Chemistry Chapter 5
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.
a
Among the alkali metals below, which has the lowest melting point? a. sodium (atomic number 11) c. rubidium (atomic number 37) b. potassium (atomic number 19) d. cesium (atomic number 55)
a
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.
a
As you move down the periodic table from carbon through lead, atomic radii a. generally increase. c. do not change. b. generally decrease. d. vary unpredictably.
a
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
a
Elements in which the d-sublevel is being filled have the properties of a. metals. c. metalloids. b. nonmetals. d. gases.
a
For each successive electron removed from an atom, the ionization energy a. increases. c. remains the same. b. decreases. d. shows no pattern.
a
For elements in Groups 1, 2, and 18, the increase in atomic number for successive elements follows the pattern 8, 8, 18, ____, 32. a. 18 c. 24 b. 20 d. 26
a
If n stands for the highest occupied energy level, the outer configuration for all Group 1 elements is a. ns1. c. n - s. b. 2n. d. np1.
a
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.
a
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. 72 b. 68 d. 90
a
Magnesium, atomic number 12, has the electron configuration [Ne] 3s2. To what group does magnesium belong? a. Group 2 c. Group 5 b. Group 3 d. Group 12
a
Mendeleev did not always list elements in his periodic table in order of increasing atomic mass because he grouped together elements with similar a. properties. c. densities. b. atomic numbers. d. colors.
a
Mendeleev is credited with developing the first successful a. periodic table. b. method for determining atomic number. c. test for radioactivity. d. use of X rays.
a
Strontium's highest occupied energy level is 5s2. To what group does strontium belong? a. Group 2 c. Group 6 b. Group 4 d. Group 8
a
The alkali metals belong to the ____-block in the periodic table. a. s c. d b. p d. f
a
The energy required to remove an electron from an atom ____ as you move left to right from potassium through iron. a. generally increases c. does not change b. generally decreases d. varies unpredictably
a
The first member of the noble gas family, whose highest energy level consists of an octet of electrons, is a. helium. c. neon. b. argon. d. krypton.
a
The force of attraction by Group 1 metals for their valence electrons is a. weak. b. zero. c. strong. d. greater than that for inner shell electrons.
a
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.
a
The most reactive group of the nonmetals are the a. lanthanides. c. halogens. b. transition elements. d. rare-earth elements.
a
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.
a
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.
a
The person whose work led to a periodic table based on increasing atomic number was a. Moseley. c. Rutherford. b. Mendeleev. d. Cannizzaro.
a
To which group do lithium and potassium belong? Refer to the figure above. a. alkali metals c. halogens b. transition metals d. noble gases
a
What are the elements whose discovery added an entirely new row to Mendeleev's periodic table? a. noble gases c. transition elements b. radioactive elements d. metalloids
a
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
a
When an electron is acquired by a neutral atom, the energy change is called a. electron affinity. c. ionization energy. b. electronegativity. d. electron configuration.
a
Which represents a neutral atom acquiring an electron in an exothermic process? a. A + e- + energy → A- c. A + e- → A- + energy b. A + e- → A- - energy d. A- + energy → A + e-
a
Within a group of elements, as the atomic number increases, the atomic radius a. increases. c. decreases regularly. b. remains approximately constant. d. decreases, but not regularly.
a
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.
c
A positive ion is known as a(n) a. ionic radius. c. cation. b. valence electron. d. anion
c
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. 88 b. 74 d. 103
c
Compared to the alkali metals, the alkaline-earth metals a. are less reactive. c. are less dense. b. have lower melting points. d. combine more readily with nonmetals.
c
For groups 1, 2, and 18, the atomic number of the fourth element in the group is ____ more than the preceding element. a. 3 c. 18 b. 4 d. 20
c
In Period 3 there are 8 elements. What sublevel(s) is (are) being filled? a. s c. s and p b. s and d d. d and f
c
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.
c
Mendeleev left spaces in his periodic table and predicted several elements and their a. atomic numbers. c. properties. b. colors. d. radioactivity.
c
Nitrogen's electron configuration is 1s2 2s2 2p3. To what group does nitrogen belong? a. Group 2 c. Group 15 b. Group 7 d. Group 17
c
One-half the distance between the nuclei of identical atoms that are bonded together is called the a. atomic radius. c. atomic volume. b. atomic diameter. d. electron cloud.
c
Period 4 contains 18 elements. How many of these elements have electrons in the d sublevel? a. 8 c. 16 b. 10 d. 18
c
Refer to the figure above. To which group do fluorine and chlorine belong? a. alkaline-earth metals c. halogens b. transition elements d. actinides
c
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.
c
The discovery of the noble gases changed Mendeleev's periodic table by adding a new a. period. c. group. b. series. d. sublevel block.
c
The electron configuration of an element is [Kr] 4d6 5s1. To what group does this element belong? a. Group 4 c. Group 7 b. Group 5 d. Group 9
c
The elements in Group 1 are also known as the a. alkali metals. c. Period 1 elements. b. rare-earth series. d. actinide series.
c
The elements that border the zigzag line in the periodic table are a. inactive. c. metalloids. b. metals. d. nonmetals.
c
The length of each period in the periodic table is determined by the a. atomic masses of the elements. b. atomic numbers of the elements. c. sublevels being filled with electrons. d. number of isotopes of the elements in the period.
c
The most characteristic property of the noble gases is that they a. have low boiling points. c. are gases at ordinary temperatures. b. are radioactive. d. are largely unreactive.
c
The most useful source of general information about the elements for anyone associated with chemistry is a a. calculator. c. periodic table. b. table of metric equivalents. d. table of isotopes.
c
The periodic law states that the properties of elements are periodic functions of their atomic numbers. This means that the ____ determines the position of each element in the periodic table. a. mass number c. number of protons b. number of neutrons d. number of nucleons
c
Titanium, atomic number 22, has the configuration [Ar] 3d2 4s2. To what group does titanium belong? a. Group 2 c. Group 4 b. Group 3 d. Group 5
c
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
c
When determining the size of an atom by measuring the distance between identical adjacent nuclei, the radius of an atom is a. equal to the distance between nuclei. c. twice the distance between nuclei. b. one-half the distance between nuclei. d. one-fourth the distance between nuclei.
c
Which is the best reason that the atomic radius generally increases with atomic number in each group of elements? a. The nuclear charge increases. c. The number of energy levels increases. b. The number of neutrons increases. d. A new octet forms.
c
Which orbitals are characteristic of the lanthanide elements? a. d orbitals c. f orbitals b. s orbitals d. p orbitals
c
Which two periods have the same number of elements? a. 2 and 4 c. 4 and 5 b. 3 and 4 d. 5 and 6
c
A negative ion is known as a(n) a. ionic radius. c. cation. b. valence electron. d. anion.
d
Atomic size is determined by measuring the a. radius of an individual atom. b. distance between nuclei of adjacent atoms. c. diameter of an individual atom. d. volume of the electron cloud of adjacent atoms.
d
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.
d
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.
d
Identify the sublevels in a period that contains 32 elements. a. s, f c. s, p, d b. s, p d. s, p, d, f
d
In developing his periodic table, Mendeleev listed on cards each element's name, atomic mass, and a. atomic number. c. isotopes. b. electron configuration. d. properties.
d
In the alkaline-earth group, atoms with the smallest radii a. are the most reactive. c. are all gases. b. have the largest volume. d. have the highest ionization energies.
d
Ionization energy is the energy required to remove ____ from an atom of an element. a. the electron cloud c. an electron b. the nucleus d. an ion
d
Mendeleev noticed that properties of elements usually repeated at regular intervals when the elements were arranged in order of increasing a. atomic number. c. reactivity. b. density. d. atomic mass.
d
Mendeleev predicted that the spaces in his periodic table represented a. isotopes. c. permanent gaps. b. radioactive elements. d. undiscovered elements.
d
Moseley's work led to the realization that elements with similar properties occurred at regular intervals when the elements were arranged in order of increasing a. atomic mass. c. radioactivity. b. density. d. atomic number.
d
Neutral atoms with an s2p6 electron configuration in the highest energy level are best classified as a. metalloids. c. nonmetals. b. metals. d. gases.
d
The electron configurations of the noble gases from neon to radon in the periodic table end with filled a. f orbitals. c. s orbitals. b. d orbitals. d. p orbitals.
d
The elements whose electron configurations end with s2 p5 in the highest occupied energy level belong to Group a. 3. c. 10. b. 7. d. 17.
d
The ionization energies for removing successive electrons from sodium are 496 kJ/mol, 4562 kJ/mol, 6912 kJ/mol, and 9544 kJ/mol. The great jump in ionization energy after the first electron is removed indicates that a. sodium has four or five electrons. b. the atomic radius has increased. c. a d-electron has been removed. d. the noble gas configuration has been reached.
d
The period of an element can be determined from its a. reactivity. c. symbol. b. density. d. electron configuration.
d
When an electron is added to a neutral atom, a certain amount of energy is a. always absorbed. c. either released or absorbed. b. always released. d. burned away.
d
When chemical compounds form, valence electrons are those that may be a. lost only. c. shared only. b. gained only. d. lost, gained, or shared.
d
Who used his experimental evidence to determine the order of the elements according to atomic number? a. Meyer c. Stas b. Ramsay d. Moseley
d
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.
d
A horizontal row of blocks in the periodic table is called a(n) a. group. c. family. b. period. d. octet.
b
Argon, krypton, and xenon are a. alkaline earth metals. c. actinides. b. noble gases. d. lanthanides.
b
As you move left to right from gallium through bromine, atomic radii a. generally increase. c. do not change. b. generally decrease. d. vary unpredictably.
b
Because the first energy level contains only the 1s sublevel, the number of elements in this period is a. 1. c. 4. b. 2. d. 8.
b
Calcium, atomic number 20, has the electron configuration [Ar] 4s2. In what period is calcium? a. Period 2 c. Period 8 b. Period 4 d. Period 20
b
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.
b
Evidence gathered since Mendeleev's time indicates that a better arrangement than atomic mass for elements in the periodic table is an arrangement by a. mass number. c. group number. b. atomic number. d. series number.
b
How many elements are in a period in which only the s and p sublevels are filled? a. 2 c. 18 b. 8 d. 32
b
In nature, the alkali metals occur as a. elements. c. complex ions. b. compounds. d. gases.
b
Mendeleev attempted to organize the chemical elements based on their a. symbols. c. atomic numbers. b. properties. d. electron configurations.
b
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.
b
Periods with occupied f sublevels a. have only Group 1 and 2 elements. c. have 32 groups. b. are not assigned group numbers. d. contain only Group 18 elements.
b
The electron configuration of aluminum, atomic number 13, is [Ne] 3s2 3p1. Aluminum is in Period a. 2. c. 6. b. 3. d. 13.
b
The electron configuration of cesium, atomic number 55, is [Xe] 6s1. In what period is cesium? a. Period 1 c. Period 8 b. Period 6 d. Period 55
b
The electrons available to be lost, gained, or shared when atoms form molecules are called a. ions. c. d electrons. b. valence electrons. d. electron clouds.
b
The element that has the greatest electronegativity is a. oxygen. c. chlorine. b. sodium. d. fluorine.
b
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.
b
The group of 14 elements in the sixth period that have occupied 4f orbitals is the a. actinides. c. transition elements. b. lanthanides. d. metalloids.
b
The group of soft, silvery active 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.
b
The ionization energies required to remove successive electrons from one mole of calcium atoms are 590 kJ/mol, 1145 kJ/mol, 4912 kJ/mol, and 6474 kJ/mol. The most common ion of calcium is probably a. Ca+. c. Ca3+. b. Ca2+. d. Ca4+.
b
The periodic law states that a. no two electrons with the same spin can be found in the same place in an atom. b. the physical and chemical properties of the elements are functions of their atomic numbers. c. electrons exhibit properties of both particles and waves. d. the chemical properties of elements can be grouped according to periodicity but physical properties cannot.
b
The periodic law states that the physical and chemical properties of elements are periodic functions of their atomic a. masses. c. radii. b. numbers. d. structures.
b
The principle that states that the physical and chemical properties of the elements are periodic functions of their atomic numbers is a. the periodic table. c. the law of properties. b. the periodic law. d. Mendeleev's law.
b
