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VSEPR . Valence Shell Electron Pair Repulsion. Electron pairs orient themselves so as to make the angles between themselves as large as possible Repulsion follows Coulomb’s law This includes bonded as well as non-bonded pairs. Molecular Geometry.

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VSEPR

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Vsepr

VSEPR


Valence shell electron pair repulsion

Valence Shell Electron Pair Repulsion

  • Electron pairs orient themselves so as to make the angles between themselves as large as possible

  • Repulsion follows Coulomb’s law

  • This includes bonded as well as non-bonded pairs


Molecular geometry

Molecular Geometry

  • Non-bonded pairs are not seen on the molecule but they do affect it

  • In determining molecular geometries, multiple bonds are considered like single bonds

  • Six types of molecular geometries


Electron pair geometry

Electron Pair Geometry

  • Geometry if unshared pair thought of as a bond


Linear molecular and electron pair geometry

Linear Molecular and Electron-Pair Geometry

  • Two bonded pair and no non-bonded pairs on central atom

  • 180°


Trigonal planer molecular and electron pair geometry

TrigonalPlaner Molecular and Electron-Pair Geometry

  • Three bonded pair and no non-bonded pairs

  • 120° between bonds


Bent molecular and trigonal planer electron pair geometry

Bent Molecular and Trigonal Planer Electron-Pair Geometry

  • Two bonded pair and one non-bonded pair

  • 120° between bonds


Tetrahedral molecular and electron pair geometry

Tetrahedral Molecular and Electron-Pair Geometry

  • Four bonded pairs

  • 109.5° between bonds


Trigonal pyramidal molecular and tetrahedral electron pair geometry

TrigonalPyramidal Molecular and Tetrahedral Electron-Pair Geometry

  • Three bonded and one non-bonded

  • 109.5° between bonds


Bent molecular and tetrahedral electron pair geometry

Bent Molecular and Tetrahedral Electron-Pair Geometry

  • Two bonded and two non-bonded

  • 104.5° between bonds


Non bonding pairs

Non-Bonding Pairs

  • Exert greater repulsive forces on adjacent pairs than bonded electrons do

  • Example – All of these have tetrahedral electron pair geometries

    • CH4 109.5°

    • NH3 107°

    • H2O 104.5°


More geometries of expanded octets

More Geometries of Expanded Octets


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