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Polar and Non-polar Covalent Bonds

Polar and Non-polar Covalent Bonds. Polar Bond - When the electron pair in a covalent bond is NOT shared equally. H EN = 2.1 Cl EN = 3.0  EN = 0.8  = 1.03 D.  =q*d (unit Debyes (D)) (pg. 298). Polar Bond - When the electron pair in a covalent bond is

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Polar and Non-polar Covalent Bonds

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  1. Polar and Non-polar Covalent Bonds Polar Bond - When the electron pair in a covalent bond is NOT shared equally H EN = 2.1 Cl EN = 3.0 EN = 0.8  = 1.03 D =q*d (unit Debyes (D)) (pg. 298) Polar Bond - When the electron pair in a covalent bond is shared equally H EN = 2.1 EN = 0.0  = 0.0 D

  2. Put the following compound in order of increasing polarity: HF, HBr, HI & HCl HF > HCl > HBr > HI

  3.  EN Zero Intermediate  Large Bonding Covalent Polar Covalent Ionic Ionic Character NH4NO3 Covalent bonding inside NH4+ Covalent bonding inside NO3- Ionic bonding between the NH4+ and NO3- K2SO4 Covalent bonding inside SO42- Ionic bonding between K+ and SO42- Covalent Character

  4. Valence Shell Electron Pair Repulsion (VSEPR) Theory Valence shell electrons will arrange themselves about a central atom so that replusions among them are as small as possible Used to determine the Molecular Geometry (Shape) of a molecule (Lewis Dot structures only give us the order of bonding) Count the # of regions of high electron density: a region of high e- density is a bond (single, double or triple) or a lone pair.

  5. CO2 • Lewis Dot Structure • O=C=O • only tells us the bonding and not the Geometry • VSEPR • # of high e- density regions around the central atom • 2 bonds and 0 lone pairs • Linear O=C=O OCO  180o • Therefore, the Molecular Geometry (Shape) is linear

  6. BF3 Lewis Dot Structure VSEPR # of high e- density regions around the central atom 3 bonds and 0 lone pairs Trigonal Planar FBF  120o  the Molecular Geometry (Shape) is Trigonal Planar

  7. H H C H H CH4 Lewis Dot Structure VSEPR # of high e- density regions around the central atom 4 bonds and 0 lone pairs Tetrahedral HCH  109.5o  the Molecular Geometry (Shape) is Tetrahedral

  8. F F F P F F PF5 Lewis Dot Structure VSEPR # of high e- density regions around the central atom 5 bonds and 0 lone pairs Trigonal Bipyramidal FPF 90.0o & 120.0o & 180.0o  the Molecular Geometry (Shape) is Trigonal Bipyramidal

  9. F F SF6 Lewis Dot Structure VSEPR # of high e- density regions around the central atom 6 bonds and 0 lone pairs Octahedral FSF 90.0o & 180.0o  the Molecular Geometry (Shape) is Octahedral S F F F F

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