Practice Exercises

The following questions are in the format that is used on the SAT Subject Area Test in Chemistry. If you are not familiar with these types of questions, study pages xiii–xvi before doing these review questions. Record your answers on a separate sheet of paper.

Directions: The following set of lettered choices refers to the numbered questions immediately below it. For each numbered item, choose the one lettered choice that fits it best and record your answer on a separate sheet of paper. Each choice in the set may be used once, more than once, or not at all.

1. 1. Questions 1–7 refer to the following terms:

      1. Ionic
      2. Nonpolar covalent
      3. Polar covalent
      4. Metallic
      5. Hydrogen bonding

   1. When the electronegativity difference between two atoms is 2, what type of bond can be predicted?

   2. If two atoms are bonded in such a way that both members of the pair equally share one electron with the other, what is the bond called?

   3. Which of the five choices is considered the weakest bond in the group?

   4. Which of the above bonds explains water’s abnormally high boiling point?

   5. If the sharing of an electron pair is unequal and the atoms have an electronegativity difference of 0.4 to 1.6, what is this type of bonding called?

   6. If an electron is lost by one atom and completely captured by another, what is this type of bond called?

   7. If one or more valence electrons become detached from the atoms and migrate in a “sea” of free electrons among the positive ions, what is this type of bonding called?

2. Directions: (Further explanation and the examples for this type of question can be found on pages xv–xvi.) Every question below contains two statements, I in the left-hand column and II in the right-hand column. For each question, decide if statement I is true or false and whether statement II is true or false, and fill in the corresponding T or F ovals in the answer spaces. *Fill in oval CE only if statement II is a correct explanation of statement I.

1. *Fill in oval CE only if II is a correct explanation of I.

   

8. I		II
   Maximum repulsion between two electron pairs in a molecular compound will result in a linear structure	BECAUSE	the VSEPR model says that like charges will orient themselves so as to diminish the repulsion between them.

9. I		II
   Sodium chloride is an example of ionic bonding	BECAUSE	sodium and chlorine have the same electronegativity.

10. I		II
    Ammonia has a trigonal pyramidal molecular structure	BECAUSE	ammonia has a tetrahedral electron pair geometry with three atoms bonded to the central atom.

11. 1. Directions: Each of the questions or incomplete statements below is followed by five suggested answers or completions. Select the one that is best in each case and record your answer on a separate sheet of paper.

    11. 1. A substance with a melting point of 420°C, that doesn’t dissolve in water, and that conducts electricity in the solid state could be
        1. CH₄
        2. NaCl
        3. Zn
        4. HF
        5. Ar
    12. 1. A substance with a boiling point of –85°C, that dissolves in water, and that produces an acid could be
        1. C₂H₄
        2. LiF
        3. HCl
        4. K
        5. Kr
    13. 1. A substance with a melting point of 730°C, that dissolves in water, and that doesn’t conduct electricity as a solid could be
        1. CaBr₂
        2. Ca
        3. Br₂
        4. He
        5. HC₂H₃O₂
    14. 1. A substance that has a melting point of 54°C, that doesn’t dissolve in water, and that is volatile in the solid state could be
        1. K₂O
        2. Ag
        3. N₂
        4. Xe
        5. C₆H₅Cl
    15. 1. Of those shown, the polar molecule is
        1. N₂O₄
        2. HBr
        3. CCl₄
        4. H₂Br
        5. CO₂
    16. 1. Which of the following molecules exhibits the hybridization known as sp?
        1. CO₂
        2. CH₄
        3. PH₃
        4. H₂S
        5. SF₆
    17. 1. Which of the following is a type of chemical bonding?
        1. Hydrogen bonding
        2. Metallic bonding
        3. Intermolecular bonding
        4. Covalent bonding
        5. Dipole–dipole bonding