Chem 161-2009 homework 13th week

Chem 161-2009 homework 13th week - Chem 161-2009 Homework...

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Chem 161-2009 Homework 13 th Week Chapter 10 problems: 31,35,41,43,45, 3,10,14,45,53,55,57,75,77,84,87,90 31. Explain why the molecule BF 3 is trigonal planar, whereas a molecule with a similar formula, ClF3, is T-shaped. BF 3 . . : F : . . | . . : F ― B ― F : Trigonal planar . . . . . . .. . . . . : F ― Cl ― F : T-shaped . . | . . : F : . . The difference is that boron only has three electrons in its valence shell, whereas chlorine has seven electrons in its valence shell. This difference of four electrons explains the electron group geometry. 35. The molecules NF 3 and PCl 3 are both trigonal pyramidal, and we can conclude that their bond angles are about the same. The molecules H 2 O and SO 2 are both angular, but we cannot draw the same conclusion about them. Why not? . . : F : . . | . . : F ― N ― F : . . . . . . . . : Cl : . . | . . : Cl ― P ― Cl : . . . . . . NF 3 and PCl 3 have identical Lewis structures, so their bond angles should be identical. 1
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H ·· : O H 2 O is bent. H . . . . . . SO 2 is bent. : O ― S = O : . . Although both H 2 O and SO 2 are angular, the electron group geometry for water is tetrahedral (bond angle 109.5 o ), while the electron group geometry for SO2 is trigonal planar (bond angle 120 o ). Molecular Shape and Dipole Moments 41. Draw structural formulas and use cross-based arrows to represent bond dipoles and any resultant molecular dipole in molecules of (a) GeCl 4 and (b) SF 4 . . . :Cl: . . | . . :Cl―Ge―Cl : No molecular dipole due to . . | . . vectorial symmetry :Cl: . . . . : F : . . . . | . . : F ― S ― F : Molecular dipole away . . | . . from non-bonding : F : electron pair. . . 2
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Valence Bond Theory 43. Describe the bonding in the molecules Li 2 (g) and F 2 (g) by the valence bond theory. How can the theory account for the difference in bond energies, 106 kJ/mol for the Li―Li bond and 157 kJ/mol for the F―F bond? 3
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Chem 161-2009 homework 13th week - Chem 161-2009 Homework...

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