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VSPER Structures

VSPER Structures. Chapter 6 Section 5. Molecular Geometry. Help to determine the properties of molecules Molecular polarity- the uneven distribution of molecular charge. VSPER Theory. “valence shell, electron pair repulsion”

benjamin-bates
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VSPER Structures

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  1. VSPER Structures Chapter 6 Section 5

  2. Molecular Geometry • Help to determine the properties of molecules • Molecular polarity- the uneven distribution of molecular charge

  3. VSPER Theory • “valence shell, electron pair repulsion” • Repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be orientated as far apart as possible

  4. Using VSPER Theory • Step one- Draw the Lewis Dot structure for the compound CBr4 • Step two- Be sure to arrange the atoms so they are the farthest distance apart

  5. VSPER and Molecular Geometry • Molecular Shape: Linear • Atoms bonded to the central atom: 2 • Lone pair of electrons: 0 • Type of molecule: AB2 • Example Formula: Carbon Dioxide

  6. VSPER and Molecular Geometry • Molecular Shape: Bent • Atoms bonded to the central atom: 2 • Lone pairs of electrons: 1 • Type of Molecule: AB2E • Example: Water

  7. VSPER and Molecular Geometry • Molecular Shape: Trigonalplanar • Atoms bonded to central atom: 3 • Lone Pairs of electrons: 0 • Type of molecule: AB3 • Example: AlCl3

  8. VSPER and Molecular Geometry • Molecular Shape: Tetrahedral • Atoms bonded to central atom: 4 • Lone Pairs of electrons: 0 • Type of molecule: AB4 • Example: CH4

  9. VSPER and Molecular Geometry • Molecular Shape: Trigonal-pyramidal • Atoms bonded to central atom: 3 • Lone Pairs of electrons: 1 • Type of molecule: AB3E • Example:PH3

  10. VSPER and Molecular Geometry • Molecular Shape: Trigonal-bipyramidal • Atoms bonded to central atom: 5 • Lone Pairs of electrons: 0 • Type of molecule: AB5 • Example: NbBr5

  11. VSPER and Molecular Geometry • Molecular Shape: Octahedral • Atoms bonded to central atom: 6 • Lone Pairs of electrons: 0 • Type of molecule: AB6 • Example: SF6

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