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3.7: Polar Covalent Bonds and Electronegativity

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Presentation on theme: "3.7: Polar Covalent Bonds and Electronegativity"— Presentation transcript:

1 3.7: Polar Covalent Bonds and Electronegativity
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2 Electronegativity Electronegativity is a measure of an element to attract electrons toward itself when bonded to another element. An electronegative element attracts electrons. An electropositive element releases electrons. 2

3 Pauling Electronegativity Scale
Electronegativity increases from left to right in the periodic table. Electronegativity decreases going down a group. 5

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5 Generalization The greater the difference in electronegativity between two bonded atoms; the more polar the bond. F : .. H—H : N nonpolar bonds connect atoms of the same electronegativity 7

6 Generalization The greater the difference in electronegativity between two bonded atoms; the more polar the bond. O .. H d+ d- d- d+ d- F : .. H d+ d- : O C O : .. .. polar bonds connect atoms of different electronegativity 7

7 3.7 Molecular Dipole Moments
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8 (expressed in Debye units)
Dipole Moment A substance possesses a dipole moment if its centers of positive and negative charge do not coincide. m = e x d (expressed in Debye units) + — not polar 17

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12 (expressed in Debye units)
Dipole Moment A substance possesses a dipole moment if its centers of positive and negative charge do not coincide. m = e x d (expressed in Debye units) — + polar 17

13 Molecular Dipole Moments
molecule must have polar bonds necessary, but not sufficient need to know molecular shape because individual bond dipoles can cancel 18

14 Molecular Dipole Moments
Carbon dioxide has no dipole moment; m = 0 D 18

15 Comparison of Dipole Moments
Carbon tetrachloride Dichloromethane m = 0 D m = 1.62 D 20

16 Carbon tetrachloride m = 0 D
Resultant of these two bond dipoles is Resultant of these two bond dipoles is m = 0 D Carbon tetrachloride has no dipole moment because all of the individual bond dipoles cancel. 20

17 Dichloromethane Resultant of these two bond dipoles is Resultant of these two bond dipoles is m = 1.62 D The individual bond dipoles do not cancel in dichloromethane; it has a dipole moment. 20

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