Week 10 Chemistry Homework - 10.19 List the following...

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Week 10 Chemistry Homework 9.37 Four atoms are arbitrarily labeled D, E, F, G. Their electronegativities are as follows: D= 3.8, E = 3.3, F = 2.8, and G = 1.3. If the atoms of these elements form the molecules DE, DG, EG, and DF, how would you arrange these molecules in order of increasing covalent bond character? Answer: Subtract the electronegativities for each element with the following results. DE = .5, DG = 2.5, EG = 2.0 and DF = 1.0 thus the answer is: DE, DF, EG, DG 9.67 From the following data, calculate the average bond energy for the N---H bond: NH<sub>3</sub>(<i>g</i>) ---> NH<sub>2</sub>(<i>g</i>) + H(<i>g</i>) &Delta;H<sup>o</sup> = 435 kJ NH<sub>2</sub>(<i>g</i>) ---> NHi>g</i>) + H(<i>g</i>) &Delta;H<sup>o</ sup> = 381 kJ NH(<i>g</i>) ---> N(<i>g</i>) + H(<i>g</i>) &Delta;H<sup>o</sup> = 360 kJ Answer: Average the 3 bond energies to achieve the average bond energy. (435kJ + 381kJ + 360kJ) / 3 = 392kJ
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Unformatted text preview: 10.19 List the following molecules in order of increasing dipole moment: H<sub>2</sub>O, CBr<sub>4</sub>, H<sub>2</sub>S, HF, NH<sub>3</sub>, CO<sub>2</sub>. Answer: Based on Table 10.3 the order would be H<sub>2</sub>S, NH<sub>3</sub>, H<sub>2</sub>O, HF this leaves CO<sub>2</sub>, and CBr<sub>4</sub> to be included. Based on Linear arrangement CO<sub>2</sub> has no dipole moment as for CBr<sub>4</sub> it has the smallest covalent bond characteristic and thus it has the second lowest dipole moment. CO<sub>2</sub>, CBr<sub>4</sub>, H<sub>2</sub>S, NH<sub>3</sub>, H<sub>2</sub>O, HF 10.21 Which of the following molecules has a higher dipole moment? Answer: molecule (a) has some dipole moment vectors going towards each other and others moving apart. On molecule (b) all dipole moment is in the identical direction thus it would have the higher dipole moment. (b)...
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