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Chapter 10: Chemical Bonding I: Basic Concepts 446 129. (D) (a) The two bond dipole moments can be added geometrically, by placing the head of one at the tail of the other, as long as we do not change the direction or the length of the moved dipole. The resultant molecular dipole moment is represented by the arrow drawn from the tail of one bond dipole to the head of the other. This is shown in the figure to the right. The 52.0" angle in the figure is one-half of the 104" bond angle in water. The length is given as 1.84 D. We can construct a right angled triangle by bisecting the 76.06 angle. The right angled triangle has a hypotenuse O * H bond dipole and the two other angles are 526 and 386. The side opposite the bisected 76.0 6 angles is ½ (1.84 D) 0.92 D. We can calculate the bond dipole using: sin 38.06 0.92D O-H bond dipole 0.61566, hence O*H bond dipole 1.49 D. (b) For H S2 , we do not know the bond angle. We shall represent this bond angle as 2:. Using a similar procedure to that described in part (a), above, a diagram can be constructed and the angle 2 : calculated as follows: cos : 1 (0.93D) 2 0.67 D 0.694 : 46.056 or 2: 92.1 6 The H*S*H angle is approximately 926.5 (c) sin (<) = 0.25 D 1.87 D <5= 7.6o Molecule and associated individual bond dipoles Relationship between dipole moment(molecular) and bond dipoles(Vector addition) Geometric Relationship 1.87 D 0.23 D C Cl < o Mathematical solution: 1.87 D 0.23 D C H ClCl Cl (90 + <) o < o =C-H + 3(=C-Cl) 1.04 D 0.30 D + 3(x) 1.04 D x 0.25 D =C-Cl C H ClCl Cl 0.3 D 1.87 D 1.87 D 1.87 D The H-C-Cl bond angle is (90 + <)o = 90o + 7.6 o = 97.6o 52o 52o 1. 84 D 76o 52o 52o 104o 38o 38o 0. 93 D 0.67 D 0 .6 7 D 90 o : 0 .6 7 D : : :
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