Molecular Shapes AB2 Linear AB3 Trigonal planar AB2E Angular or Bent
{"Image DocumentName": "Molecular Shapes AB2 Linear AB3 Trigonal planar AB2E Angular or Bent", "Image ImageDescription": "Tetrahedral. AB3E. Trigonal. pyramidal. AB2E2. Angular. or Bent. (Source: R.J. Gillespie, J. Chem. Educ., 40, 295, 1963.) Predicts the structure of nearly any molecule or polyatomic ion that has a nonmetal central atom and the structures of many compounds that contain a central metal atom. In discussions of the structures of molecules or polyatomic ions, species are classified according to the number of atoms (n) of one type (B) attached to the central atom (A) using the notation ABn, but not all ABn species with the same value of n have the same structure. VSEPR model assumes that the electron pairs around the central atom of a Lewis structure occupy space, whether they are bonding pairs or lone pairs, and the most stable arrangement of electron pairs (the one with the lowest energy) is the one that minimizes repulsions between the electrons. VSEPR model distinguishes between the electron-pair geometry, the three-dimensional arrangement of electron pairs around the central atom, and the molecular geometry, the arrangement of the bonded atoms in a molecule or polyatomic ion. Electron-pair geometry. \u2013 Describes the arrangement of all valence electrons around the central atom, whether bonding or not. \u2013 Electrostatic repulsion between two particles that have the same charge depends on the distance between them. \u2013 Repulsions between electron pairs depend strongly on the angle between them \u2014 the smaller the angle, the closer they are and the greater the electrostatic repulsion. 1. For compounds with two electron pairs around the central atom, the lowest-energy arrangement is linear and has the electron pairs on opposite sides of the central atom with a 180\u00ba angle between them. 2. For compounds with three electron pairs around the central atom, the lowest-energy arrangement is trigonal planar, with electron pairs at 120\u00ba angles from each other. 3. In compounds with four electron pairs around the central atom, the electron pairs point toward the vertices of a tetrahedron with 109.5\u00ba angles between adjacent electron pairs. 4. In compounds with five electron pairs, the electron pairs have a trigonal bipyramidal arrangement, which has two sets of angles between adjacent electron pairs; one set contains three electron pairs at 120\u00ba. angles to one another in a plane, and a second set contains two electron pairs positioned at 90\u00ba to that plane. 5. Lowest-energy arrangement for six electron pairs is an octahedron, in which adjacent electron pairs are positioned at 90\u00ba angles to one another. AB5. Trigonal bipyramidal. AB4E. Irregular tetrahedral. (see saw) AB3E2. T-shaped. AB2E3. Linear. AB6. Octahedral. AB5E. Square pyramidal. AB4E2. Square planar.", "Image XResolution": "37", "Image YResolution": "37", "Image ResolutionUnit": "Pixels/Centimeter", "Image Software": "SlidePlayer", "Image YCbCrPositioning": "Centered"}