5 Steps to a 5 AP Chemistry 2019

160 ❯ STEP 4. Review the Knowledge You Need to Score High

❯ Review Questions

Use these questions to review the content of this chapter and practice for the AP Chemistry

exam. First are 20 multiple-choice questions similar to what you will encounter in Section I

of the AP Chemistry exam. Following those is a long free-response question like the ones

in Section II of the exam. To make these questions an even more authentic practice for the

actual exam, time yourself following the instructions provided.

Multiple-Choice Questions

Answer the following questions in 30 minutes. You may not use a calculator. You may use

the periodic table and the equation sheet at the back of this book.

1. VSEPR predicts an SbF 5 molecule will be which
   of the following shapes?
   (A) tetrahedral
   (B) trigonal bipyramidal
   (C) square pyramid
   (D) trigonal planar


2. The shortest bond would be present in which of
   the following substances?
   (A) I 2
   (B) CO
   (C) CCl 4
   (D) O 22 -


3. Which of the following does not have one or
   more p bonds?
   (A) H 2 O
   (B) HNO 3
   (C) O 2
   (D) N 2
   4. Which of the following is nonpolar?
   (A) IF 5
   (B) IF 3
   (C) SiF 4
   (D) SeF 4
   5. Resonance structures are necessary to describe the
   bonding in which of the following?
   (A) H 2 O
   (B) ClF 3
   (C) HNO 3
   (D) CH 4
   For questions 6 and 7, pick the best choice from
   the following:
   (A) ionic bonds
   (B) hybrid orbitals
   (C) resonance structures
   (D) van der Waals attractions
   6. An explanation of the equivalent bond lengths of
   the nitrite ion is:
   7. Most organic substances have low melting points.
   This may be because, in most cases, the intermo-
   lecular forces are:


4. In using the VSEPR theory, when going from the electron-group geometry to the
   molecular geometry, start with the electron-group geometry; make the nonbonding
   electrons mentally invisible; and then describe what is left.


5. When adding electrons to the molecular orbitals, remember: lowest energy first. On
   orbitals with equal energies, half fill and then pair up.


6. When writing Lewis structures of polyatomic ions, don’t forget to show the charge.


7. When you draw resonance structures, you can move only electrons (bonds). Never
   move the atoms.


8. When answering questions, the stability of the noble-gas configurations is a result, not
   an explanation. Your answers will require an explanation, i.e., lower energy state.