VALENCESHELL ELECTRON PAIR REPULSION (VSEPR) MODEL
Assumptions the the VSEPR Model:
1. Electrons repel eachother. Electron bag in the valence shell orbitals of an atom exertrepulsive pressures on various other electron pairs.
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2. Electron bag adoptconfiguration that minimization the electron pair repulsions in the valence shell.
3. Multiple bonds count together asingle pair that electrons.
Determination of shortcut Angles
1. Lone pair electronsoccupy more space than bonding electrons. The visibility of lone pairelectrons will certainly distort predicted shortcut angles.
e.g. No lonepairs one lone pairtwo lone pairs
CH4NH3H2O
109.5o107o104.5o
2. Many bonds perform notaffect the gross stereosdrta.netistry that the molecule. The geometry ofthe molecule is determined by the number of bonded atoms plus the number of lonepairs that electrons about the main atom.
Note: Geometry describes thebond angles about a central atom. Geometry is determined by thetotal variety of bonded atoms and also lone pairs approximately the central atom. Shape(or molecular structure) describes the position of the atoms in amolecule. Form is identified by the family member placement of the bondedatoms approximately the central atom. Because that a molecule, geometry and shape room thesame only as soon as there are no lone bag of electrons approximately the centralatom.
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| Examples | total bonds + e- pairs | lone e- pairs | Lewis structure | Geometry | Shape | Structure | Bond angles | Hybridization | |
| CO2† | 2 | 0 |  | linear | linear | 180 | sp | ||
| CH2O† | 3 | 0 |  | trigonal planar | trigonal planar | 120 | sp2 | ||
| SO2† | 3 | 1 |  | trigonal planar | V-shaped or bent | 120 | sp2 | ||
| CH4 | 4 | 0 |  | tetrahedral | tetrahedral | 109.5 | sp3 | ||
| NH3 | 4 | 1 |  | tetrahedral | trigonal pyramid | 107 | sp3 | ||
| H2O | 4 | 2 |  | tetrahedral | V-shaped or bent | 104.5 | sp3 | ||
| HCl | 4 | 3 |  | tetrahedral | linear | 180 | sp3 | ||
| PCl5 | 5 | 0 |  | trigonal bipyramid | trigonal bipyramid | 120, 90, 180 | sp3d | ||
| SF4‡ | 5 | 1 |  | trigonal bipyramid | see-saw | 120, 90, 180 | sp3d | ||
| ClF3‡ | 5 | 2 |  | trigonal bipyramid | T-shaped | 90, 180 | sp3d | ||
| KrF2‡ | 5 | 3 |  | trigonal bipyramid | linear | 180 | sp3d | ||
| SF6 | 6 | 0 |  | octahedral | octahedral | 90, 180 | sp3d2 | ||
| ICl5 | 6 | 1 |  | octahedral | square pyramid | 90, 180 | sp3d2 | ||
| XeF4* | 6 | 2 |  | octahedral | square planar | 90, 180 | sp3d2 |
†Multiple bonds execute not affect the geometry that a molecule, i.e., multiple binding = single bonds, in effect.‡Lone pair electrons occupy the roomier, equatorial orbitals.*Lone pairs occupy orbitals as far from each other as possible.