Download Ionic Compounds Practice Test

Ionic Compounds Practice Test
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. Mendeleev left spaces in his periodic table and predicted the existence of three elements and their
a. atomic numbers.
c. properties.
b. colors.
d. radioactivity.
____
2. Mendeleev did not always list elements in his periodic table in order of increasing atomic mass because he
grouped together elements with similar
a. properties.
c. densities.
b. atomic numbers.
d. colors.
____
3. The periodic table
a. permits the properties of an element to be predicted before the element is discovered.
b. will be completed with element 118.
c. has been of little use to chemists since the early 1900s.
d. was completed with the discovery of the noble gases.
____
4. Argon, krypton, and xenon are
a. alkaline earth metals.
b. noble gases.
c. actinides.
d. lanthanides.
____
5. The periodic law states that the physical and chemical properties of elements are periodic functions of their
atomic
a. masses.
c. radii.
b. numbers.
d. charges.
____
6. The periodic law states that
a. no two electrons with the same spin can be found in the same place in an atom.
b. the physical and chemical properties of the elements are functions of their atomic
numbers.
c. electrons exhibit properties of both particles and waves.
d. the chemical properties of elements can be grouped according to periodicity but physical
properties cannot.
____
7. The most reactive group of the nonmetals is the
a. lanthanides.
c. halogens.
b. transition elements.
d. noble gases.
____
8. The most characteristic property of the noble gases is that they
a. have low boiling points.
b. are radioactive.
c. are gases at ordinary temperatures.
d. are largely unreactive.
____
9. The energy required to remove an electron from an atom is the atom's
a. electron affinity.
c. electronegativity.
b. electron energy.
d. ionization energy.
____ 10. The element that has the greatest electronegativity is
a. oxygen.
b. sodium.
____ 11. A negative ion is known as a(n)
a. ionic radius.
b. valence electron.
c. chlorine.
d. fluorine.
c. cation.
d. anion.
____ 12. Across a period in the periodic table, atomic radii
a. gradually decrease.
b. gradually decrease, then sharply increase.
c. gradually increase.
d. gradually increase, then sharply decrease.
____ 13. The number of valence electrons in Group 17 elements is
a. 7.
c. 17.
b. 8.
d. equal to the period number.
____ 14. The electrostatic attraction between positively charged nuclei and negatively charged electrons permits two
atoms to be held together by a(n)
a. chemical bond.
c. neutron.
b. London force.
d. ion.
____ 15. As atoms bond with each other, they
a. increase their potential energy, thus creating less-stable arrangements of matter.
b. decrease their potential energy, thus creating less-stable arrangements of matter.
c. increase their potential energy, thus creating more-stable arrangements of matter.
d. decrease their potential energy, thus creating more-stable arrangements of matter.
____ 16. The ions in most ionic compounds are organized into a
a. molecule.
c. polyatomic ion.
b. Lewis structure.
d. crystal.
____ 17. The lattice energy is a measure of the
a. strength of an ionic bond.
b. strength of a metallic bond.
c. strength of a covalent bond.
d. net charge on a crystal.
____ 18. The properties of both ionic and molecular compounds are related to the
a. lattice energies of the compounds.
b. strengths of attraction between the particles in the compounds.
c. number of covalent bonds each contains.
d. mobile electrons that they contain.
____ 19. Compared with nonmetals, the number of valence electrons in metals is generally
a. smaller.
c. about the same.
b. greater.
d. almost triple.
____ 20. In metallic bonds, the mobile electrons surrounding the positive ions are called a(n)
a. Lewis structure.
c. electron cloud.
b. electron sea.
d. dipole.
____ 21. If a material can be shaped or extended by physical pressure, such as hammering, which property does the
material have?
a. conductivity
c. ductility
b. malleability
d. luster
____ 22. What is the formula for zinc fluoride?
a. ZnF
b. ZnF2
c. Zn2F
d. Zn2F3
____ 23. What is the formula for the compound formed by calcium ions and chloride ions?
a. CaCl
c. CaCl3
b. Ca2Cl
d. CaCl2
____ 24. What is the formula for the compound formed by lead(II) ions and chromate ions?
a. PbCrO4
c. Pb2(CrO4)3
b. Pb2CrO4
d. Pb(CrO4)2
____ 25. What is the formula for aluminum sulfate?
a. AlSO4
b. Al2SO4
c. Al2(SO4)3
d. Al(SO4)3
____ 26. The oxidation number of fluorine is
a. always 0.
b. –1 in all compounds.
c. +1 in all compounds.
d. equal to the negative charge of all the metal ions in a compound.
____ 27. In a compound, the algebraic sum of the oxidation numbers of all atoms equals
a. 0.
c. 8.
b. 1.
d. the charge on the compound.
____ 28. What is the formula mass of magnesium chloride, MgCl2?
a. 46 amu
c. 95.21 amu
b. 59.76 amu
d. 106.35 amu
____ 29. The molar mass of NO2 is 46.01 g/mol. How many moles of NO2 are present in 114.95 g?
a. 0.4003 mol
c. 2.498 mol
b. 1.000 mol
d. 114.95 mol
____ 30. The molar mass of H2O is 18.02 g/mol. How many grams of H2O are present in 0.20 mol?
a. 0.2 g
c. 35.9 g
b. 3.6 g
d. 89.9 g
____ 31. What is the mass of 0.240 mol glucose, C6H12O6?
a. 24.0 g
c. 180.16 g
b. 43.2 g
d. 750. g
____ 32. What is the percentage composition of CO?
a. 50% C, 50% O
b. 12% C, 88% O
c. 25% C, 75% O
d. 43% C, 57% O
____ 33. The percentage composition of sulfur in SO2 is about 50%. What is the percentage of oxygen in this
compound?
a. 25%
c. 75%
b. 50%
d. 90%
____ 34. What is the mass percentage of OH– in Ca(OH)2?
a. 45.9%
c. 75%
b. 66.6%
d. 90.1%
Short Answer
1. In terms of the periodic law, explain which two of these elements are most similar: sodium (element 11),
phosphorus (element 15), and sulfur (element 16).
2. What can you predict about the properties of xenon and helium, both in Group 18 in the periodic table? Why?
3. Why do most atoms form chemical bonds?
4. Explain why metals are good conductors of electricity.
Essay
1. Explain nuclear charge and how it affects the general trend in radii of atoms of elements going from left to
right across a period in the periodic table.
Completion
Complete each statement.
1. The name and formula for the compound formed by strontium ions and sulfite ions are
____________________.
2. The name for the
ion is ____________________.
Problem
1. The molar mass of aluminum is 26.98 g/mol and the molar mass of fluorine is 19.00 g/mol. Calculate the
molar mass of aluminum trifluoride, AlF3.
2. The molar mass of iron is 55.85 g/mol, the molar mass of silicon is 28.08 g/mol, and the molar mass of
oxygen is 16.00 g/mol. Calculate the molar mass of iron(II) silicate, Fe2SiO4.
3. The molar mass of aluminum is 26.98 g/mol and the molar mass of oxygen is 16.00 g/mol. Determine the
molar mass of Al2O3.
Ionic Compounds Practice Test
Answer Section
MULTIPLE CHOICE
1. ANS:
REF:
2. ANS:
REF:
3. ANS:
REF:
4. ANS:
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5. ANS:
REF:
6. ANS:
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7. ANS:
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8. ANS:
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9. ANS:
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10. ANS:
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11. ANS:
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12. ANS:
REF:
13. ANS:
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14. ANS:
REF:
15. ANS:
REF:
16. ANS:
REF:
17. ANS:
REF:
18. ANS:
REF:
19. ANS:
REF:
20. ANS:
REF:
21. ANS:
REF:
C
PTS: 1
DIF:
cb766065-f97e-11de-9c72-001185f0d2ea
A
PTS: 1
DIF:
cb78e9d2-f97e-11de-9c72-001185f0d2ea
A
PTS: 1
DIF:
cb7fe9d9-f97e-11de-9c72-001185f0d2ea
B
PTS: 1
DIF:
cb873800-f97e-11de-9c72-001185f0d2ea
B
PTS: 1
DIF:
cb89734d-f97e-11de-9c72-001185f0d2ea
B
PTS: 1
DIF:
cb8e5f17-f97e-11de-9c72-001185f0d2ea
C
PTS: 1
DIF:
cbcc3579-f97e-11de-9c72-001185f0d2ea
D
PTS: 1
DIF:
cbd0fa33-f97e-11de-9c72-001185f0d2ea
D
PTS: 1
DIF:
cbd8485a-f97e-11de-9c72-001185f0d2ea
D
PTS: 1
DIF:
cbe1aabe-f97e-11de-9c72-001185f0d2ea
D
PTS: 1
DIF:
cbe40d1b-f97e-11de-9c72-001185f0d2ea
A
PTS: 1
DIF:
cbeb3432-f97e-11de-9c72-001185f0d2ea
A
PTS: 1
DIF:
cbfe6e2a-f97e-11de-9c72-001185f0d2ea
A
PTS: 1
DIF:
cc13bc5f-f97e-11de-9c72-001185f0d2ea
D
PTS: 1
DIF:
cc188119-f97e-11de-9c72-001185f0d2ea
D
PTS: 1
DIF:
cc51b9d1-f97e-11de-9c72-001185f0d2ea
A
PTS: 1
DIF:
cc54433e-f97e-11de-9c72-001185f0d2ea
B
PTS: 1
DIF:
cc5dccb2-f97e-11de-9c72-001185f0d2ea
A
PTS: 1
DIF:
cc64f3c9-f97e-11de-9c72-001185f0d2ea
B
PTS: 1
DIF:
cc699173-f97e-11de-9c72-001185f0d2ea
B
PTS: 1
DIF:
cc6e7d3d-f97e-11de-9c72-001185f0d2ea
I
OBJ: 1
I
OBJ: 1
I
OBJ: 2
I
OBJ: 2
I
OBJ: 3
I
OBJ: 3
I
OBJ: 4
I
OBJ: 4
I
OBJ: 1
II
OBJ: 2
I
OBJ: 2
II
OBJ: 2
I
OBJ: 3
I
OBJ: 1
I
OBJ: 2
I
OBJ: 2
I
OBJ: 3
I
OBJ: 4
I
OBJ: 1
I
OBJ: 1
I
OBJ: 3
22. ANS: B
PTS: 1
DIF:
REF: ccb11859-f97e-11de-9c72-001185f0d2ea
23. ANS: D
PTS: 1
DIF:
REF: ccb37ab6-f97e-11de-9c72-001185f0d2ea
24. ANS: A
PTS: 1
DIF:
REF: ccb3a1c6-f97e-11de-9c72-001185f0d2ea
25. ANS: C
PTS: 1
DIF:
REF: ccb5dd13-f97e-11de-9c72-001185f0d2ea
26. ANS: B
PTS: 1
DIF:
REF: ccd01712-f97e-11de-9c72-001185f0d2ea
27. ANS: A
PTS: 1
DIF:
REF: ccd2a07f-f97e-11de-9c72-001185f0d2ea
28. ANS: C
PTS: 1
DIF:
REF: ccecda7e-f97e-11de-9c72-001185f0d2ea
29. ANS: C
Solution:
III
OBJ: 2
III
OBJ: 2
III
OBJ: 2
III
OBJ: 2
II
OBJ: 1
II
OBJ: 1
III
OBJ: 1
PTS: 1
OBJ: 2
30. ANS: B
Solution:
DIF: III
REF: ccf3da85-f97e-11de-9c72-001185f0d2ea
PTS: 1
OBJ: 2
31. ANS: B
Solution:
DIF: III
REF: ccf663f2-f97e-11de-9c72-001185f0d2ea
PTS: 1
OBJ: 2
32. ANS: D
Solution:
DIF: III
REF: ccfd63f9-f97e-11de-9c72-001185f0d2ea
PTS:
OBJ:
33. ANS:
REF:
1
DIF: III
REF: cd094fca-f97e-11de-9c72-001185f0d2ea
4
B
PTS: 1
DIF: II
cd0bd937-f97e-11de-9c72-001185f0d2ea
OBJ: 4
34. ANS: A
Solution:
PTS: 1
OBJ: 4
DIF: III
REF: cd0e1484-f97e-11de-9c72-001185f0d2ea
SHORT ANSWER
1. ANS:
Their locations in the periodic table indicate that phosphorus and sulfur are nonmetals and sodium is a metal.
Nonmetals are a group with characteristic properties, so phosphorus and sulfur are the most similar elements
of the three.
PTS: 1
DIF: III
REF: cc0a32eb-f97e-11de-9c72-001185f0d2ea
OBJ: 3
2. ANS:
In the periodic table, elements in the same column or group have similar properties. Because helium and
xenon are in the same group, they have similar properties.
PTS: 1
DIF: I
REF: cc0c9548-f97e-11de-9c72-001185f0d2ea
OBJ: 4
3. ANS:
Atoms form chemical bonds to establish a more-stable arrangement. As independent particles, they are at high
potential energy. By bonding, they decrease their potential energy, thus becoming more stable.
PTS: 1
DIF: II
REF: cc9ba314-f97e-11de-9c72-001185f0d2ea
OBJ: 2
4. ANS:
The valence electrons in a metal's structure are delocalized, so they can move freely and carry an electric
charge throughout the metal.
PTS: 1
OBJ: 3
DIF: II
REF: cca067ce-f97e-11de-9c72-001185f0d2ea
ESSAY
1. ANS:
Nuclear charge is the attraction an atomic nucleus has on the electrons surrounding it. As you move from left
to right across a period, the atomic number increases, and therefore the number of protons in the nucleus
increases. The more protons within a nucleus, the greater is the nuclear charge. A greater nuclear charge pulls
the electrons closer to the nucleus, decreasing the atomic radius.
PTS: 1
OBJ: 2
DIF: II
REF: cc0cbc58-f97e-11de-9c72-001185f0d2ea
COMPLETION
1. ANS: strontium sulfite, SrSO3
PTS: 1
DIF: III
OBJ: 3
2. ANS: chromate ion
PTS: 1
OBJ: 3
DIF: III
REF: cd3dead8-f97e-11de-9c72-001185f0d2ea
REF: cd428882-f97e-11de-9c72-001185f0d2ea
PROBLEM
1. ANS:
83.98 g/mol AlF3
Solution:
26.98 g/mol Al + (3
19.00 g/mol F) = 89.3 g/mol AlF3
PTS: 1
DIF: III
REF: cd38ff0e-f97e-11de-9c72-001185f0d2ea
OBJ: 1
2. ANS:
203.78 g/mol Fe2SiO4
Solution:
(2 55.85 g/mol Fe) + (28.08 g/mol Si) + (4 16.00 g/mol O) = 203.78 g/mol Fe2SiO4
PTS: 1
DIF: III
REF: cd3b616b-f97e-11de-9c72-001185f0d2ea
OBJ: 1
3. ANS:
101.96 g/mol Al2O3
Solution:
(2 26.98 g/mol Al) + (3 16.00 g/mol O) = 101.96 g/mol Al2O3
PTS: 1
OBJ: 1
DIF: III
REF: cd3dc3c8-f97e-11de-9c72-001185f0d2ea