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Section 6-5

Section 6-5 . Molecular Geometry. Exceptions to the Octet Rule. Hydrogen forms bonds in which it is surrounded by only two electrons. Boron tends to form bonds in which it is surrounded by only six electrons. Ex: BF3

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Section 6-5

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  1. Section 6-5 Molecular Geometry

  2. Exceptions to the Octet Rule • Hydrogen forms bonds in which it is surrounded by only two electrons. • Boron tends to form bonds in which it is surrounded by only six electrons. Ex: BF3 • Other elements can be surrounded by more than eight electrons when they combine with the highly electronegative elements fluorine, oxygen, and chlorine.

  3. VSEPR Theory • Repulsion between electrons causes these sets of electrons to be as far apart as possible.

  4. 2. Trigonal Planar • 3 Atoms bonded to central atom • No lone pairs of electrons • Ex: BF3

  5. 3. Tetrahedral • 4 Atoms bonded to central atom • 0 Lone pairs of electrons • Ex: CH4

  6. 4. Trigonal pyramidal • 3 atoms bonded to central atom • 1 lone pair of electrons • Ex: NH3

  7. 5. Trigonal bipyramidal • 5 atoms bonded to central atom • 0 Lone pairs of electrons • Ex: PCl5

  8. 6. Bent or Angular • 2 Atoms bonded to central atom • 1 or 2 lone pairs of electrons • Ex: H2O

  9. 7. Octahedral • 6 Atoms bonded to central atom • 0 Lone pairs of electrons • Ex: SF6

  10. Intermolecular Forces • Forces of attraction between molecules • Ionic bonds have stronger intermolecular forces than covalent bonds. • This contributes to a higher melting and boiling point.

  11. Dipole-Dipole Forces • Polar molecules act as tiny dipoles because of their uneven charge distribution. • The negative region in one polar molecule attracts the positive region in adjacent molecules.

  12. Hydrogen Bonding • Type of Dipole-Dipole force. • Occurs when hydrogen is bonded to a highly electronegative atom giving it a slightly positive charge. • Hydrogen (slightly positive) is attracted to the unshared pair of electrons on the electronegative element. • Ex: HF, H2O, NH3 • Causes these compounds to have a high boiling point

  13. Hydrogen Bonding

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