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Chapter 9: Q69P (page 375)

The energy of the C-C bond is 347 kJ/mol, and that of the Cl-Cl bond is 243 kJ/mol. Which of the following values might you expect for the C-Cl bond energy? Explain.

(a) 590 kJ/mol (sum of the values given)

(b) 104 kJ/mol (difference of the values given)

(c) 295 kJ/mol (average of the values given)

(d) 339 kJ/mol (greater than the average of the values given)

Short Answer

Expert verified

It had formed between two different atoms, carbon and chlorine, the bond between C-Cl is known as a heteronuclear bond. As a result, the bond energy is 339 kJ/mol (more significant than the average of the values given)

Step by step solution

01

Step-1: Heteronuclear bond's between C-Cl

A heteronuclear bond's bond energy is usually more significant than the mean of the two independent bonds formed by the same atoms.

That is, the sum of C-C and Cl-Cl atoms; these are referred to as homonuclear bonds.

02

Step-2: Calculation between the bonds

Hence,

C-C = 347 kj/mol

Cl-Cl = 243 kJ/mol

Average = (347 + 243) / 2 =295 kJ/mol

As a result, the bond energy must be more incredible than 295 kJ/mol.

As a result, the correct answer is D; 339 kJ/mol (greater than the average of the values given)

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Most popular questions from this chapter

Rank the members of each set of compounds in order of increasing the ionic character of their bonds. Use polar arrows to indicate the bond polarity of each:

(a) HBr, HCl, HI

(b) H2O, CH4 , HF

(c) SCI2 , PCI3 , SiCI4

Use Figure 9.20, p. 364, to indicate the polarity of each bond with partial charges

(a) Br-Cl

(b) F-Cl

(c) H-O

(d) Se-H

(e) As-H

(f) S-N.

The average C-H bond energy in CH4 is 415kJ/mol. Use table 9.2(p. 353) and the following to calculate the average C-H bond energy in ethane(C2H6;C-C bond), in ethene (C2H4;C=C bond), and ethyne (C2H2;C鈮�C):

C2H6(g)+H2(g)鈫�2CH4(g)鈥勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌�螖贬o=-65.07kJ/molC2H4(g)+2H2(g)鈫�2CH4(g)鈥勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌�螖贬o=-202kJ/molC2H2(g)+3H2(g)鈫�2CH4(g)鈥勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌勨赌�螖贬o=-376.74kJ/mol

By using photons of specific wavelengths, chemists can dissociate gaseous Hi to produce H atoms at certain speeds. When HI dissociates, the H atoms move away rapidly. Whereas the heavier I atoms move away more slowly.

  1. What is the longest wavelength (in nm) that can dissociate a molecule of HI?
  2. If a photon of 254 nm is used, what is the excess energy (in J) over that needed for dissociation?
  3. If the excess energy is carried away by the H atom as kinetic energy, what is the speed (in m/s)?

Is the H-O bond in water nonpolar covalent, polar-covalent, or ionic? Define each term, and explain your choice.
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