Lecture 3 - Chem 172 Advanced Inorganic Chemistry Lecture 3...

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1 Chem 172 Advanced Inorganic Chemistry Lecture 3 Simple Bonding Theory: 1. Lewis Electron Dot Diagrams 2. Valence Shell Electron Repulsion Theory To construct Lewis structure: Octet Rule: for many molecules, each atom shares electrons with neighboring atoms to achieve a total of eight valence electrons (an ‘Octet’). (1) decide total number of valence electrons provided by all atoms (2) write chemical symbols of the atoms in the arrangement with bonded atoms next to each other. (3) distribute electron pairs so that there is one pair between each pair of bonded atoms, with the extras for lone pairs or multiple bond. within octet rule, in general: # of bonds = (# of atoms x 8 - # of valence electrons)/2 ( if H, x2 )
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2 In general, the skeleton of a molecule (central and outer atoms) need to be deretmined experimentally. A few guidelines to predict skeleton structures from molecular formulas. ± Central atoms are usually the atoms with highest valence, or the largest atoms, or the least electronegative atom. ± H and the halogens are usually ( not always ) outside atoms. How to Determine the Central Atom Valence Shell Electron-Pair Repulsion Theory (VSEPR) • Allows the prediction of molecular geometry
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Lecture 3 - Chem 172 Advanced Inorganic Chemistry Lecture 3...

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