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Chemistry First Semester Review

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

 1. 

Chemistry is defined as the study of the composition and structure of materials and
a.
the categories of matter.
c.
the electrical currents in matter.
b.
the changes in matter.
d.
molecules in living things.
 

 2. 

Matter includes all of the following EXCEPT
a.
air.
c.
smoke.
b.
light.
d.
water vapor.
 

 3. 

The state of matter in which a material has definite shape and definite volume is the
a.
liquid state.
c.
gaseous state.
b.
solid state.
d.
vaporous state.
 

 4. 

The state of matter in which a material has neither a definite shape nor a definite volume is the
a.
gaseous state.
c.
elemental state.
b.
liquid state.
d.
solid state.
 
 
1st_sem_review_files/i0060000.jpg
 

 5. 

Group ____ in the figure above contains only metals.
a.
2
c.
17
b.
13
d.
18
 

 6. 

Use the figure above. Which element has properties most similar to those of sodium?
a.
boron
c.
sulfur
b.
calcium
d.
nitrogen
 

 7. 

What is the atomic number for aluminum from the figure above?
a.
13
c.
26.98
b.
14
d.
26.9815
 

 8. 

A vertical column of blocks in the periodic table is called a(n)
a.
group.
c.
property.
b.
period.
d.
octet.
 

 9. 

Which is NOT a property of metals?
a.
malleability
c.
unreactivity
b.
ability to conduct heat and electricity
d.
tensile strength
 

 10. 

The SI standard units for length and mass are
a.
centimeter and gram.
c.
centimeter and kilogram.
b.
meter and gram.
d.
meter and kilogram.
 

 11. 

The metric unit for length that is closest to the thickness of a dime is the
a.
micrometer.
c.
centimeter.
b.
millimeter.
d.
decimeter.
 

 12. 

The symbol for the metric unit used to measure mass is
a.
m.
c.
g.
b.
mm.
d.
L.
 

 13. 

The quantity of matter per unit volume is
a.
mass.
c.
inertia.
b.
weight.
d.
density.
 

 14. 

The unit m3 measures
a.
length.
c.
volume.
b.
mass.
d.
density.
 

 15. 

To determine density, the quantities that must be measured are
a.
mass and weight.
c.
volume and concentration.
b.
volume and weight.
d.
volume and mass.
 

 16. 

The density of aluminum is 2.70 g/cm3. The volume of a solid piece of aluminum is 1.50 cm3. Find its mass.
a.
1.50 g
c.
2.70 g
b.
1.80 g
d.
4.05 g
 

 17. 

The density of pure diamond is 3.5 g/cm3. The mass of a diamond is 0.25 g. Find its volume.
a.
0.071 cm3
c.
3.5 cm3
b.
0.875 cm3
d.
14 cm3
 

 18. 

If 1 inch equals 2.54 cm, how many centimeters equal 1 yard?
a.
0.07 cm
c.
36 cm
b.
14.17 cm
d.
91.4 cm
 

 19. 

Five darts strike near the center of the target. Whoever threw the darts is
a.
accurate.
c.
both accurate and precise.
b.
precise.
d.
neither accurate nor precise.
 

 20. 

For numbers less than 0.1, such as 0.06, the zeros to the right of the decimal point but before the first nonzero digit
a.
are significant.
b.
show the decimal place of the first digit.
c.
show that the zero on the left side of the decimal is not significant.
d.
show uncertainty.
 

 21. 

To two significant figures, the measurement 0.0255 g should be reported as
a.
0.02 g.
c.
0.026 g.
b.
0.025 g.
d.
2.5 ´ 102 g.
 

 22. 

In division and multiplication, the answer must not have more significant figures than the
a.
number in the calculation with fewest significant figures.
b.
number in the calculation with most significant figures.
c.
average number of significant figures in the calculation.
d.
total number of significant figures in the calculation.
 

 23. 

The number of significant figures in the measurement 0.000305 kg is
a.
3.
c.
5.
b.
4.
d.
6.
 

 24. 

The number of significant figures in the measurement 170.040 km is
a.
3.
c.
5.
b.
4.
d.
6.
 

 25. 

The number that has five significant figures is
a.
23 410
c.
0.01783
b.
0.00652
d.
10.292
 

 26. 

The sum of 314.53 km and 32 km is correctly expressed as
a.
346 km.
c.
346.53 km.
b.
346.5 km.
d.
347 km.
 

 27. 

The correct number of significant figures that should appear in the answer to the calculation 3.475 ´ 1.97 + 2.4712 is
a.
2.
c.
4.
b.
3.
d.
5.
 

 28. 

When 6.02 ´ 1023 is multiplied by 9.1 ´ 10–31, the product is
a.
5.5 ´ 10–8.
c.
5.5 ´ 10–7.
b.
5.5 ´ 1054.
d.
5.5 ´ 10–53.
 

 29. 

A nuclear particle that has about the same mass as a proton, but with no electrical charge, is called a(n)
a.
nuclide.
c.
electron.
b.
neutron.
d.
isotope.
 

 30. 

The mass of a neutron is
a.
about the same as that of a proton.
c.
double that of a proton.
b.
about the same as that of an electron.
d.
double that of an electron.
 

 31. 

The nucleus of most atoms is composed of
a.
tightly packed protons.
c.
tightly packed protons and neutrons.
b.
tightly packed neutrons.
d.
loosely connected protons and electrons.
 

 32. 

An atom is electrically neutral because
a.
neutrons balance the protons and electrons.
b.
nuclear forces stabilize the charges.
c.
the numbers of protons and electrons are equal.
d.
the numbers of protons and neutrons are equal.
 

 33. 

Atoms of the same element that have different masses are called
a.
moles.
c.
nuclides.
b.
isotopes.
d.
neutrons.
 

 34. 

Isotopes of an element contain different numbers of
a.
electrons.
c.
neutrons.
b.
protons.
d.
nuclides.
 

 35. 

An aluminum isotope consists of 13 protons, 13 electrons, and 14 neutrons. Its mass number is
a.
13.
c.
27.
b.
14.
d.
40.
 

 36. 

Chlorine has atomic number 17 and mass number 35. It has
a.
17 protons, 17 electrons, and 18 neutrons.
b.
35 protons, 35 electrons, and 17 neutrons.
c.
17 protons, 17 electrons, and 52 neutrons.
d.
18 protons, 18 electrons, and 17 neutrons.
 

 37. 

Argon (atomic number 18 and mass number 40) has ____ protons in its nucleus.
a.
22
c.
40
b.
9
d.
18
 

 38. 

The atomic number of neon is 10. The atomic number of calcium is 20. Compared with a mole of neon, a mole of calcium contains
a.
twice as many atoms.
c.
an equal number of atoms.
b.
half as many atoms.
d.
20 times as many atoms.
 

 39. 

An Avogadro's number amount of any element is equivalent to
a.
the atomic number of that element.
c.
6.022 ´ 1023 particles.
b.
the mass number of that element.
d.
100 g of that element.
 

 40. 

The mass of 1 mol of chromium  is
a.
12 g.
c.
52.0 g.
b.
198 g.
d.
6.02 ´ 1023 g.
 

 41. 

A quantity of sodium contains 6.02 ´ 1023 atoms. The mass of the sodium is
a.
6.02 ´ 1023 g.
c.
23.0 g.
b.
3.88 g.
d.
not determinable.
 

 42. 

How many moles of mercury are in 50.15 g of mercury?
a.
0.1000 mol
c.
0.2500 mol
b.
4.000 mol
d.
0.4000 mol
 

 43. 

A prospector finds 39.39 g of gold . She has
a.
1.203 ´ 1023 atoms.
c.
4.300 ´ 1023 atoms.
b.
3.011 ´ 1024 atoms.
d.
6.02 ´ 1023 atoms.
 

 44. 

Visible light, X rays, infrared radiation, and radio waves all have the same
a.
energy.
c.
speed.
b.
wavelength.
d.
frequency.
 

 45. 

For electromagnetic radiation, c (the speed of light) equals
a.
frequency minus wavelength.
c.
frequency divided by wavelength.
b.
frequency plus wavelength.
d.
frequency times wavelength.
 

 46. 

Because c, the speed of electromagnetic radiation, is a constant, the wavelength of the radiation is
a.
proportional to its frequency.
c.
inversely proportional to its frequency.
b.
equal to its frequency.
d.
double its frequency.
 

 47. 

The major difference between a 1s orbital and a 2s orbital is that
a.
the 2s orbital can hold more electrons.
b.
the 2s orbital has a slightly different shape.
c.
the 2s orbital is at a higher energy level.
d.
the 1s orbital can have only one electron.
 

 48. 

An orbital that could never exist according to the quantum description of the atom is
a.
3d.
c.
6d.
b.
8s.
d.
3f.
 

 49. 

The number of orbitals for the d sublevel is
a.
1.
c.
5.
b.
3.
d.
7.
 

 50. 

How many electrons are needed to completely fill the fourth energy level?
a.
8
c.
32
b.
18
d.
40
 

 51. 

What is the electron configuration for nitrogen, atomic number 7?
a.
1s2 2s2 2p3
c.
1s2 2s3 2p1
b.
1s2 2s3 2p2
d.
1s2 2s2 2p2 3s1
 

 52. 

The number of electrons in the highest energy level of the argon atom (atomic number 18) is
a.
10.
c.
6.
b.
2.
d.
8.
 

 53. 

Calculate the wavelength of light emitted by a lamp if the frequency of the light
is 5.10 x 1014 Hz
a.
1.70 x 107 m
c.
1.53 x 1023 m
b.
5.88 x 10-7 m
d.
3.00 x 108 m
 

 54. 

Calculate the energy of a single photon of green light with a wavelength of 5.50 x 10-7 m
a.
1.21 x 10-48 J
c.
1.09 x 10-31 J
b.
2.25 x 105 J
d.
3.61 x 10-19 J
 

 55. 

The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed to
a.
Mendeleev.
c.
Bohr.
b.
Moseley.
d.
Ramsay.
 

 56. 

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.
 

 57. 

Argon, krypton, and xenon are
a.
alkaline earth metals.
c.
actinides.
b.
noble gases.
d.
lanthanides.
 

 58. 

In the modern periodic table, elements are ordered according to
a.
decreasing atomic mass.
c.
increasing atomic number.
b.
Mendeleev's original design.
d.
the date of their discovery.
 

 59. 

The periodic law allows some properties of an element to be predicted based on its
a.
position in the periodic table.
c.
symbol.
b.
number of isotopes.
d.
color.
 

 60. 

A horizontal row of blocks in the periodic table is called a(n)
a.
group.
c.
family.
b.
period.
d.
octet.
 

 61. 

Elements to the right side of the periodic table have properties most associated with
a.
gases.
c.
metals.
b.
nonmetals.
d.
metalloids.
 

 62. 

Elements in which the d-sublevel is being filled have the properties of
a.
metals.
c.
metalloids.
b.
nonmetals.
d.
gases.
 

 63. 

Bromine, atomic number 35, belongs to Group 17. How many electrons does bromine have in its outermost energy level?
a.
7
c.
18
b.
17
d.
35
 

 64. 

A measure of the ability of an atom in a chemical compound to attract electrons is called
a.
electron affinity.
c.
electronegativity.
b.
electron configuration.
d.
ionization potential.
 

 65. 

In a row in the periodic table, as the atomic number increases, the atomic radius generally
a.
decreases.
c.
increases.
b.
remains constant.
d.
becomes unmeasurable.
 

 66. 

Valence electrons are those
a.
closest to the nucleus.
c.
in the highest energy level.
b.
in the lowest energy level.
d.
combined with protons.
 

 67. 

A chemical bond resulting from the electrostatic attraction between positive and negative ions is called a(n)
a.
covalent bond.
c.
charged bond.
b.
ionic bond.
d.
dipole bond.
 

 68. 

How many atoms of fluorine are present in a molecule of carbon tetrafluoride, CF4?
a.
1
c.
4
b.
2
d.
5
 

 69. 

What is the formula for zinc fluoride?
a.
ZnF
c.
Zn2F
b.
ZnF2
d.
Zn2F3
 

 70. 

What is the formula for aluminum sulfate?
a.
AlSO4
c.
Al2(SO4)3
b.
Al2SO4
d.
Al(SO4)3
 

 71. 

Name the compound Fe(NO2)2.
a.
iron(II) nitrate
c.
ferric nitrate
b.
iron(II) nitrite
d.
ferrous nitride
 

 72. 

What is the formula for nitrogen monoxide?
a.
N2O
c.
NO
b.
NOO
d.
N2O2
 

 73. 

What is the formula for carbon disulfide?
a.
CaS2
c.
S2C
b.
CS2
d.
SC2
 

 74. 

The molar mass of MgI2 is
a.
the sum of the masses of 1 mol of Mg and 2 mol of I.
b.
the sum of the masses of 1 mol of Mg and 1 mol of I.
c.
the sum of the masses of 2 mol of Mg and 2 mol of I.
d.
impossible to calculate.
 

 75. 

The molar mass of CCl4 is 153.81 g/mol. How many grams of CCl4 are needed to have 5.000 mol?
a.
5 g
c.
769.0 g
b.
30.76 g
d.
796.05 g
 

 76. 

How many oxygen atoms are there in 0.5 mol of CO2?
a.
6.02 ´ 1023
c.
15.9994
b.
3.01 ´ 1023
d.
11
 

 77. 

What is the percentage composition of CO?
a.
50% C, 50% O
c.
25% C, 75% O
b.
12% C, 88% O
d.
43% C, 57% O
 

 78. 

What is the percentage composition of oxygen in H2O?
a.
15.99%
c.
88.8%
b.
33%
d.
99.8%
 

 79. 

In a molecule of fluorine, the two shared electrons give each fluorine atom ____ electron(s) in the outer energy level.
a.
1
c.
8
b.
2
d.
32
 

 80. 

An octet is equal to
a.
2.
c.
5.
b.
4.
d.
8.
 

 81. 

The electron configuration of nitrogen is 1s2 2s2 2p3. How many more electrons does nitrogen need to satisfy the octet rule?
a.
1
c.
5
b.
3
d.
8
 

 82. 

In drawing a Lewis structure, each nonmetal atom except hydrogen should be surrounded by
a.
2 electrons.
c.
8 electrons.
b.
4 electrons.
d.
10 electrons.
 

 83. 

To draw a Lewis structure, one must know the
a.
number of valence electrons in each atom.
b.
atomic mass of each atom.
c.
bond length of each atom.
d.
ionization energy of each atom.
 
 
1st_sem_review_files/i0860000.jpg
 

 84. 

What is the Lewis structure for carbon tetraiodide, which contains one carbon atom and four iodine atoms?
a.
A
c.
C
b.
B
d.
D
 

 85. 

Name the compound KClO3.
a.
potassium chloride
c.
potassium chlorate
b.
potassium trioxychlorite
d.
hypochlorite
 

 86. 

What is the formula for nitrogen trifluoride?
a.
NiF3
c.
N3F
b.
NF3
d.
Ni3F
 

 87. 

The molar mass of NO2 is 46.0 g/mol. How many moles of NO2 are present in 114.95 g?
a.
0.400 mol
c.
2.50 mol
b.
1.00 mol
d.
114 mol
 

 88. 

The molar mass of CS2 is 76.2 g/mol. How many grams of CS2 are present in 10.00 mol?
a.
0.131 g
c.
10.0 g
b.
7.62 g
d.
762 g
 

 89. 

What is the percentage composition of CuCl2?
a.
33% Cu, 66% Cl
c.
65.50% Cu, 34.50% Cl
b.
50% Cu, 50% Cl
d.
47.263% Cu, 52.737% Cl
 

 90. 

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%
 



 
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