Multiple Choice
Identify the
letter of the choice that best completes the statement or answers the question.
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1.
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In
oxides of nitrogen, such as N2O, NO, NO2, and N2O3, atoms
combine in small whole-number ratios. This evidence supports the law of a. | conservation of
mass. | c. | definite
composition. | b. | multiple proportions. | d. | mass action. | | | | |
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2.
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The
two oxides of lead, PbO and PbO2, are explained by the a. | periodic
law. | c. | atomic
law. | b. | law of multiple
proportions. | d. | law of
conservation of mass. | | | | |
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3.
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If
two or more compounds are composed of the same two elements, the ratio of the masses of one element
that combine with a fixed mass of the other element is a simple whole number. This is a statement of
the law of a. | conservation of
mass. | c. | multiple
proportions. | b. | mass action. | d. | definite composition. | | | | |
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4.
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Who
was the schoolmaster who studied chemistry and proposed an atomic theory? a. | John
Dalton | c. | Robert
Brown | b. | Jons Berzelius | d. | Dmitri Mendeleev | | | | |
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5.
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Who
first recognized that the ratio of the number of atoms that combine is the same as the ratio of the
masses that combine? a. | Jons Berzelius | c. | John Dalton | b. | Edward
Morley | d. | Jon
Newlands | | | | |
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6.
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The
principles of atomic theory recognized today were conceived by a. | Avogadro. | c. | Dalton. | b. | Bohr. | d. | Rutherford. | | | | |
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7.
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According to Dalton's atomic theory, atoms a. | of different
elements combine in simple whole-number ratios to form compounds. | b. | can be divided
into protons, neutrons, and electrons. | c. | of all elements are identical in size and
mass. | d. | can be destroyed in chemical
reactions. | | |
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8.
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Dalton's atomic theory did NOT explain the law of a. | whole-number
ratios. | c. | conservation of
mass. | b. | definite proportions. | d. | conservation of energy. | | | | |
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9.
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In
Rutherford's experiments, most of the particles a. | bounced back. | c. | were absorbed by the foil. | b. | passed through
the foil. | d. | combined with
the foil. | | | | |
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10.
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Because most particles fired at metal foil passed straight through, Rutherford
concluded that a. | atoms were
mostly empty space. | c. | electrons formed
the nucleus. | b. | atoms contained no charged
particles. | d. | atoms were
indivisible. | | | | |
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11.
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Because a few positively charged particles bounced back from the foil, Rutherford
concluded that such particles were a. | striking electrons. | b. | indivisible. | c. | repelled by densely packed regions of positive
charge. | d. | magnetic. | | |
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12.
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Rutherford fired positively charged particles at metal foil and concluded that most of
the mass of an atom was a. | in the electrons. | c. | evenly spread throughout the atom. | b. | concentrated in
the nucleus. | d. | in rings around
the atom. | | | | |
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13.
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What
did Rutherford conclude about the structure of the atom? a. | An atom is
indivisible. | b. | Electrons make up the center of an
atom. | c. | An atom carries a positive charge. | d. | An atom contains
a small, dense, positively charged central region. | | |
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14.
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A
positively charged particle with mass 1.673 ´ 10–24 g is a(n) a. | proton. | c. | electron. | b. | neutron. | d. | positron. | | | | |
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15.
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Which
part of an atom has a mass approximately equal to 1/2000 of the mass of a common hydrogen
atom? a. | nucleus | c. | proton | b. | electron | d. | electron cloud | | | | |
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16.
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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. | | | | |
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17.
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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. | | | | |
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18.
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Protons have a. | negative charges. | c. | no charges. | b. | an attraction
for neutrons. | d. | no
mass. | | | | |
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19.
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Most
of the volume of an atom is occupied by the a. | nucleus. | c. | electron cloud. | b. | nuclides. | d. | protons. | | | | |
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20.
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The
charge on the electron cloud a. | prevents compounds from forming. | b. | balances the
charge on the nucleus. | c. | attracts electron clouds in other atoms to form
compounds. | d. | does not exist. | | |
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21.
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The
smallest unit of an element that can exist either alone or in combination with other such particles
of the same or different elements is the a. | electron. | c. | neutron. | b. | proton. | d. | atom. | | | | |
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22.
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Atoms
of the same element that have different masses are called a. | moles. | c. | nuclides. | b. | isotopes. | d. | neutrons. | | | | |
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23.
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Isotopes of an element contain different numbers of a. | electrons. | c. | neutrons. | b. | protons. | d. | nuclides. | | | | |
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24.
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The
most common form of hydrogen has a. | no neutrons. | c. | two neutrons. | b. | one
neutron. | d. | three
neutrons. | | | | |
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25.
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All
isotopes of hydrogen contain a. | one neutron. | c. | one proton. | b. | two
electrons. | d. | two
nuclei. | | | | |
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26.
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Isotopes of each element differ in a. | the number of neutrons in the
nucleus. | b. | atomic number. | c. | the number of
electrons in the highest energy level. | d. | the total number of electrons. | | |
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27.
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The
total number of protons and neutrons in the nucleus of an atom is its a. | atomic
number. | c. | mass
number. | b. | Avogadro constant. | d. | number of neutrons. | | | | |
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28.
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As
the mass number of the isotopes of an element increases, the number of protons a. | decreases. | b. | increases. | c. | remains the
same. | d. | doubles each time the mass number
increases. | | |
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29.
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Atoms
of the same element can differ in a. | chemical properties. | c. | atomic number. | b. | mass
number. | d. | number of
protons and electrons. | | | | |
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30.
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The
abbreviation for atomic mass unit is
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31.
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The
average atomic mass of an element depends on both the masses of its isotopes and each
isotope's a. | atomic
number. | c. | relative
abundance. | b. | radioactivity. | d. | mass number. | | | | |
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32.
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A
single atom of an isotope does not have a(n) a. | relative atomic mass. | c. | mass number. | b. | atomic
number. | d. | average atomic
mass. | | | | |
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33.
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The
atomic mass listed in the periodic table is the a. | average atomic mass. | b. | relative atomic
mass of the most abundant isotope. | c. | relative atomic mass of the most stable radioactive
isotope. | d. | mass number of the most abundant
isotope. | | |
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34.
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What
is the atomic number for aluminum from the figure above?
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35.
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In
the figure above, a neutral atom of silicon contains a. | 14
electrons. | c. | 16
electrons. | b. | 28.09 electrons. | d. | 38 electrons. | | | | |
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36.
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An
atom of potassium has 19 protons and 20 neutrons. What is its mass number?
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37.
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A
neutral carbon atom (atomic number 6) has a. | 3 electrons and 3 neutrons. | c. | 3 protons and 3 electrons. | b. | 6
protons. | d. | 3 protons and 3
neutrons. | | | | |
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38.
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Zn-66
(atomic number 30) has a. | 30 neutrons. | c. | 36 neutrons. | b. | 33
neutrons. | d. | 96
neutrons. | | | | |
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39.
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Ag-109 has 62 neutrons. The neutral atom has a. | 40
electrons. | c. | 53
electrons. | b. | 47 electrons. | d. | 62 electrons. | | | | |
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40.
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Carbon-14 (atomic number 6), the radioactive nuclide used in dating fossils,
has a. | 6
neutrons. | c. | 10
neutrons. | b. | 8 neutrons. | d. | 14 neutrons. | | | | |
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41.
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Sulphur-34 (atomic number 16) contains a. | 34
protons. | c. | 18
neutrons. | b. | 18 protons. | d. | 16 neutrons. | | | | |
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42.
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Phosphorus-33 (atomic number 15) contains a. | 33
protons. | c. | 33
neutrons. | b. | 18 neutrons. | d. | 18 protons. | | | | |
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43.
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Silicon-30 contains 14 protons. It also contains a. | 16
electrons. | c. | 30
neutrons. | b. | 16 neutrons. | d. | 44 neutrons. | | | | |
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44.
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Neon-22 contains 12 neutrons. It also contains a. | 12
protons. | c. | 22
electrons. | b. | 22 protons. | d. | 10 protons. | | | | |
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45.
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Calcium-48 (atomic number 20) contains a. | 20
electrons. | c. | 20
neutrons. | b. | 48 protons. | d. | 28 protons. | | | | |
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46.
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Mendeleev's table was called periodic because the properties of the
elements a. | showed no
pattern. | b. | occurred at repeated intervals called
periods. | c. | occurred at regular time intervals called
periods. | d. | were identical. | | |
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47.
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What
are the radioactive elements with atomic numbers from 90 to 103 in the periodic table
called? a. | the noble
gases | c. | the
actinides | b. | the lanthanides | d. | the rare-earth elements | | | | |
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48.
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What
are the elements with atomic numbers from 58 to 71 in the periodic table called? a. | the lanthanide
elements | c. | the actinide
elements | b. | the noble gases | d. | the alkali metals | | | | |
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49.
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Argon, krypton, and xenon are a. | alkaline earth metals. | c. | actinides. | b. | noble
gases. | d. | lanthanides. | | | | |
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50.
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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. | | | | |
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51.
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The
atomic number of lithium, the first element in Group 1, is 3. The atomic number of the second element
in this group is
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52.
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To
which group do lithium and potassium belong? Refer to the figure above. a. | alkali
metals | c. | halogens | b. | transition metals | d. | noble gases | | | | |
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53.
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Refer
to the figure above. To which group do fluorine and chlorine belong? a. | alkaline-earth
metals | c. | halogens | b. | transition elements | d. | actinides | | | | |
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54.
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What
is the relative mass of an electron? a. | 1/1840 the mass of a hydrogen
atom | c. | 1/1840 the mass
of a C-12 atom | b. | 1/1840 the mass of a neutron +
proton | d. | 1/1840 the mass
of an alpha particle | | | | |
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55.
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An
element has an atomic number of 76. The number of protons and electrons in a neutral atom of the
element are ____. a. | 152 protons and
76 electrons | c. | 38 protons and
38 electrons | b. | 76 protons and 0 electrons | d. | 76 protons and 76 electrons | | | | |
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56.
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What
does the number 84 in the name krypton-84 represent? a. | the atomic
number | c. | the sum of the
protons and electrons | b. | the mass number | d. | twice the number of protons | | | | |
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Matching
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Match each item with the correct statement below. a. | proton | d. | electron | b. | nucleus | e. | neutron | c. | atom | | | | |
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57.
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the
smallest particle of an element that retains the properties of that element
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58.
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a
positively charged subatomic particle
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59.
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a
negatively charged subatomic particle
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60.
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a
subatomic particle with no charge
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61.
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the
central part of an atom, containing protons and neutrons
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Match each item with the correct statement below. a. | mass
number | d. | atomic
mass | b. | atomic mass
unit | e. | isotope | c. | atomic number | | | | |
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62.
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atoms
with the same number of protons, but different numbers of neutrons in the nucleus of an
atom
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63.
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the
total number of protons and neutrons in the nucleus of an atom
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64.
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the
number of protons in the nucleus of an element
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65.
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the
weighted average of the masses of the isotopes of an element
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66.
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one-twelfth the mass of a carbon atom having six protons and six
neutrons
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