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Polar and Non-polar Covalent Bonds

Published bySusanti Setiabudi Modified over 4 years ago

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Presentation on theme: "Polar and Non-polar Covalent Bonds"— Presentation transcript:

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 NH4NO3 K2SO4 Covalent bonding inside NH4+ Covalent bonding inside NO3-
 EN Zero  Intermediate  Large Bonding Covalent  Polar Covalent  Ionic Ionic Character Covalent 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-

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

8 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 P F

9 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 F F F S F F F

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