygen nucleus) exert a greater mutual repulsion than the two bond pairs.<ref name=Petrucci/>{{rp|410–417}}<ref name=Miessler/>

A bond of higher [[bond order]] also exerts greater repulsion since the [[pi bond]] electrons contribute.<ref name=Miessler/> For example, in [[isobutylene]], (H<sub>3</sub>C)<sub>2</sub>C=CH<sub>2</sub>, the H<sub>3</sub>C−C=C angle (124°) is larger than the H<sub>3</sub>C−C−CH<sub>3</sub> angle (111.5°). However, in the [[carbonate]] ion, {{chem|CO|3|2−}}, all three C−O bonds are equivalent with angles of 120° due to [[resonance (chemistry)|resonance]].