Standard 3 Test
Name: ______________________
Date: _______________
Standard 3: Chemical Bonding Part 1
Circle the letter of the choice that best completes the statement or
answers the question.
1. An ionic bond is
a. an attraction of an atom for its electrons.
b. an attraction of atoms for electrons they share.
c. a force that holds two oppositely charged atoms together.
d. the movement of electrons from one atom to another.
2. The overall charge of a formula unit for an ionic compound
a. is always zero
c. is always positive
b. is always negative
d. may have any value
3. How many chloride (Cl-) ions are present in a formula unit of magnesium
chloride, given that the charge on a Mg ion is 2+?
a. one-half
c. two
b. one
d. four
4. Ionic bonds generally occur between
a. metals.
c. a metal and a nonmetal.
b. nonmetals.
d. noble gases.
5. Salts are examples of
a. nonionic compounds.
b. metals.
c. nonmetals.
d. ionic compounds.
6. In electron transfer involving a metallic atom and a nonmetallic atom during
ion formation, which of the following is correct?
a. The metallic atom gains electrons from the nonmetallic atom.
b. The nonmetallic atom gains electrons from the metallic atom.
c. Both atoms gain electrons.
d. Neither atom gains electrons.
7. The anion that has the formula ClO- is called the
a. chloride ion
c. hypochlorite ion
b. chlorate ion
d. perchlorate ion
Standard 3 Test
Name: ______________________
Date: _______________
8. Where does a subscript that indicates the number of atoms appear, relative
to a chemical symbol in a formula?
a. To the upper left
c. to the upper right
b. To the lower left
d. to the lower right
9. What is the formula of calcium phosphate, which is made up of the ions Ca2+
and PO43-?
a. Ca3PO4
c. Ca3(PO4)2
b. Ca6PO4
d. Ca2(PO4)3
10. Which of the following pairs is most likely to form an ionic compound?
a. sodium and aluminum
c. nitrogen and sulfur
b. magnesium and fluorine
d. oxygen and chlorine
11. In the formation of a covalent bond, electrons are
a. shared
c. gained
b. lost
d. transferred
12. Which of the following elements normally exists in the form of diatomic
molecules?
a. helium
c. iron
b. argon
d. nitrogen
13. Four electrons are shared in a
a. single covalent bond
b. double covalent bond
c. triple covalent bond
d. quadruple covalent bond
14. Which of the following molecules contains a triple covalent bond?
a. methane (CH4)
c. oxygen (O2)
b. carbon dioxide (CO2)
d. nitrogen (N2)
15. Which of the following pairs of elements can be joined by a covalent bond?
a. Li and Cl
c. N and C
b. Na and C
d. Mg and C
16. According to VSEPR theory, molecules adjust their shapes to keep which of
the following as far apart as possible?
a. pairs of valence electrons
c. mobile valence electrons
b. the electrons closest to the nuclei
d. inner shell electrons
Standard 3 Test
Name: ______________________
Date: _______________
17. What are the components of binary molecular compounds?
a. one metallic element and one nonmetallic element
b. two nonmetallic elements
c. two metallic elements
d. two polyatomic ions
e. two oppositely-charged ions
18. The VSEPR model is used mainly to
a. determine molecular shape
b. write resonance structures
c. determine ionic charge
d. measure intermolecular distance
19. The shape of a molecule that has two covalent single bonds and no lone pairs
on the central atom is
a. tetrahedral
c. trigonal pyramidal
b. trigonal planar
d. linear
20. Unequal sharing of electrons between two bonded atoms always indicates
a. a nonpolar covalent bond
c. a polar covalent bond
b. an ionic bond
d. a polar molecule
True or False.
21. In a chemical name, the prefix used to indicate the presence of two atoms
of a given kind is bi-.
22. The prefix hydro- is used in naming binary acids.
23. In Lewis structures, hydrogen is always a central atom.
24. The prefix tetra- indicates three atoms.
25. A ternary acid contains only two elements.
26. Resonace occurs when more than one valid Lewis structure can be written
for a molecule.
27. The electrons in a coordinate covalent bond are donated by both the bonded
atoms.
28. Delocalized (mobile) valence electrons are typical of ionic compounds.
29. In naming ionic compounds, the cation is named first.
Standard 3 Test
Name: ______________________
Date: _______________
30. Metals tend to be malleable and ductile and have relatively high melting
points.
Matching.
____ 31. ClO2-
a. hydrobromic acid
____ 32. ClO4-
b. chlorate
____ 33. ClO-
c. dinitrogen tetroxide
____ 34. Cl-
d. hypochlorite
____ 35. ClO3-
e. carbon monoxide
____ 36. CO
f. chloride
____ 37. CO2
g. nitrous acid
____ 38. H2CO3
h. perchlorate
____ 39. NH3
i. nitrogen trihydride
____ 40. N2O4
j. chlorite
____ 41. HNO2
k. nitric acid
____ 42. HNO3
l. carbonic acid
____ 43. HBr
m. carbon dioxide
Essay:
44. Explain how scientists have used metallic bonding to account for many of the
physical properties of metals such as electrical conductivity and malleability.
______________________________________________________________
______________________________________________________________
______________________________________________________________
______________________________________________________________
Standard 3 Test
Name: ______________________
Date: _______________
45. Compare the characteristics of ionic and molecular compounds.
____________________________________________________________
____________________________________________________________
____________________________________________________________
____________________________________________________________
Complete the tables:
46. Complete the following table by writing in the chemical formula for the
compounds formed by combining the indicated positive and negative ions.
K+
Mg2+
Fe3+
Sn4+
BrO2PO43CO32-
47. Write the name of the compounds formed when the following ions
combine.
Fluoride ion
Hydrogen ion
Cobalt (II) ion
Lead (IV) ion
Sulfate ion
Nitrite ion
Standard 3 Test
Name: ______________________
Date: _______________
Standard 3: Chemical Bonding Part 2
CP/Tech
The graph shows the electronegativities of the elements in periods 2 and 3 of the
periodic table, except for the noble gases. Use the graph to answer the following
questions.
F
4.0
O
3.5
3.0
Period 2
C
2.5
2.0
0.5
Cl
B
S
P
Be
1.5
1.0
N
Si
Li
Al
Period 3
Mg
Na
0.0
1
2
13
14
15
16
17
1. If two atoms of differing electronegativity are bonded covalently to each
other, what is true of the electrons they share? What type of bond results
in such a case?
____________________________________________________________
____________________________________________________________
2. How does the electronegativity of boron (B) compare with that of nitrogen
(N)? In terms of the periodic table, how are these two elements related?
Compare aluminum (Al) with phosphorus (P) in the same way.
____________________________________________________________
____________________________________________________________
Standard 3 Test
Name: ______________________
Date: _______________
3. Describe the trend in electronegativity illustrated for period-2 and period-3
elements.
____________________________________________________________
____________________________________________________________
4. How does the electronegativity of boron (B) compare with that of aluminum
(Al)? In terms of the periodic table, how are these two elements related?
Compare nitrogen (N) with phosphorus (P) in the same way.
____________________________________________________________
____________________________________________________________
5. Describe the trend in electronegativity within a group of the periodic table,
as suggested by the graph.
____________________________________________________________
____________________________________________________________
Standard 3 Test
Name: ______________________
Date: _______________
Standard 3: Chemical Bonding Part 2
Honors Applying Scientific Methods
Four students (A, B, C, and D) are given separate solid samples of the same unknown
pure substance. They are asked to determine whether the substance is a metallic
element, a nonmetallic element, or an ionic compound. In order to find out, they
independently carry out experiments to determine some of the properties of the
substance. Student A observes the substance to determine its luster. Student B
tests the solid’s ability to conduct electricity. Student C determines whether the
solid is malleable and ductile. Student D determines its melting point and tests the
melted liquid’s ability to conduct electricity. The students do not communicate
their separate findings to one another. The results of their experiments are shown
in the table below. Use the information to answer the questions that follow.
Student
A
B
C
D
D
Property Studied
Luster
Ability of a solid to
conduct electricity
Malleability and ductility
Melting point
Ability of melted liquid to
conduct electricity
Result
Nonlustrous
Nonconducting
Nonmalleable
Approximately 800C
Good
1. On the basis of his results, Student A concludes that the solid is a
nonmetallic element rather than a metallic element or an ionic compound.
Comment on the soundness of his conclusion, given only what he has
determined about luster.
____________________________________________________________
____________________________________________________________
____________________________________________________________
2. On the basis of her results, Student B also concludes that the unknown
compound is a nonmetallic element. Evaluate her conclusion.
____________________________________________________________
____________________________________________________________
Standard 3 Test
Name: ______________________
Date: _______________
3. On the basis of his results, Student C concludes that the unknown is a
metallic element. Evaluate his conclusion.
____________________________________________________________
____________________________________________________________
____________________________________________________________
4. On the basis of her results, Student D states that she cannot conclude
anything about whether the unknown is a metallic element, nonmetallic
element, or ionic solid. Evaluate her comment.
____________________________________________________________
____________________________________________________________
____________________________________________________________
____________________________________________________________
5. Suppose that Student B and Student C shared their results with each other.
Should they then be able to come to a definite conclusion as to the nature of
the unknown? Explain.
____________________________________________________________
____________________________________________________________
6. Suppose that Student B and Student D shared their results with each other.
Should they then be able to come to a definite conclusion as to the nature of
the unknown? Explain.
____________________________________________________________
____________________________________________________________
7. Would a test of a water solution of the unknown might also have been useful
in determining the nature of the unknown compound? Explain.
____________________________________________________________
____________________________________________________________