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Chapter 9: Problem 38

Classify these bonds as ionic, polar covalent, or covalent, and give your reasons: (a) the SiSi bond in \(\mathrm{Cl}_{3} \mathrm{SiSiCl}_{3},\) (b) the \(\mathrm{SiCl}\) bond in \(\mathrm{Cl}_{3} \mathrm{SiSiCl}_{3},\) (c) the CaF bond in \(\mathrm{CaF}_{2},\) (d) the \(\mathrm{NH}\) bond in \(\mathrm{NH}_{3}\).

Short Answer

Expert verified
The SiSi bond in \(\mathrm{Cl}_{3} \mathrm{SiSiCl}_{3}\) is covalent, the SiCl bond in \(\mathrm{Cl}_{3} \mathrm{SiSiCl}_{3}\) is polar covalent, the CaF bond in \(\mathrm{CaF}_{2}\) is ionic, and the NH bond in \(\mathrm{NH}_{3}\) is polar covalent.

Step by step solution

01

The SiSi bond in \(\mathrm{Cl}_{3} \mathrm{SiSiCl}_{3}\)

The electronegativity values required here are those of silicon (Si). Silicon has an electronegativity of 1.8. The electronegativity difference between the two silicon atoms is 1.8 - 1.8 = 0 which falls within the range for a covalent bond. Therefore, the SiSi bond in \(\mathrm{Cl}_{3} \mathrm{SiSiCl}_{3}\) is covalent.
02

The SiCl bond in \(\mathrm{Cl}_{3} \mathrm{SiSiCl}_{3}\)

The electronegativity values required here are those of silicon (Si) and chlorine (Cl). Silicon has an electronegativity of 1.8, while chlorine's electronegativity is 3.0. The electronegativity difference is 3.0 - 1.8 = 1.2, which falls within the range for a polar covalent bond. Therefore, the SiCl bond in \(\mathrm{Cl}_{3} \mathrm{SiSiCl}_{3}\) is a polar covalent bond.
03

The CaF bond in \(\mathrm{CaF}_{2}\)

The electronegativity values required here are those of calcium (Ca) and fluorine (F). Calcium's electronegativity value is 1.0, while that of fluorine is 3.98. The electronegativity difference is 3.98 - 1.0 = 2.98, which falls in the range of an ionic bond. Therefore, the CaF bond in \(\mathrm{CaF}_{2}\) is ionic.
04

The NH bond in \(\mathrm{NH}_{3}\)

The electronegativity values required here are those of nitrogen (N) and hydrogen (H). Nitrogen's electronegativity value is 3.04, while that of hydrogen is 2.20. The electronegativity difference is 3.04 - 2.20 = 0.84, which falls in the range of a polar covalent bond. Therefore, the NH bond in \(\mathrm{NH}_{3}\) is polar covalent.

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Most popular questions from this chapter

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

Which of these molecules has the shortest nitrogento-nitrogen bond? Explain. $$ \begin{array}{llll} \mathrm{N}_{2} \mathrm{H}_{4} & \mathrm{~N}_{2} \mathrm{O} & \mathrm{N}_{2} & \mathrm{~N}_{2} \mathrm{O}_{4} \end{array} $$

Write Lewis structures for these four isoelectronic species: (a) CO, (b) \(\mathrm{NO}^{+},\) (c) \(\mathrm{CN}^{-},\) (d) \(\mathrm{N}_{2}\). Show formal charges.

What is a coordinate covalent bond? Is it different from a normal covalent bond?

Give an example of an ion or molecule containing Al that (a) obeys the octet rule, (b) has an expanded octet, and (c) has an incomplete octet.
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