Multiple Choice
Identify the
letter of the choice that best completes the statement or answers the question.
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Choose the
letter of the choice that best completes the statement or answers the question. Use the periodic
table in your textbook.
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1.
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Elements in
the same group have the same ____. a. | atomic radius. | c. | nuclear charge. | b. | energy level of outer
electrons. | d. | number of valence
electrons. | | | | |
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2.
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Most of the
elements in groups 6A–8A are classified as ____. a. | alkali
metals. | c. | nonmetals. | b. | inner transition metals. | d. | alkaline earth metals. | | | | |
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3.
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Which energy
level of the period 4 transition elements is being filled with electrons? a. | third | c. | fifth | b. | fourth | d. | sixth | | | | |
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4.
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Identify the
period and group of the element that has the electron configuration
[Ne]3s23p3. a. | period 2, group 2A | c. | period 3, group 3A | b. | period 3, group
1A | d. | period 3, group
5A | | | | |
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5.
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Which of the
following classifications describes the element with the electron configuration  ? a. | stable
metal | c. | unstable
nonmetal | b. | stable nonmetal | d. | unstable metal | | | | |
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6.
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What is the
electron configuration of the element in group 4A and period 4 of the periodic
table?
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7.
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What is the
trend in atomic radii as you move from left-to-right across a period? a. | generally
decreases | c. | remains the
same | b. | generally
increases | d. | varies
randomly | | | | |
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8.
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The trend in
the atomic radii as you move down the group 1A elements is partially due to ____. a. | decreased distance of
outer electrons. | b. | increased nuclear charge. | c. | increased number of
electrons in outer energy level. | d. | shielding by inner electrons. | | |
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9.
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In which of
the following pair is the second particle listed larger than the first? a. | K,
Ga | c. | Br,
Br- | b. | Pb, C | d. | Li, Li+ | | | | |
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10.
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How many
electrons does an atom generally need in its outer level to be the most stable?
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11.
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Which of the
following electron configurations represents the most chemically stable atom?
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Matching
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Match the
terms below with their correct definitions. a. | alkali metals | h. | noble gases | b. | alkaline earth metals | i. | octet rule | c. | electronegativity | j. | periodic law | d. | halogens | k. | representative
elements | e. | period | l. | transition elements | f. | ion | m. | group | g. | ionization energy | | | | |
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12.
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Statement
that when the elements are arranged by increasing atomic number, there is a periodic repetition of
their chemical and physical properties
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13.
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Group A
elements
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14.
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Group B
elements
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15.
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Group 1A
elements (except for hydrogen)
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16.
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Group 2A
elements
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17.
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A column in
the periodic table
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18.
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A row in the
periodic table
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19.
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Group 7A
elements
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20.
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Group 8A
elements
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21.
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Atom or
bonded group of atoms that has a positive or negative charge
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22.
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Energy
required to remove an electron from a gaseous atom
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23.
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Statement
that atoms tend to gain, lose, or share electrons to acquire a full set of eight valence
electrons
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24.
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Indication
of an atom’s ability to attract electrons in a chemical bond
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Short Answer
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Write a
sentence that uses each group of terms.
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25.
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transition
metals, inner transition metals
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26.
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metal,
nonmetal, metalloid
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Briefly
describe the contribution of each of the following to the development of the periodic
table.
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27.
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John
Newlands:
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28.
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Henry
Moseley:
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29.
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Dmitri
Mendeleev:
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Match each
of the following terms with a number or chemical symbol from the periodic table below.
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30.
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alkali
metals
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31.
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alkaline
earth metals
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32.
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a d-block
element
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33.
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an f-block
element
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34.
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halogens
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35.
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inner
transition metals
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36.
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a metalloid
element
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37.
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noble
gases
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38.
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a p-block
element that is not a metalloid
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39.
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an s-block
element
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40.
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transition
metals
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The graph
below shows the atomic radii of the elements in the first four periods of the periodic table, as well
as the major ionic radii of the group A elements. The charge of each ion is indicated above the
plotted point representing its radius. Use the graph and the periodic table in your textbook to
answer the following questions.
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41.
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Describe the
relationship between atomic radii and atomic number for the group A elements in the first four
periods.
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42.
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How can you
account for the trend you described in your answer to question 1?
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43.
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Describe the
relationship between the atomic radii and the atomic numbers of the transition elements (group B) in
period 4.
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44.
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Explain why
the two elements in the first period do not have ionic radii listed.
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45.
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Predict
whether the arsenic ion shown in the graph has a positive or negative charge. (Arsenic has an atomic
number of 33.) Explain your prediction.
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Problem
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At the
beginning of the nineteenth century, chemists were searching for numerical relationships among the
elements. From these relationships, they hoped that some fundamental chemical principle might be
revealed. One such chemist was the German, Johann Wolfgang Döbereiner. In 1817, Döbereiner
noted that if the three alkaline earth metals Ca, Sr, and Ba were arranged in increasing atomic mass,
the atomic mass of the middle element was close to the average of the other two atomic masses, as
shown below.
In 1829, Döbereiner discovered that the halogens—Cl, Br, and
I—also followed a similar pattern, as shown below. He named these three-member groups of
elements with similar chemical and physical properties triads.
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46.
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Six of the
eight elements in the table below make up two of Döbereiner’s triads. Plot the atomic mass
of each element on the number line below the table. From the sequence of the atomic masses and your
knowledge of elements with similar chemical and physical properties, identify the three elements in
each of the two triads. Explain your choices.
Element | Mass
(amu) | Lithium (Li) | 7 | Carbon
(C) | 12 | Sodium
(Na) | 23 | Sulfur
(S) | 32 | Potassium
(K) | 39 | Selenium
(Se) | 79 | Tellurium
(Te) | 128 | Gold
(Au) | 197 | | |
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47.
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Recall that
atomic mass is a quantitative physical property of an element. So are density, melting point, and
boiling point. Use the table below to sequence the values of the densities, melting points, and
boiling points of the following triads—Ca, Sr, and Ba; and Cl, Br, and I. Then determine whether
each property shows a trend similar to that of the atomic masses of the elements in the triads.
Explain your reasoning.
Element | Density
(g/mL) | Melting Point
(°C) | Boiling Point
(°C) | Barium
(Ba) | 3.62 | 726.9 | 1845 | Bromine
(Br) | 3.11 | -7.25 | 59.35 | Calcium
(Ca) | 1.55 | 841.5 | 1500.5 | Chlorine
(Cl) | 0.003 214 | -101 | -34 | Iodine
(I) | 4.93 | 113.6 | 184.5 | Strontium
(Sr) | 2.6 | 776.9 | 1412 | | | | |
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48.
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If silicon
(Si), germanium (Ge), and tin (Sn) are classified as a triad similar to those of Döbereiner,
predict values that will complete the following table. Record the values in the table.
Element | Atomic Mass
(amu) | Density
(g/mL) | Melting Point
(°C) | Silicon
(Si) | 28 | | 1411 | Germanium
(Ge) | | 5.3 | 945 | Tin
(Sn) | 119 | 7.3 | | | | | |
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