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Polar and Nonpolar Covalent Bonds

Learn the difference between polar and nonpolar covalent bonds, electron pair sharing, polarity, and molecular geometry using VSEPR theory. Explore examples and order of increasing polarity for compounds such as HF, HBr, HI, and HCl.

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Polar and Nonpolar 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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