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Chapter 8: Problem 30

Without using Fig. \(8.3\), predict which bond in each of the following groups will be the most polar. a. \(\mathrm{C}-\mathrm{H}, \mathrm{Si}-\mathrm{H}, \mathrm{Sn}-\mathrm{H}\) b. \(\mathrm{Al}-\mathrm{Br}, \mathrm{Ga}-\mathrm{Br}, \mathrm{In}-\mathrm{Br}, \mathrm{Tl}-\mathrm{Br}\) c. \(\mathrm{C}-\mathrm{O}\) or \(\mathrm{Si}-\mathrm{O}\) d. \(\mathrm{O}-\mathrm{F}\) or \(\mathrm{O}-\mathrm{Cl}\)

Short Answer

Expert verified
The most polar bonds in each group are: a. C-H b. Al-Br c. C-O d. O-F

Step by step solution

01

Review the concept of polarity

Polarity occurs when there is an unequal sharing of electrons between atoms in a molecule or a bond. This results in a slightly positive charge on one atom and a slightly negative charge on another. The larger the difference in electronegativity, the more polar the bond.
02

Identify the trends in electronegativity

Electronegativity generally increases across a period from left to right and decreases down a group. So, as we move from left to right or up a group in the periodic table, the elements become more electronegative. Now, let's apply this knowledge to the given bonds.
03

Predict the most polar bond for group a

For group a, we have the bonds C-H, Si-H, and Sn-H. As we move from C to Si to Sn down group 14 of the periodic table, the electronegativity of the element decreases. Since H has constant electronegativity, the bond with the largest difference in electronegativity will be the most polar. Therefore, the most polar bond in group a is C-H.
04

Predict the most polar bond for group b

For group b, we have the bonds Al-Br, Ga-Br, In-Br, and Tl-Br. As we move down group 13 of the periodic table from Al to Tl, the electronegativity decreases. Since Br has constant electronegativity, the bond with the largest difference in electronegativity is the most polar. Therefore, the most polar bond in group b is Al-Br.
05

Predict the most polar bond for group c

For group c, we need to compare the polarity of the bonds C-O and Si-O. As we move from C to Si down group 14 of the periodic table, the electronegativity decreases. Since O has constant electronegativity, the bond with the largest difference in electronegativity is the most polar. Therefore, the most polar bond in group c is C-O.
06

Predict the most polar bond for group d

For group d, we need to compare the polarity of the bonds O-F and O-Cl. As we move from F to Cl down group 17 of the periodic table, the electronegativity decreases. Since O has constant electronegativity, the bond with the largest difference in electronegativity is the most polar. Therefore, the most polar bond in group d is O-F. In conclusion, the most polar bonds in each group are: a. C-H b. Al-Br c. C-O d. O-F

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Most popular questions from this chapter

What is the electronegativity trend? Where does hydrogen fit into the electronegativity trend for the other elements in the periodic table?

For each of the following, write an equation that corresponds to the energy given. a. lattice energy of \(\mathrm{NaCl}\) b. lattice energy of \(\mathrm{NH}_{4} \mathrm{Br}\) c. lattice energy of \(\mathrm{MgS}\) d. \(\mathrm{O}=\mathrm{O}\) double bond energy beginning with \(\mathrm{O}_{2}(g)\) as a reactant

Use the formal charge arguments to rationalize why \(\mathrm{BF}_{3}\) would not follow the octet rule.

Write Lewis structures that obey the octet rule (duet rule for H) for each of the following molecules. a. \(\mathrm{H}_{2} \mathrm{CO}\) b. \(\mathrm{CO}_{2}\) c. \(\mathrm{HCN}\) Carbon is the central atom in all of these molecules.

Consider the following: \(\operatorname{Li}(s)+\frac{1}{2} \mathrm{I}_{2}(g) \rightarrow \operatorname{LiI}(s) \Delta H=\) \(-292 \mathrm{~kJ} . \mathrm{LiI}(s)\) has a lattice energy of \(-753 \mathrm{~kJ} / \mathrm{mol}\). The ionization energy of \(\operatorname{Li}(g)\) is \(520 . \mathrm{kJ} / \mathrm{mol}\), the bond energy of \(\mathrm{I}_{2}(g)\) is \(151 \mathrm{~kJ} / \mathrm{mol}\), and the electron affinity of \(\mathrm{I}(g)\) is \(-295 \mathrm{~kJ} / \mathrm{mol}\). Use these data to determine the heat of sublimation of \(\operatorname{Li}(s)\).
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