Name ______________________________ Class ___________________ Date __________________
Chapter 6 Practice Test: Chemical Bonding
In the space provided, write the letter of the term or phrase that best completes
each statement or best answers each question.
_____ 1. The charge on an ion is
a. always positive.
b. always negative.
c. either positive or negative.
d. zero.
_____ 2. According to the octet rule, a calcium atom has a tendency to
a. lose one electron.
b. lose two electrons.
c. gain one electron.
d. gain two electrons.
_____ 3. If a compound forms by ionic bonding, which is not true?
a. A positively charged atom or group of atoms attracts a negatively
charged atom or group of atoms.
b. The net charge of the compound is zero.
c. The compound contains just two atoms, each of opposite charge.
d. Several ions group together in a tightly packed structure.
_____ 4. The only property listed that is not characteristic of ionic compounds is
a. high melting point.
b. hardness.
c. lack of crystal structure.
d. good conductor of electricity.
_____ 5. Which formula listed below represents a polyatomic ion?
a. NH4+
b. H2SO4
c. NaCl
d. H2O
_____ 6. The melting points of ionic compounds are higher than the melting
points of molecular compounds because
a. ionic substances tend to vaporize at room temperature.
b. ionic substances are brittle.
c. attractive forces between ions are greater than the attractive forces
between molecules.
d. the numbers of positive and negative charges are equal in an ionic
compound.
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Modern Chemistry
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Chapter 6 Practice Test
Name ______________________________ Class ___________________ Date __________________
_____ 7. A covalent bond is formed when two atoms
a. share an electron with each other.
b. share one or more pairs of electrons with each other.
c. gain electrons.
d. gain and lose electrons.
_____ 8.Two atoms will likely form a polar covalent bond if the
electronegativity difference is
a. 0.1.
b. 1.0.
c. 2.5.
d. 4.0.
_____ 9. In which of these compounds is the bond between the atoms not a
nonpolar covalent bond?
a. Cl2
b. H2
c. HCl
d. O2
_____ 10. As the electronegativity difference between bonded atoms decreases,
the bond becomes more
a. covalent.
b. ionic.
c. metallic.
d. Both (b) and (c)
_____ 11. Lattice energy is an indication of the
a. strength of an ionic bond.
b. number of ions in a crystal.
c. strength of a metallic bond.
d. strength of a covalent bond.
_____ 12.Which is the correct Lewis structure for SiF4?
a.
b.
c.
d.
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
47
Chapter 6 Practice Test
Name ______________________________ Class ___________________ Date __________________
_____ 13.Which is the correct Lewis structure for C2H4?
a.
b.
c.
d.
PART II
Write the correct term (or terms) in the space provided.
14. A covalent bond in which the bonded atoms have an unequal attraction for the
shared electrons is called a(n) _______________________.
15. A molecule containing two atoms is called a(n) _______________________.
16. The degree to which bonding between atoms of two different elements is ionic
or covalent can be determined from the differences in the
_______________________ of the elements.
17. A neutral group of atoms held together by covalent bonds is called a(n)
_______________________.
18. The electron dot notation for a neon atom is _______________________.
19. A shorthand representation of the composition of a substance using atomic
symbols and numerical subscripts is called a(n) _______________________.
20. A charged group of covalently bonded atoms is called a(n)
_______________________.
21. A covalent bond between two atoms produced by sharing two pairs of
electrons is called a(n) _______________________.
22. The simplest collection of atoms from which the formula of an ionic
compound can be established is called a(n)_______________________.
23. A chemical bond that results from the attraction between metal atoms and the
surrounding sea of electrons is called a(n) _______________________.
24. The property of being able to be drawn, pulled, or extruded through a small
opening to produce a wire is called _______________________.
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Modern Chemistry
48
Chapter 6 Practice Test
Name ______________________________ Class ___________________ Date __________________
PART III Draw the Lewis structures for the following substances in the space
provided. Use VESPR theory to predict the molecular shape of the following
molecules.
25. nitrogen molecule, N2
28. phosphorous trihidride, PH3
26. hydrogen chloride, HCl
29. boron trichloride, BCl3
27. carbon tetraiodide, CI4
30.
water molecule, H2O
PART IV Use electron-dot structures to show the formation of ionic compounds
involving the following elements. Label cation and anion.
31. Na and S
32. Ca and Cl
PART V Classify each compound as ionic or covalent.
33. Water (H2) _____________________________
34. Sulfur dichloride (SCl2) ______________________________
35. Magnesium chloride (MgCl2) ____________________________
36. Iron (II) oxide (FeO) ______________________________________
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
49
Chapter 6 Practice Test