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Chapter 9: Problem 39

Classify the following bonds as ionic, polar covalent, or covalent, and give your reasons: (a) the CC bond in \(\mathrm{H}_{3} \mathrm{CCH}_{3},\) (b) the KI bond in \(\mathrm{KI}\), (c) the \(\mathrm{NB}\) bond in \(\mathrm{H}_{3} \mathrm{NBCl}_{3}\) (d) the CF bond in \(\mathrm{CF}_{4}\).

Short Answer

Expert verified
(a) the CC bond in \(\mathrm{H}_{3} \mathrm{CCH}_{3}\) is covalent, (b) the KI bond in \(\mathrm{KI}\) is ionic, (c) the \(\mathrm{NB}\) bond in \(\mathrm{H}_{3}\mathrm{NBCl}_{3}\) is polar covalent, (d) the CF bond in \(\mathrm{CF}_{4}\) is polar covalent.

Step by step solution

01

Classify the CC bond in \(\mathrm{H}_{3} \mathrm{CCH}_{3}\)

First, determine the electronegativity values of the elements. Carbon (C) has an electronegativity of approximately 2.5. The difference in electronegativity between two carbon atoms is 0, so the bond is covalent.
02

Classify the KI bond in \(\mathrm{KI}\)

Potassium (K) has an electronegativity of approximately 0.8 and iodine (I) has an electronegativity of approximately 2.66. The difference in electronegativity is 1.86, which is greater than 1.7, so the bond is ionic.
03

Classify the NB bond in \(\mathrm{H}_{3}\mathrm{NBCl}_{3}\)

Nitrogen (N) has an electronegativity of approximately 3.04 and boron (B) has an electronegativity of approximately 2.04. The difference in electronegativity is 1, which is less than 1.7 but greater than 0.4, so the bond is polar covalent.
04

Classify the CF bond in \(\mathrm{CF}_{4}\)

Carbon (C) has an electronegativity of approximately 2.5 and fluorine (F) has an electronegativity of approximately 3.98. The difference in electronegativity is 1.48, which is less than 1.7 but greater than 0.4, so the bond is polar covalent.

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Most popular questions from this chapter

Because fluorine has seven valence electrons \(\left(2 s^{2} 2 p^{5}\right),\) seven covalent bonds in principle could form around the atom. Such a compound might be \(\mathrm{FH}_{7}\) or \(\mathrm{FCl}_{7}\). These compounds have never been prepared. Why?

In the gas phase, aluminum chloride exists as a dimer (a unit of two) with the formula \(\mathrm{Al}_{2} \mathrm{Cl}_{6}\). Its skeletal structure is given by Complete the Lewis structure and indicate the coordinate covalent bonds in the molecule.

Which of the following molecules has the shortest nitrogen-to-nitrogen bond: \(\mathrm{N}_{2} \mathrm{H}_{4}, \mathrm{~N}_{2} \mathrm{O}, \mathrm{N}_{2}, \mathrm{~N}_{2} \mathrm{O}_{4} ?\) Explain.

Among the common inhaled anesthetics are: halothane: \(\mathrm{CF}_{3} \mathrm{CHClBr}\) enflurane: CHFClCF \(_{2} \mathrm{OCHF}_{2}\) isoflurane: \(\mathrm{CF}_{3} \mathrm{CHClOCHF}_{2}\) methoxyflurane: \(\mathrm{CHCl}_{2} \mathrm{CF}_{2} \mathrm{OCH}_{3}\) Draw Lewis structures of these molecules.

From the following data, calculate the average bond enthalpy for the \(\mathrm{N}-\mathrm{H}\) bond: \(\begin{aligned} \mathrm{NH}_{3}(g) & \longrightarrow \mathrm{NH}_{2}(g)+\mathrm{H}(g) & \Delta H^{\circ} &=435 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{NH}_{2}(g) & \longrightarrow \mathrm{NH}(g)+\mathrm{H}(g) & \Delta H^{\circ} &=381 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{NH}(g) & \longrightarrow \mathrm{N}(g)+\mathrm{H}(g) & \Delta H^{\circ} &=360 \mathrm{~kJ} / \mathrm{mol} \end{aligned}\)
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