Problem 58
For each of the following bonds, indicate the positive end with \(\delta^{+}\) and the negative end with \(\delta\). Draw an arrow to show the dipole for each. a. \(\mathrm{N}-\mathrm{F}\) b. \(\mathrm{Si}-\mathrm{Br}\) c. \(\mathrm{C}-\mathrm{O}\) d. \(\mathrm{P}-\mathrm{Br}\) e. \(\mathrm{N}-\mathrm{P}\)
Problem 59
Predict the shape of a molecule with each of the following: a. two bonded atoms and two lone pairs b. three bonded atoms and one lone pair
Problem 60
Predict the shape of a molecule with each of the following: a. three bonded atoms and no lone pairs b. two bonded atoms and one lone pair
Problem 61
In the molecule \(\mathrm{PCl}_{3}\), the four electron pairs around the phosphorus atom are arranged in a tetrahedral geometry. However, the shape of the molecule is called trigonal pyramidal. Why does the shape of the molecule have a different name from the name of the electron pair geometry?
Problem 62
In the molecule \(\mathrm{H}_{2} \mathrm{~S}\), the four electron pairs around the sulfur atom are arranged in a tetrahedral geometry. However, the shape of the molecule is called bent. Why does the shape of the molecule have a different name from the name of the electron pair geometry?
Problem 63
Compare the electron-dot formulas of \(\mathrm{PH}_{3}\) and \(\mathrm{NH}_{3}\). Why do these molecules have the same shape?
Problem 66
Use VSEPR theory to predict the shape of each of the following: a. \(\mathrm{NCl}_{3}\) b. \(\mathrm{OBr}_{2}\) c. \(\mathrm{SiF}_{2} \mathrm{Cl}_{2}\) d. \(\mathrm{BeBr}_{2}\)
Problem 67
The molecule \(\mathrm{Cl}_{2}\) is nonpolar, but \(\mathrm{HCl}\) is polar. Explain.
Problem 68
The molecules \(\mathrm{CH}_{4}\) and \(\mathrm{CH}_{3} \mathrm{Cl}\) both contain four bonds. Why is \(\mathrm{CH}_{4}\) nonpolar whereas \(\mathrm{CH}_{3} \mathrm{Cl}\) is polar?
Problem 69
Identify each of the following molecules as polar or nonpolar: a. HBr b. \(\mathrm{NF}_{3}\) c. \(\mathrm{CHF}_{3}\)
