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Chapter 8: Problem 41

Which of the following bonds are polar? (a) \(\mathrm{C}-\mathrm{O}\) (b) \(\mathrm{Sl}-\mathrm{F},(\mathbf{c}) \mathrm{N}-\mathrm{Cl}\) (d) \(\mathrm{C}-\mathrm{Cl}\). Which is the more electronegative atom in each polar bond?

Short Answer

Expert verified
The polar bonds are (a) C-O, (b) Si-F, and (d) C-Cl. The more electronegative atoms in each polar bond are oxygen (O) in C-O, fluorine (F) in Si-F, and chlorine (Cl) in C-Cl. The N-Cl bond is nonpolar.

Step by step solution

01

Electronegativity Values

For reference, here are the electronegativity values of the atoms involved in the given bonds: - Carbon (C): 2.55 - Oxygen (O): 3.44 - Silicon (Si): 1.90 - Fluorine (F): 3.98 - Nitrogen (N): 3.04 - Chlorine (Cl): 3.16
02

Bond (a): C-O

The electronegativity difference between carbon (2.55) and oxygen (3.44) is 0.89. Since this value is greater than 0.5, the C-O bond is polar. The more electronegative atom in this bond is oxygen (O).
03

Bond (b): Si-F

The electronegativity difference between silicon (1.90) and fluorine (3.98) is 2.08. As this value is much larger than 0.5, the Si-F bond is polar. The more electronegative atom in this bond is fluorine (F).
04

Bond (c): N-Cl

The electronegativity difference between nitrogen (3.04) and chlorine (3.16) is 0.12. The difference is smaller than 0.5, so the N-Cl bond is nonpolar.
05

Bond (d): C-Cl

The electronegativity difference between carbon (2.55) and chlorine (3.16) is 0.61. Since this value is larger than 0.5, the C-Cl bond is polar. The more electronegative atom in this bond is chlorine (Cl).
06

Summary

Out of the given bonds, the polar bonds are C-O, Si-F, and C-Cl. The more electronegative atoms in each polar bond are oxygen (O) in C-O, fluorine (F) in Si-F, and chlorine (Cl) in C-Cl. The N-Cl bond is nonpolar as the electronegativity difference is smaller than 0.5.

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Most popular questions from this chapter

(a) Which of these compounds is an exception to the octet rule: carbon dioxide, water, ammonia, phosphorus trifluoride, or arsenic pentafluoride? (b) Which of these compounds or ions is an exception to the octet rule: borohydride \(\left(\mathrm{BH}_{4}^{-}\right),\) borazine $\left(\mathrm{B}_{3} \mathrm{~N}_{3} \mathrm{H}_{6},\right.$ which is analogous to benzene with alternating \(\mathrm{B}\) and \(\mathrm{N}\) in the ring \(),\) or boron trichloride?

(a) Is lattice energy usually endothermic or exothermic? (b) Write the chemical equation that represents the process of lattice energy for the case of NaCl. (c) Would you expect salts like \(\mathrm{NaCl}\), which have singly charged ions, to have larger or smaller lattice energies compared to salts like CaO which are composed of doubly-charged ions?

(a) Write the electron configuration for the element titanium, Ti. How many valence electrons does this atom possess? (b) Hafnium, Hf, is also found in group 4. Write the electron configuration for Hf. (c) Ti and Hf behave as though they possess the same number of valence electrons. Which of the subshells in the electron configuration of Hf behave as valence orbitals? Which behave as core orbitals?

State whether each of these statements is true or false. (a) The longer the bond, the stronger the bond. (b) \(\mathrm{C}-\mathrm{C}\) bonds are stronger than \(\mathrm{C}-\mathrm{F}\) bonds. (c) A typical double bond length is in the \(500-1000\) pm range. (d) Energy is required to form a chemical bond. (e) The longer the bond, the more energy is stored chemical bonds.

The substance chlorine monoxide, \(\mathrm{ClO}(g)\), is important in atmospheric processes that lead to depletion of the ozone layer. The ClO molecule has an experimental dipole moment of \(1.24 \mathrm{D},\) and the \(\mathrm{Cl}-\mathrm{O}\) bond length is \(160 \mathrm{pm} .(\mathbf{a})\) Determine the magnitude of the charges on the \(\mathrm{Cl}\) and \(\mathrm{O}\) atoms in units of the electronic charge, \(e .(\mathbf{b})\) Based on the electronegativities of the elements, which atom would you expect to have a partial negative charge in the ClO molecule? (c) Using formal charges as a guide, propose the dominant Lewis structure for the molecule. (d) The anion ClO \(^{-}\) exists. What is the formal charge on the Cl for the best Lewis structure for \(\mathrm{ClO}^{-} ?\)
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