1.10 The Shapes of Some Simple Molecules. tetrahedral geometry H—C—H angle = 109.5° Methane.

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Presentation transcript:

1.10 The Shapes of Some Simple Molecules

tetrahedral geometry H—C—H angle = 109.5° Methane

tetrahedral geometry each H—C—H angle = 109.5° Methane

The most stable arrangement of groups attached to a central atom is the one that has the maximum separation of electron pairs (bonded or nonbonded). Valence Shell Electron Pair Repulsions

bent geometry H—O—H angle = 105° but notice the tetrahedral arrangement of electron pairs O H.. H : Figure 1.9 (a): Water

trigonal pyramidal geometry H—N—H angle = 107° but notice the tetrahedral arrangement of electron pairs N H H H : Figure 1.9 (b): Ammonia

F—B—F angle = 120° trigonal planar geometry allows for maximum separation of three electron pairs Figure 1.9 (c): Boron Trifluoride

Four-electron double bonds and six-electron triple bonds are considered to be similar to a two-electron single bond in terms of their spatial requirements. Multiple Bonds

H—C—H and H—C—O angles are close to 120° trigonal planar geometry C O HH Figure 1.11: Formaldehyde

O—C—O angle = 180° linear geometry OCO Figure 1.12: Carbon Dioxide

1.11 Molecular Dipole Moments

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

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

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

OCO Carbon dioxide has no dipole moment;  = 0 D Molecular Dipole Moments

 = 1.62 D  = 0 D Carbon tetrachloride Dichloromethane Figure 1.13

Resultant of these two bond dipoles is  = 0 D Carbon tetrachloride has no dipole moment because all of the individual bond dipoles cancel. Resultant of these two bond dipoles is Figure 1.13

Resultant of these two bond dipoles is  = 1.62 D Resultant of these two bond dipoles is The individual bond dipoles do not cancel in dichloromethane; it has a dipole moment. Figure 1.13