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Bonding Theories Section 16.2

Bonding Theories Section 16.2. Do not worry about the Molecular Orbitals! VSEPR Theory – Valence Shell Electron Pair Repulsion Theory Electrons will repel each other, so that they are as far apart as possible

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Bonding Theories Section 16.2

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  1. Bonding TheoriesSection 16.2 • Do not worry about the Molecular Orbitals! • VSEPR Theory – Valence Shell Electron Pair Repulsion Theory • Electrons will repel each other, so that they are as far apart as possible • Determines the shape of the atom, based on the number of bonding pairs of electrons and lone pairs of electrons

  2. Example of how VSEPR Theory works: Each bond will repel each other so that the atoms are as far away as possible. CH4 (shown to the left) is tetrahedral ( 4 bonding pairs, 0 lone pairs) Lone pairs of electrons will push the bonding pairs down, which changes the shape NH3 is trigonal pyramidal(3 bonding pairs and 1 lone pairs)

  3. Lone pairs and bonding pairs Bonding pairs = the number of elements bonded to the central atom Oxygen is bonded to 2 hydrogen atoms, so it has 2 bonding pairs Lone pairs = the number of paired electrons on the central atom that is not bonded to another atom Oxygen is sharing all 4 electrons with hydrogen, but it has 2 pairs of electrons that are not bonded to another atom (2 lone pairs) O C O O H H Bonding pairs = the number of elements bonded to the central atom Carbon is bonded to 2 oxygen atoms, so it has 2 bonding pairs Lone pairs = the number of paired electrons on the central atom that is not bonded to another atom Carbon is sharing all 8 electrons with oxygen, therefore it has 0 bonding pairs

  4. After reading Section 16.2, you should know: • How to determine the number of bonding pairs and lone pairs of electrons on the central atom • How to determine the shape of a given covalent compound

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