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Chemical Bonding
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Draw the following PBr3 N2H2 CH3OH NO2-
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VSEPR Theory Repulsion between valence electron pairs causes the pairs to be oriented as far apart as possible
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Tetrahedral geometry 4 single bonds No unshared pais
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Triangular Pyramidal 3 single bonds and one unshared pair
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Bent 2 single bonds and two unshared pairs
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Linear Only two atoms or Two double bonds and no unshared pairs
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Bent One single and one double bond and one unshared pair
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Triangular Planer One double and two single bonds and no unshared pairs
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Polar Molecules When two unlike atoms are covalently bonded, the shared electrons will be more strongly attracted to the atom of greater electronegativity
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Polar molecules behave as if one end is positive and one end is negative
The more electronegative atom is negative
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Sometimes atoms with high differences in electronegativity will not be polar molecules because the structure is symmetrical and the polarity cancels out
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Polar Molecules In order to be a polar molecule, two conditions must be met 1) there must be a polar difference in electronegativity 2) the molecule is NOT be symmetrical
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