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Chapter 8: Problem 20

Give one example of a compound having a linear molecular structure that has an overall dipole moment (is polar) and one example that does not have an overall dipole moment (is nonpolar). Do the same for molecules that have trigonal planar and tetrahedral molecular structures.

Short Answer

Expert verified
Polar and nonpolar examples for different molecular structures: - Linear: Polar - \(HCl\) (Hydrogen chloride), Nonpolar - \(O_2\) (Oxygen) - Trigonal Planar: Polar - \(SO_3\) (Sulfur trioxide), Nonpolar - \(BF_3\) (Boron trifluoride) - Tetrahedral: Polar - \(CH_3Cl\) (Chloromethane), Nonpolar - \(CH_4\) (Methane)

Step by step solution

01

Linear Molecular Structure

For a linear molecular structure, the atoms are arranged in a straight line, such as diatomic molecules or molecules with two bonds to a central atom. Example of a polar molecule with a linear molecular structure: \(HCl\) (Hydrogen chloride) Example of a nonpolar molecule with a linear molecular structure: \(O_2\) (Oxygen)
02

Trigonal Planar Molecular Structure

In a trigonal planar molecular structure, three atoms are bonded to a central atom to form a flat, three-sided shape. Example of a polar molecule with a trigonal planar molecular structure: \(SO_3\) (Sulfur trioxide) Example of a nonpolar molecule with a trigonal planar molecular structure: \(BF_3\) (Boron trifluoride)
03

Tetrahedral Molecular Structure

In a tetrahedral molecular structure, four atoms are bonded to a central atom in a shape resembling a pyramid with a triangular base. Example of a polar molecule with a tetrahedral molecular structure: \(CH_3Cl\) (Chloromethane) Example of a nonpolar molecule with a tetrahedral molecular structure: \(CH_4\) (Methane)

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Most popular questions from this chapter

The space shuttle orbiter utilizes the oxidation of methyl hydrazine by dinitrogen tetroxide for propulsion: \(5 \mathrm{~N}_{2} \mathrm{O}_{4}(g)+4 \mathrm{~N}_{2} \mathrm{H}_{3} \mathrm{CH}_{3}(g) \longrightarrow 12 \mathrm{H}_{2} \mathrm{O}(g)+9 \mathrm{~N}_{2}(g)+4 \mathrm{CO}_{2}(g)\) Use bond energies to estimate \(\Delta H\) for this reaction. The structures for the reactants are:

Use the following data to estimate \(\Delta H_{\mathrm{f}}^{\circ}\) for magnesium fluoride. $$ \mathrm{Mg}(s)+\mathrm{F}_{2}(g) \longrightarrow \mathrm{MgF}_{2}(s) $$ $$ \begin{array}{lr} \text { Lattice energy } & -2913 \mathrm{~kJ} / \mathrm{mol} \\ \text { First ionization energy of } \mathrm{Mg} & 735 \mathrm{~kJ} / \mathrm{mol} \\ \text { Second ionization energy of } \mathrm{Mg} & 1445 \mathrm{~kJ} / \mathrm{mol} \\ \text { Electron affinity of } \mathrm{F} & -328 \mathrm{~kJ} / \mathrm{mol} \\\ \text { Bond energy of } \mathrm{F}_{2} & 154 \mathrm{~kJ} / \mathrm{mol} \\ \text { Enthalpy of sublimation for } \mathrm{Mg} & 150 . \mathrm{kJ} / \mathrm{mol} \end{array} $$

Without using Fig. 8.3, predict which bond in each of the following groups will be the most polar. a. \(\mathrm{C}-\mathrm{F}, \mathrm{Si}-\mathrm{F}, \mathrm{Ge}-\mathrm{F}\) b. \(\mathrm{P}-\mathrm{Cl}\) or \(\mathrm{S}-\mathrm{Cl}\) c. \(\mathrm{S}-\mathrm{F}, \mathrm{S}-\mathrm{Cl}, \mathrm{S}-\mathrm{Br}\) d. \(\mathrm{Ti}-\mathrm{Cl}, \mathrm{Si}-\mathrm{Cl}, \mathrm{Ge}-\mathrm{Cl}\)

What do each of the following sets of compounds/ions have in common with each other? See your Lewis structures for Exercises 107 through 110 . a. \(\mathrm{XeCl}_{4}, \mathrm{XeCl}_{2}\) b. \(\mathrm{ICl}_{5}, \mathrm{TeF}_{4}, \mathrm{ICl}_{3}, \mathrm{PCl}_{3}, \mathrm{SCl}_{2}, \mathrm{SeO}_{2}\)

Predict the molecular structure (including bond angles) for each of the following. a. \(\mathrm{SeO}_{3}\) b. \(\mathrm{SeO}_{2}\)
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