Molecular Shapes Lesson Review
(from textbook: questions on p. 297; answers on p. 321; * extra questions not in textbook)
10.13 Predict the shape of a molecule with each of the following:
a. two bonded atoms and no lone pairs
b. three bonded atoms and one lone pair
*c. three bonded atoms and no lone pairs
*d. two bonded atoms and one lone pair
*e. two bonded atoms and two lone pairs
*f. four bonded atoms and no lone pairs
*g. one bonded atom and three lone pairs
10.15 In the molecule PCl3, the four electron groups 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 group geometry?
10.17 Compare the electron-dot formulas of BF3 and NF3. Why do these molecules have different shapes?
10.19 Use VSEPR theory to predict the shape of each molecule:
a. GaH3
d. CCl4
b. OF2
e. SeO2
c. HCN
10.21 Draw the electron-dot formula and predict the shape for each polyatomic ion:
a. CO32-
b. SO42-
c. BH4-
d. NO2+