Teacher Answer Key
November 23, 2011
Periodic Table Review
3
1. Which element is a solid at STP and a good conductor of electricity?
1. iodine
3. nickel
2. mercury
4. sulfur
3 Metals are good conductors of electricity. Both
mercury and nickel are metals, but nickel is a solid at
STP while mercury is a liquid.
1. Rb
2. Rn
3
2. Which element has both metallic and nonmetallic properties?
3. Si
4. Sr
3 Refer to the accompanying diagram, which
represents a portion of the Periodic Table of the
Elements:
4
3. The carbon atoms in graphite and the carbon atoms in diamond
The metalloids—those elements that have both
metallic and nonmetallic properties—are found in the have different
shaded boxes. Of the choices given, only choice (3),
Si, is a metalloid.
1. atomic numbers
3. electronegativities
2. atomic masses
4. structural arrangements
4 Graphite and diamond are known as allotropes—
forms of an element in which the atoms have
different structural arrangements in space.
1. Magnesium is malleable.
2. Magnesium conducts electricity.
3
4. Which statement describes a chemical property of the element
magnesium?
3. Magnesium reacts with an acid.
4. Magnesium has a high boiling point.
3 A chemical property is one in which the substance
is changed when the property is investigated. In other
words, a chemical reaction occurs. When magnesium
atoms react with an acid, hydrogen gas and
1
magnesium ions are formed.
5. Which statement explains why sulfur is classified as a Group
16 element?
Wrong Choices Explained:
(1), (2), (4) Malleability, conductivity, and boiling
point are physical properties. The magnesium atoms
are not changed by these properties.
1. A sulfur atom has 6 valence electrons.
2. A sulfur atom has 16 neutrons.
1 The group numbers of the representative elements
are related to the number of valence electrons in an
atom of the element, as shown in the accompanying
table:
1. Sodium has a larger atomic radius and is more
metallic.
2. Sodium has a larger atomic radius and is less
metallic.
3. Sulfur is a yellow solid at STP.
4. Sulfur reacts with most metals.
1
6. How do the atomic radius and metallic properties of sodium
compare to the atomic radius and metallic properties of
phosphorus?
3. Sodium has a smaller atomic radius and is more
metallic.
4. Sodium has a smaller atomic radius and is less
metallic.
1 See Reference Table S and the Periodic Table of the 1
Elements. Sodium has a larger atomic radius than
7. Which group on the Periodic Table of the Elements contains
phosphorus. Sodium is classified as a metal, and
phosphorus is classified as a nonmetal.
1. Group 1
2. Group 2
1 Refer to the Periodic Table of the Elements. In the
formula X2O, oxygen has an oxidation state of –2.
Therefore, the substance X must have an oxidation
state of +1, which places it in Group 1.
elements that react with oxygen to form compounds with the
general formula X2O?
3. Group 14
4. Group 18
'see explanation below'
8. Base your answers to the question on the information below.
Two isotopes of potassium are K-37 and K-42.
What is the total number of neutrons in the nucleus of a K-37
atom?
Use the Periodic Table of the Elements. The atomic number of potassium (K) is 19; there are 19 protons in
the nucleus of each potassium atom. The mass number of this isotope is 37; there are a total of 37 protons
and neutrons in the nucleus of this isotope. Subtract the atomic number from the mass number to obtain the
number of neutrons:
37 protons and neutrons ¿ 19 protons = 18 neutrons
[1 point]
'see explanation below'
9. Base your answers to the question on the information below.
Two isotopes of potassium are K-37 and K-42.
Explain, in terms of subatomic particles, why K-37 and K-42 are isotopes of potassium.
K-37 and K-42 are both isotopes of potassium because they have the same number of protons (19) but
different numbers of neutrons (18 and 23, respectively). [1 point]
'see explanation below'
10. Base your answer on the accompanying table.
Explain, in terms of atomic structure, why cesium has a lower first ionization energy than rubidium.
Of the elements given in the table that was shown with the question, cesium has a larger atomic radius than
rubidium (see Reference Table S). The larger size of the atom results in a smaller force of attraction between
the nucleus and the valence electron. Therefore, removing a valence electron from cesium is easier than
from rubidium. This is confirmed by the fact that cesium has a lower first ionization energy than rubidium.
[1 point]
'see explanation below'
11. Base your answer to the question on the information below.
The decomposition of sodium azide, NaN3(s), is used to inflate airbags. On impact, the NaN3(s) is ignited by
an electrical spark, producing N2(g) and Na(s). The N2(g) inflates the airbag.
An inflated airbag has a volume of 5.00 × 10 4 cm3 at STP. The density of N2(g) at STP is 0.00125 g/cm3.
What is the total number of grams of N2(g) in the airbag?
Use the density formula on Reference Table T:
'see explanation below'
12. Explain, in terms of electron configuration, why selenium and sulfur have similar chemical properties.
[1]
Both selenium (Se) and sulfur (S) are located in Group 16, and both have 6 valence electrons. [1 point]
'see explanation below'
13. Base your answer on the information below.
A metal, M, was obtained from a compound in a rock sample. Experiments have determined that the element
is a member of Group 2 on the Periodic Table of the Elements.
What is the phase of element M at STP? [1]
Every element in Group 2 is a solid at STP. [1 point]
'see explanation below'
14. Base your answer on the information below.
Elements with atomic numbers 112 and 114 have been produced and their IUPAC names are pending
approval. However, an element that would be put between these two elements on the Periodic Table has not
yet been produced. If produced, this element will be identified by the symbol Uut until an IUPAC name is
approved.
Identify one element that would be chemically similar to Uut. [1]
Any element in Group 13 would be chemically similar to Uut: boron (B), aluminum (Al), gallium (Ga),
indium (In), or thallium (Tl).
'see explanation below'
15. Base your answer on the accompanying information.
Identify one element from this table for each type of element: metal, metalloid, and nonmetal. [1]
Refer to the abbreviated Periodic Table of the Elements shown on the accompanying image:
The metals on this table are Sn and Pb. The metalloids are Si and Ge. The nonmetal is C. You need to
choose only one from each category. [1 point]
'see explanation below'
16. Base your answer on the elements in Group 2 on the Periodic Table.
State the general trend in first ionization energy for the elements in Group 2 as these elements are
considered in order from top to bottom in the group. [1]
Use the Periodic Table of the Elements and Reference Table S. The accompanying table lists the first
ionization energies of the elements in Group 2 (from top to bottom):
As the atomic number of Group 2 elements increases, the first ionization energy decreases. [1 point]
'see explanation below'
17. Base your answer on the elements in Group 2 on the Periodic Table.
State, in terms of the number of electron shells, why the radius of a strontium atom in the ground state is
larger than the radius of a magnesium atom in the ground state. [1]
A strontium atom in the ground state has two more electron shells than a magnesium atom in the ground
state. As a result, a strontium atom is larger than a magnesium atom. [1 point]
'see explanation below'
18. Base your answer on the elements in Group 2 on the Periodic Table.
Explain, in terms of atomic structure, why the elements in Group 2 have similar chemical properties. [1]
Chemical properties depend on the number of valence electrons in an atom. Each element in Group 2 has
two valence electrons. [1 point]
'see explanation below'
19. Base your answer on the information below.
The radioisotope uranium-238 occurs naturally in Earth's crust. The disintegration of this radioisotope is the
first in a series of spontaneous decays.
The sixth decay in this series produces the radioisotope radon-222. The decay of radon-222 produces the
radioisotope polonium-218 that has a half life of 3.04 minutes. Eventually, the stable isotope lead-206 is
produced by the alpha decay of an unstable nuclide.
Explain, in terms of electron configuration, why atoms of the radioisotope produced by the sixth decay in
the U-238 disintegration series do not readily react to form compounds. [1]
Use the Periodic Table of the Elements. Radon (Rn, atomic number 86) is a noble gas. It is found in Group
18. Elements in Group 18 have completed outer (valence) shells of electrons and do not readily form
compounds. [1 point]
'see explanation below'
20. Base your answer on the accompanying information.
Identify one element from this table for each type of element: metal, metalloid, and nonmetal. [1]
Refer to the abbreviated Periodic Table of the Elements shown on the accompanying image:
The metals on this table are Sn and Pb. The metalloids are Si and Ge. The nonmetal is C. You need to
choose only one from each category. [1 point]
'see explanation below'
21. Base your answer on the elements in Group 2 on the Periodic Table.
State the general trend in first ionization energy for the elements in Group 2 as these elements are
considered in order from top to bottom in the group. [1]
Use the Periodic Table of the Elements and Reference Table S. The accompanying table lists the first
ionization energies of the elements in Group 2 (from top to bottom):
As the atomic number of Group 2 elements increases, the first ionization energy decreases. [1 point]
'see explanation below'
22. Base your answer on the elements in Group 2 on the Periodic Table.
State, in terms of the number of electron shells, why the radius of a strontium atom in the ground state is
larger than the radius of a magnesium atom in the ground state. [1]
A strontium atom in the ground state has two more electron shells than a magnesium atom in the ground
state. As a result, a strontium atom is larger than a magnesium atom. [1 point]
'see explanation below'
23. Base your answer on the elements in Group 2 on the Periodic Table.
Explain, in terms of atomic structure, why the elements in Group 2 have similar chemical properties. [1]
Chemical properties depend on the number of valence electrons in an atom. Each element in Group 2 has
two valence electrons. [1 point]
'see explanation below'
24. Base your answer on the information below.
The radioisotope uranium-238 occurs naturally in Earth's crust. The disintegration of this radioisotope is the
first in a series of spontaneous decays.
The sixth decay in this series produces the radioisotope radon-222. The decay of radon-222 produces the
radioisotope polonium-218 that has a half life of 3.04 minutes. Eventually, the stable isotope lead-206 is
produced by the alpha decay of an unstable nuclide.
Explain, in terms of electron configuration, why atoms of the radioisotope produced by the sixth decay in
the U-238 disintegration series do not readily react to form compounds. [1]
Use the Periodic Table of the Elements. Radon (Rn, atomic number 86) is a noble gas. It is found in Group
18. Elements in Group 18 have completed outer (valence) shells of electrons and do not readily form
compounds. [1 point]
'see explanation below'
25. Base your answer on the information below.
Ozone gas, O3, can be used to kill adult insects in storage bins for grain without damaging the grain. The
ozone is produced from oxygen gas, O2, in portable ozone generators located near the storage bins. The
concentrations of ozone used are so low that they do not cause any environmental damage. This use of
ozone is safer and more environmentally friendly than a method that used bromomethane, CH 3Br. However,
bromomethane was more effective than ozone because CH3Br killed immature insects as well as adult
insects.
Adapted From: The Sunday Gazette (Schenectady, NY) 3/9/03
Based on the information in the passage, state one advantage of using ozone instead of bromomethane for
insect control in grain storage bins. [1]
According to the paragraph, ozone is better to use than bromoethane because the low ozone concentration
does not cause any environmental damage.
[1 point]
'see explanation below'
26. Base your answer on the information below and the accompanying table.
The table shown lists physical and chemical properties of six elements at standard pressure that correspond
to known elements on the Periodic Table. The elements are identified by the code letters, D, E, G, J, L, and
Q.
What is the total number of elements in the "Properties of Six Elements at Standard Pressure" table that are
solids at STP? [1]
Use Reference Table A. The temperature at STP is 0oC (273 K). In order to be a solid at STP, the melting
point of the solid must be 0oC or greater. Four elements (E, G, L, and Q) have melting points above 0oC and
are therefore solids at STP.
[1 point]
'see explanation below'
27. Base your answer on the information below and the accompanying table.
The table shown lists physical and chemical properties of six elements at standard pressure that correspond
to known elements on the Periodic Table. The elements are identified by the code letters, D, E, G, J, L, and
Q.
An atom of element G is in the ground state. What is the total number of valence electrons in this atom? [1]
Since oxygen has an oxidation state of -2, the oxidation state of G in G2O must be +1. An atom of this
element will have one valence electron. (Note that this element can be identified using Reference Table S. It
is sodium, Na.)
[1 point]
'see explanation below'
28. Base your answer on the information below and the accompanying table.
The table shown lists physical and chemical properties of six elements at standard pressure that correspond
to known elements on the Periodic Table. The elements are identified by the code letters, D, E, G, J, L, and
Q.
Letter Z corresponds to an element on the Periodic Table other than the six listed elements. Elements G, Q,
L, and Z are in the same group on the Periodic Table, as shown in diagram A.
Based on the trend in the melting points for elements G, Q, and L listed in the "Properties of Six Elements at
Standard Pressure" table, estimate the melting point of element Z, in degrees Celsius. [1]
Refer to the accompanying table:
By assuming that these elements are listed in order of increasing atomic number, the periodic trend shows a
decrease in melting point as the atomic number increases. Therefore, any melting point below 64 oC is
acceptable for credit.
[1 point]
'see explanation below'
29. Base your answer on the information below and the accompanying table.
The table shown lists physical and chemical properties of six elements at standard pressure that correspond
to known elements on the Periodic Table. The elements are identified by the code letters, D, E, G, J, L, and
Q.
Identify, by code letter, the element that is a noble gas in the "Properties of Six Elements at Standard
Pressure" table. [1]
The only element that does not combine with oxygen to form an oxide is element D. (Note that this element
can be identified using Reference Table S. It is helium, He.)
[1 point]
'see explanation below'
30. Base your answer on the information below.
Arsenic is often obtained by heating the ore arsenopyrite, FeAsS. The decomposition of FeAsS is
represented by the balanced equation shown.
In the solid phase, arsenic occurs in two forms. One form, yellow arsenic, has a density of 1.97 g/cm 3 at
STP. The other form, gray arsenic, has a density of 5.78 g/cm3 at STP. When arsenic is heated rapidly in air,
arsenic(III) oxide is formed.
Although arsenic is toxic, it is needed by the human body in very small amounts. The body of a healthy
human adult contains approximately 5 milligrams of arsenic.
Explain, in terms of the arrangement of atoms, why the two forms of arsenic have different densities at STP.
[1]
In gray arsenic, the atoms are arranged closer together, resulting in more mass per unit volume.
[1 point]
'see explanation below'
31. Base your answer on the information below.
Two sources of copper are cuprite, which has the IUPAC name copper(I) oxide, and malachite, which has
the formula Cu2CO3(OH)2. Copper is used in home wiring and electric motors because it has good electrical
conductivity. Other uses of copper not related to its electrical conductivity include coins, plumbing, roofing,
and cooking pans. Aluminum is also used for cooking pans.
At room temperature, the electrical conductivity of a copper wire is 1.6 times greater than an aluminum wire
with the same length and cross-sectional area. At room temperature, the heat conductivity of copper is 1.8
times greater than the heat conductivity of aluminum. At STP, the density of copper is 3.3 times greater than
the density of aluminum.
Identify one physical property of aluminum that could make it a better choice than copper for a cooking pan.
[1]
Use Reference Table S. Aluminum has a lower density than copper. Therefore, an aluminum pan would
weigh less than an identical-size copper pan. [1 point]
'see explanation below'
32. Base your answer on the information below.
Two sources of copper are cuprite, which has the IUPAC name copper(I) oxide, and malachite, which has
the formula Cu2CO3(OH)2. Copper is used in home wiring and electric motors because it has good electrical
conductivity. Other uses of copper not related to its electrical conductivity include coins, plumbing, roofing,
and cooking pans. Aluminum is also used for cooking pans.
At room temperature, the electrical conductivity of a copper wire is 1.6 times greater than an aluminum wire
with the same length and cross-sectional area. At room temperature, the heat conductivity of copper is 1.8
times greater than the heat conductivity of aluminum. At STP, the density of copper is 3.3 times greater than
the density of aluminum.
Identify one physical property of copper that makes it a good choice for uses that are not related to electrical
conductivity. [1]
Two acceptable responses are:


Copper is very malleable.
Copper is a good conductor of heat.
Note that only one property need be listed in order to receive credit. [1 point]
4
33. The elements in Period 5 on the Periodic Table are arranged from left to right in order of
1. decreasing atomic mass
3. increasing atomic mass
2. decreasing atomic number
4. increasing atomic number
4 Refer to the Periodic Table of the Elements.
Elements are placed in order of increasing atomic
number.Wrong Choice Explained:(3) Element 53 (I)
has a smaller atomic mass than element 52 (Te).
1. Zn, Ga, Ge
2. Si, Ge, Sn
3
34. Which list of elements contains a metal, a metalloid, and a
nonmetal?
3. Cd, Sb, I
4. F, Cl, Br
3 Refer to the Periodic Table of the Elements. Cd,
located in Group 12 and to the left of the metal1
nonmetal line, is a metal; Sb, located in Group 15 and 35. Which element is malleable and conducts electricity?
on the metal-nonmetal line, is a metalloid; I, located
in Group 17 and to the right of the metal-nonmetal
line, is a nonmetal.
WRONG CHOICES EXPLAINED:
(1) Zn and Ga are metals; Ge is a metalloid.
(2) Si and Ge are metalloids; Sn is a metal.
(4) F, Cl, and Br are nonmetals.
1. iron
2. iodine
3. sulfur
4. phosphorus
4
36. At STP, solid carbon can exist as graphite or as diamond.
These two forms of carbon have
1. the same properties and the same crystal structures 3. different properties and the same crystal structures
2. the same properties and different crystal structures 4. different properties and different crystal structures
1 Malleability and conductivity are properties found
in metallic substances such as iron.
4 Graphite and diamond have distinctly different
crystal stuctures. Therefore, they will have different
properties as well.
1. iron
2. iodine
1
37. Which element is malleable and conducts electricity?
3. sulfur
4. phosphorus
4
38. At STP, solid carbon can exist as graphite or as diamond.
These two forms of carbon have
1. the same properties and the same crystal structures 3. different properties and the same crystal structures
2. the same properties and different crystal structures 4. different properties and different crystal structures
1 Malleability and conductivity are properties found
in metallic substances such as iron.
4 Graphite and diamond have distinctly different
crystal stuctures. Therefore, they will have different
properties as well.
1. Zn, Ga, Ge
2. Si, Ge, Sn
3
39. Which list of elements contains a metal, a metalloid, and a
nonmetal?
3. Cd, Sb, I
4. F, Cl, Br
3 Refer to the Periodic Table of the Elements. Cd,
located in Group 12 and to the left of the metalnonmetal line, is a metal; Sb, located in Group 15 and
on the metal-nonmetal line, is a metalloid; I, located
in Group 17 and to the right of the metal-nonmetal
4
line, is a nonmetal.
40. The elements in Period 5 on the Periodic Table are arranged
from left to right in order of
WRONG CHOICES EXPLAINED:
(1) Zn and Ga are metals; Ge is a metalloid.
(2) Si and Ge are metalloids; Sn is a metal.
(4) F, Cl, and Br are nonmetals.
1. decreasing atomic mass
3. increasing atomic mass
2. decreasing atomic number
4. increasing atomic number
4 Refer to the Periodic Table of the Elements.
Elements are placed in order of increasing atomic
number.Wrong Choice Explained:(3) Element 53 (I)
has a smaller atomic mass than element 52 (Te).
1. calcium
2. fluorine
2
41. An atom in the ground state has seven valence electrons. This
atom could be an atom of which element?
3. oxygen
4. sodium
representative elements (Groups 1, 2, and 13 through
18) are classified by the number of valence electrons
1
contained in each ground-state atom of the element.
42. Which statement identifies the element arsenic?
Refer to the acompanying table: Of the choices given,
only choice (2), fluorine, is located in Group 17.
3. An atom of arsenic in the ground state has eight
1. Arsenic has an atomic number of 33.
valence electrons.
4. An atom of arsenic in the ground state has a radius
2. Arsenic has a melting point of 84 K.
of 146 pm.
1 Elements are primarily identified by their atomic
numbers. Refer to the Periodic Table of the Elements.
Arsenic (As) has an atomic number of 33.
Wrong Choices Explained:
(2) See Reference Table S. The melting point of
arsenic is 1090 K.
(3) Arsenic is located in Group 15. An atom of
arsenic contains 5 valence electrons.
(4) See Reference Table S. The atomic radius of an
arsenic atom is 139 pm.
1. electron shells
2. valence electrons
2 Elements with similar chemical properties are
located in the same group of the Periodic Table of the
Elements. Elements within a single representative
group have the same number of valence electrons.
(See Question 1.)
1. Al
2. Ar
2
43. Magnesium and calcium have similar chemical properties
because an atom of each element has the same total number of
3. neutrons
4. protons
3
44. Which element is a metalloid?
3. As
4. Au
3 Refer to the accompanying diagram of the
abbreviated Periodic Table of the Elements and to
Reference Table S.
3
45. An element that is malleable and a good conductor of heat
The metalloids have been shaded in the table. Of the and electricity could have an atomic number of
choices given, only arsenic (As) is a metalloid.
1. 16
3. 29
2. 18
4. 35
3 Refer to the Periodic Table of the Elements. The
description given in this question refers to an element
with metallic properties. Of the choices given, only
element number 29 (copper, Cu) is a metallic
3
element.
46. The compound X Cl is classified as ionic if X represents the
element
Wrong Choices Explained:
(1), (4) Elements number 16 and 35 (S and Br) are
nonmetallic elements.
(2) Element number 18 (Ar) is a noble gas.
1. H
2. I
3. Rb
4. Br
3 If a binary compound (such as X Cl) is ionic, the
4
electronegativity difference between X and Cl must
be 1.7 or more. See Reference Table S. Of the choices
given, only choice (3), Rb, produces an
electronegativity difference with Cl greater than or
equal to 1.7.
1. atomic number
2. mass number
4 Elements with similar chemical properties are
located in the same group of the Periodic Table of the
Elements. The similarity in their properties is because
elements within a group have the same total number
of valence electrons.
1. 6
2. 8
3 The mass number of an isotope is the sum of the
protons and neutrons contained within its nucleus.
1. barium
2. beryllium
47. Magnesium and calcium have similar chemical properties
because a magnesium atom and a calcium atom have the same
3. total number of electron shells
4. total number of valence electrons
3
48. What is the mass number of a carbon atom that contains six
protons, eight neutrons, and six electrons?
3. 14
4. 20
4
49. Which element has the greatest density at STP?
3. magnesium
4. radium
4 See Reference Table S. Of the four elements listed, 1
50. At STP, solid carbon can exist as diamond and graphite.
the element radium (element number 88) has the
Compared to the molecular structure and chemical properties of
greatest density as STP.
diamond, graphite has
1. a different molecular structure and different
3. the same molecular structure and different
properties
properties
2. a different molecular structure and the same
4. the same molecular structure and the same
properties
properties
1 Diamond and graphite have different molecular
structures. Therefore, they have different chemical
and physical properties.
1. carbon
2. germanium
4
51. Which Group 14 element is classified as a metal?
3. silicon
4. tin
4 Refer to the Periodic Table of the Elements and the
accompanying diagram. The diagram is a small
portion of the Periodic Table. The metalloids are
shaded in this table. Metallic elements lie below the
metalloids, and nonmetallic elements lie above them. 1
Of the choices given, only choice (4), tin, is a
52. Which element forms a compound with chlorine with the
metallic element in Group 14.
general formula MCl?
Wrong Choices Explained:
(1) Carbon is a nonmetallic element.
(2), (3) Germanium and silicon are metalloids.
1. Rb
2. Ra
3. Re
4. Rn
1 Use the Periodic Table of the Elements. Chlorine
(Cl, atomic number 17) has an oxidation state of –1.
In the compound MCl, the oxidation state of M must
be +1. Of the choices given, only choice (1), Rb
(atomic number 37), has an oxidation state of +1.
3
53. Which characteristics both generally decrease when the
elements in Period 3 on the Periodic Table are considered in order
from left to right?
1. nonmetallic properties and atomic radius
2. nonmetallic properties and ionization energy
3 Use the Periodic Table of the Elements and
Reference Table S. As one proceeds across Period 3
from Na to Ar, the properties of the elements change
from metal to metalloid to nonmetal to noble gas.
Therefore, the metallic properties decrease. Table S
reveals that the atomic radii of the eight successive
elements all decrease from 190 pm to 88 pm.
1. more protons than neutrons
2. more neutrons than protons
4 Use the Periodic Table of the Elements. When
atoms bond, they generally complete a valence shell
that will contain either 2 or 8 electrons. Since an atom
of argon (Ar, atomic number 18) is a noble gas and
already has 8 valence electrons, it will not bond with
another atom.
1. atomic number
2. mass number
1 The Periodic Table is arranged in order of
increasing atomic number because this arrangement
displays the repeating nature of physical and
chemical properties.
1. each atom in the sample has 29 protons
2. atoms in the sample react with oxygen
1 An element is defined by its atomic number—the
number of protons in the nucleus of each atom. Refer
to the Periodic Table of the Elements. The atomic
number of copper (Cu) is 29.
1. tantalum
2. rhenium
2 Use Reference Table S. Rhenium (element number
75), with a melting point of 3453 K, has a higher
melting point than any of the other elements listed in
the question.
1. the same crystal structure and the same properties
2. the same crystal structure and different properties
3. metallic properties and atomic radius
4. metallic properties and ionization energy
4
54. An atom of argon in the ground state tends not to bond with
an atom of a different element because the argon atom has
3. a total of two valence electrons
4. a total of eight valence electrons
1
55. The elements on the Periodic Table are arranged in order of
increasing
3. number of isotopes
4. number of moles
1
56. A sample of matter must be copper if
3. the sample melts at 1768 K
4. the sample can conduct electricity
2
57. Which element has the highest melting point?
3. osmium
4. hafnium
4
58. At STP, both diamond and graphite are solids composed of
carbon atoms. These solids have
3. different crystal structures and the same properties
4. different crystal structures and different properties
4 Diamond and graphite are allotropes of the element 1
carbon. As such, they have different crystal structures 59. Compared to the atoms of nonmetals in Period 3, the atoms of
and different chemical and physical properties.
metals in Period 3 have
1. fewer valence electrons
3. fewer electron shells
2. more valence electrons
4. more electron shells
1 Valence electrons are the electrons in the outermost
shell of an atom. Refer to the Periodic Table of the
Elements. The metals of Period 3 (Na, Mg, and Al) 3
have 1, 2, and 3 valence electrons, respectively. The 60. Which elements are malleable and good conductors of
nonmetals of Period 3 (P, S, and Cl) have 5, 6, and 7 electricity?
valence electrons, respectively.
1. iodine and silver
2. iodine and xenon
3 Use the Periodic Table of the Elements. Metallic
elements are good conductors of electricity. Of the
choices given, only choice (3), tin and silver, are both
metallic elements.
1. lithium atom
2. potassium atom
3 The first ionization energy measures the amount of
energy needed to remove the most loosely held
electron from a ground-state atom. Use Reference
Table S. Of the choices given, rubidium (Rb), has the
smallest first ionization and, therefore, requires the
least amount of energy to remove its single valence
electron.
3. tin and silver
4. tin and xenon
3
61. Which atom in the ground state requires the least amount of
energy to remove its valence electron?
3. rubidium atom
4. sodium atom