Chm 1.3. Matter: Properties and Change - Physical and Chemical Properties of Atoms based on Periodic Table Location - Chapter 4 and 5
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
____1.The element with electron configuration 1s2 2s2 2p6 3s2 3p2 is
a. / Mg (Z = 12). / c. / S (Z = 16).b. / C (Z = 6). / d. / Si (Z = 14).
____2.The electron configuration for the carbon atom (C) is 1s2 2s2 2p2. The atomic number of carbon is
a. / 3. / c. / 11.b. / 6. / d. / 12.
____3.What is the electron configuration for nitrogen, atomic number 7?
a. / 1s2 2s2 2p3b. / 1s2 2s3 2p2
c. / 1s2 2s3 2p1
d. / 1s2 2s2 2p2 3s1
____4.The electron notation for aluminum (atomic number 13) is
a. / 1s2 2s2 2p3 3s2 3p3 3d1.b. / 1s2 2s2 2p6 3s2 2d1.
c. / 1s2 2s2 2p6 3s2 3p1.
d. / 1s2 2s2 2p9.
____5.A spherical electron cloud surrounding an atomic nucleus would best represent
a. / an s orbital.b. / a px orbital.
c. / a combination of px and py orbitals.
d. / a combination of an s and a px orbital.
____6.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.
____7.The p orbitals are shaped like
a. / electrons. / c. / dumbbells.b. / circles. / d. / spheres.
____8.The letter designations for the first four sublevels with the maximum number of electrons that can be accommodated in each sublevel are
a. / s:2, p:4, d:6, and f:8.b. / s:1, p:3, d:5, and f:7.
c. / s:2, p:6, d:10, and f:14.
d. / s:1, p:2, d:3, and f:4.
____9.The number of orbitals for the d sublevel is
a. / 1. / c. / 5.b. / 3. / d. / 7.
____10.For the f sublevel, the number of orbitals is
a. / 5. / c. / 9.b. / 7. / d. / 18.
____11.The total number of orbitals that can exist at the second main energy level is
a. / 2. / c. / 4.b. / 3. / d. / 8.
____12.How many electrons can occupy the s orbitals at each energy level?
a. / two, if they have opposite spinsb. / two, if they have the same spin
c. / one
d. / no more than eight
____13.How many electrons are needed to completely fill the fourth energy level?
a. / 8 / c. / 32b. / 18 / d. / 40
____14.At n = 1, the total number of electrons that could be found is
a. / 1. / c. / 6.b. / 2. / d. / 18.
____15.The atomic sublevel with the next highest energy after 4p is
a. / 4d. / c. / 5p.b. / 4f. / d. / 5s.
____16.In the electron configuration for scandium (atomic number 21), what is the notation for the three highest-energy electrons?
a. / 3d1 4s2 / c. / 3d3b. / 4s3 / d. / 4s2 4p1
____17.Which of the following lists atomic orbitals in the correct order they are filled according to the Aufbau principle?
a. / 1s 2s 2p 3s 4s 3p 3d 4p 5sb. / 1s 2s 2p 3s 3p 4s 3d 4p 5s
c. / 1s 2s 2p 3s 3p 4s 4p 3d 4d
d. / 1s 2s 2p 3s 3p 3d 4s 4p 5s
____18.In the ground state, the 3d and 4s sublevels of the chromium atom (atomic number 24) are represented as
a. / 3d6 4s1. / c. / 3d5 4s1.b. / 3d4 4s2. / d. / 4s2 3d4.
____19.If the s and p orbitals of the highest main energy level of an atom are filled with electrons, the atom has a(n)
a. / electron pair. / c. / empty d orbital.b. / octet. / d. / electron in an excited state.
____20.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.
____21.If an element has an octet of electrons in its highest main energy level, there are ____ electrons in this level.
a. / 2 / c. / 10b. / 8 / d. / 32
____22.An element with 8 electrons in its highest main energy level is a(n)
a. / octet element. / c. / Aufbau element.b. / third period element. / d. / noble gas.
____23.What are the radioactive elements with atomic numbers from 90 to 103 called?
a. / the noble gases / c. / the actinidesb. / the lanthanides / d. / the rare-earth elements
____24.What are the elements with atomic numbers from 58 to 71 called?
a. / the lanthanides / c. / the actinidesb. / the noble gases / d. / the alkali metals
____25.Argon, krypton, and xenon are
a. / alkaline earth metals. / c. / actinides.b. / noble gases. / d. / lanthanides.
____26.Elements in a group or column in the periodic table can be expected to have similar
a. / atomic masses. / c. / numbers of neutrons.b. / atomic numbers. / d. / properties.
____27.The atomic number of lithium, the first element in Group 1, is 3. The atomic number of the second element in this group is
a. / 4. / c. / 11.b. / 10. / d. / 18.
____28.Krypton, atomic number 36, is the fourth element in Group 18. What is the atomic number of xenon, the fifth element in Group 18?
a. / 54 / c. / 72b. / 68 / d. / 90
____29.Barium, atomic number 56, is the fifth element in Group 2. What is the atomic number of radium, the next element in Group 2?
a. / 64 / c. / 88b. / 74 / d. / 103
____30.Refer to the figure below. To which group do fluorine and chlorine belong?
a. / alkaline-earth metals / c. / halogensb. / transition elements / d. / actinides
____31.A horizontal row of blocks in the periodic table is called a(n)
a. / group. / c. / family.b. / period. / d. / octet.
____32.Refer to the figure above. Potassium and bromine belong to
a. / Period 4. / c. / Period 1.b. / Group 4. / d. / Group 1.
____33.The electron configuration of aluminum, atomic number 13, is [Ne] 3s2 3p1. Aluminum is in Period
a. / 2. / c. / 6.b. / 3. / d. / 13.
____34.The electron configuration of cesium, atomic number 55, is [Xe] 6s1. In what period is cesium?
a. / Period 1 / c. / Period 8b. / Period 6 / d. / Period 55
____35.The period of an element can be determined from its
a. / reactivity. / c. / symbol.b. / density. / d. / electron configuration.
____36.Elements to the right side of the periodic table (p-block elements) have properties most associated with
a. / gases. / c. / metals.b. / nonmetals. / d. / metalloids.
____37.Neutral atoms with an s2p6 electron configuration in the highest energy level belong to which block of the periodic table?
a. / s block / c. / d blockb. / p block / d. / f block
____38.Elements in which the d-sublevel is being filled have the properties of
a. / metals. / c. / metalloids.b. / nonmetals. / d. / gases.
____39.The group of 14 f block elements in the sixth period is the
a. / actinides. / c. / transition elements.b. / lanthanides. / d. / metalloids.
____40.Within the p-block elements, the elements at the top of the table, compared with those at the bottom,
a. / have larger radii. / c. / have lower ionization energies.b. / are more metallic. / d. / are less metallic.
____41.The electron configurations of the noble gases from neon to radon in the periodic table make these elements part of the
a. / f block. / c. / s block.b. / d block. / d. / p block.
____42.Hydrogen is placed separately from other elements in the periodic table because it
a. / is a gas.b. / does not exist as a free element in nature.
c. / has atomic number one.
d. / has many unique properties.
____43.To which block do the actinide elements belong?
a. / d block / c. / f blockb. / s block / d. / p block
____44.For groups 13 through 18, the total number of electrons in the highest occupied level equals the group number
a. / plus 1. / c. / plus 5.b. / minus 1. / d. / minus 10.
____45.Strontium's highest occupied energy level is 5s2. To what group does strontium belong?
a. / Group 2 / c. / Group 6b. / Group 5 / d. / Group 8
____46.Bromine, atomic number 35, belongs to Group 17. How many electrons does bromine have in its outermost energy level?
a. / 7 / c. / 18b. / 17 / d. / 35
____47.In nature, the alkali metals occur as
a. / elements. / c. / complex ions.b. / compounds. / d. / gases.
____48.The elements in Group 1 are also known as the
a. / alkali metals. / c. / Period 1 elements.b. / rare-earth series. / d. / actinide series.
____49.Which block in the periodic table contains the alkali metals?
a. / s / c. / db. / p / d. / f
____50.The most reactive group of the nonmetals is the
a. / lanthanides. / c. / halogens.b. / transition elements. / d. / noble gases.
____51.The group of soft, silvery, reactive metals, all of which have one electron in an s orbital, is known as the
a. / alkaline-earth metals. / c. / alkali metals.b. / transition metals. / d. / metalloids.
____52.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.
____53.Compared to the alkali metals, the alkaline-earth metals
a. / are less reactive.b. / have lower melting points.
c. / are less dense.
d. / combine more readily with nonmetals.
____54.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.
____55.A measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound is called
a. / electron affinity. / c. / electronegativity.b. / electron configuration. / d. / ionization potential.
____56.The element that has the greatest electronegativity is
a. / oxygen. / c. / chlorine.b. / sodium. / d. / fluorine.
____57.A positive ion is known as a(n)
a. / ionic radius. / c. / cation.b. / valence electron. / d. / anion
____58.A negative ion is known as a(n)
a. / ionic radius. / c. / cation.b. / valence electron. / d. / anion.
____59.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 immeasurable.
____60.Within a group of elements, as the atomic number increases, the atomic radius
a. / increases.b. / remains approximately constant.
c. / decreases regularly.
d. / varies unpredictably.
____61.In the alkaline-earth group, atoms with the smallest radii
a. / are the most reactive.b. / have the largest volume.
c. / are all gases.
d. / have the highest ionization energies.
____62.As the atomic number of the metals of Group 1 increases, the ionic radius
a. / increases. / c. / remains the same.b. / decreases. / d. / cannot be determined.
____63.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.
____64.Which is the best reason that the atomic radius generally increases with atomic number in each group of elements?
a. / The nuclear charge increases.b. / The number of neutrons increases.
c. / The number of occupied energy levels increases.
d. / A new octet forms.
____65.As you move down Group 14 in the periodic table from carbon through lead, atomic radii
a. / generally increase. / c. / do not change.b. / generally decrease. / d. / vary unpredictably.
____66.As you move left to right in Period 4 from gallium through bromine, atomic radii
a. / generally increase. / c. / do not change.b. / generally decrease. / d. / vary unpredictably.
____67.Hoe does the energy required to remove an electron from an atom changer as you move left to right in Period 4 from potassium through iron?
a. / It generally increases. / c. / It does not change.b. / It generally decreases. / d. / It varies unpredictably.
____68.The electrons available to be lost, gained, or shared when atoms form compounds are called
a. / ions. / c. / d electrons.b. / valence electrons. / d. / electron clouds.
____69.The number of valence electrons in Group 1 elements is
a. / 1. / c. / 8.b. / 2. / d. / equal to the period number.
____70.The number of valence electrons in Group 17 elements is
a. / 7. / c. / 17.b. / 8. / d. / equal to the period number.
____71.The first electrons to be removed when d-block elements form ions are the
a. / d electrons. / c. / s electrons.b. / p electrons. / d. / f electrons.
Short Answer
72.The electron configuration for nitrogen is 1s2 2s2 2p3. What does the 3 in 2p3 mean?
Problem
73.Write the electron configuration for nitrogen, atomic number 7.
74.Which element has the following electron configuration: [Ar] 4s2 3d10 4p5?
75.Write the noble-gas electron configuration for silicon.
76.Draw the orbital diagram for phosphorus.
77.Draw the orbital diagram for argon.
78.Write the noble-gas electron configuration represented in the orbital diagram below.
79.What element's orbital diagram is shown in the figure below?
Essay
80.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.
Chm 1.3. Matter: Properties and Change - Physical and Chemical Properties of Atoms based on Periodic Table Location - Chapter 4 and 5
Answer Section
MULTIPLE CHOICE
1.ANS:DDIF:IIREF:3OBJ:3
2.ANS:BDIF:IIREF:3OBJ:3
3.ANS:ADIF:IIREF:3OBJ:3
4.ANS:CDIF:IIREF:3OBJ:3
5.ANS:ADIF:IIREF:2OBJ:5
6.ANS:CDIF:IIREF:2OBJ:5
7.ANS:CDIF:IREF:2OBJ:5
8.ANS:CDIF:IIREF:2OBJ:5
9.ANS:CDIF:IIREF:2OBJ:5
10.ANS:BDIF:IIREF:2OBJ:5
11.ANS:CDIF:IIREF:2OBJ:5
12.ANS:ADIF:IIREF:2OBJ:5
13.ANS:CDIF:IIREF:3OBJ:1
14.ANS:BDIF:IIREF:3OBJ:1
15.ANS:DDIF:IIREF:3OBJ:2
16.ANS:ADIF:IIIREF:3OBJ:3
17.ANS:BDIF:IIREF:3OBJ:3
18.ANS:CDIF:IIREF:3OBJ:3
19.ANS:BDIF:IIREF:3OBJ:3
20.ANS:DDIF:IIREF:3OBJ:3
21.ANS:BDIF:IREF:3OBJ:3
22.ANS:DDIF:IREF:3OBJ:3
23.ANS:CDIF:IREF:1OBJ:2
24.ANS:ADIF:IREF:1OBJ:2
25.ANS:BDIF:IREF:1OBJ:2
26.ANS:DDIF:IREF:1OBJ:4
27.ANS:CDIF:IIREF:1OBJ:4
28.ANS:ADIF:IIREF:1OBJ:4
29.ANS:CDIF:IIREF:1OBJ:4
30.ANS:CDIF:IREF:1OBJ:4
31.ANS:BDIF:IREF:1OBJ:4
32.ANS:ADIF:IREF:1OBJ:4
33.ANS:BDIF:IREF:2OBJ:1
34.ANS:BDIF:IREF:2OBJ:1
35.ANS:DDIF:IREF:2OBJ:1
36.ANS:BDIF:IREF:2OBJ:2
37.ANS:DDIF:IIREF:2OBJ:2
38.ANS:ADIF:IREF:2OBJ:2
39.ANS:BDIF:IREF:2OBJ:2
40.ANS:DDIF:IREF:2OBJ:2
41.ANS:DDIF:IREF:2OBJ:2
42.ANS:DDIF:IREF:2OBJ:2
43.ANS:CDIF:IREF:2OBJ:2
44.ANS:DDIF:IIREF:2OBJ:3
45.ANS:ADIF:IIREF:2OBJ:3
46.ANS:ADIF:IIREF:2OBJ:3
47.ANS:BDIF:IREF:2OBJ:4
48.ANS:ADIF:IREF:2OBJ:4
49.ANS:ADIF:IREF:2OBJ:4
50.ANS:CDIF:IREF:2OBJ:4
51.ANS:CDIF:IREF:2OBJ:4
52.ANS:DDIF:IREF:2OBJ:4
53.ANS:ADIF:IIREF:2OBJ:4
54.ANS:DDIF:IREF:3OBJ:1
55.ANS:CDIF:IREF:3OBJ:1
56.ANS:DDIF:IIREF:3OBJ:2
57.ANS:CDIF:IREF:3OBJ:2
58.ANS:DDIF:IREF:3OBJ:2
59.ANS:ADIF:IIREF:3OBJ:2
60.ANS:ADIF:IIREF:3OBJ:2
61.ANS:DDIF:IIREF:3OBJ:2
62.ANS:ADIF:IIREF:3OBJ:2
63.ANS:ADIF:IIREF:3OBJ:2
64.ANS:CDIF:IIREF:3OBJ:2
65.ANS:ADIF:IIREF:3OBJ:2
66.ANS:BDIF:IIREF:3OBJ:2
67.ANS:ADIF:IIREF:3OBJ:2
68.ANS:BDIF:IREF:3OBJ:3
69.ANS:ADIF:IREF:3OBJ:3
70.ANS:ADIF:IREF:3OBJ:3
71.ANS:CDIF:IREF:3OBJ:4
SHORT ANSWER
72.ANS:
The 3 in 2p3 indicates that three electrons are in the p orbitals of the second energy level.
DIF:IIREF:3OBJ:3
PROBLEM
73.ANS:
1s2 2s2 2p3
DIF:IIIREF:3OBJ:3
74.ANS:
bromine
DIF:IIIREF:3OBJ:3
75.ANS:
[Ne] 3s2 3p2
DIF:IIIREF:3OBJ:3
76.ANS:
DIF:IIIREF:3OBJ:3
77.ANS:
DIF:IIIOBJ:4-3.3
78.ANS:
[Ne] 3s2 3p4
DIF:IIIREF:3OBJ:3
79.ANS:
fluorine
DIF:IIIREF:3OBJ:3
ESSAY
80.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.
DIF:IIREF:3OBJ:2