Chapter 4-5

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. occurred at repeated intervals called periods.

Mendeleev attempted to organize the chemical elements based on their a. symbols. c. atomic numbers. b. properties. d. electron configurations.

b. properties.

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. the periodic law.

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. valence electrons.

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. 11.

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. 16

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-

c. A + e- A- + energy

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.

c. alkali metals.

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

c. an electron

A positive ion is known as a(n) a. ionic radius. c. cation. b. valence electron. d. anion

c. cation.

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.

c. either released or absorbed.

Which orbitals are characteristic of the lanthanide elements? a. d orbitals c. f orbitals b. s orbitals d. p orbitals

c. f orbitals

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. halogens

The most reactive group of the nonmetals are the a. lanthanides. c. halogens. b. transition elements. d. rare-earth elements.

c. halogens.

Valence electrons are those a. closest to the nucleus. c. in the highest energy level. b. in the lowest energy level. d. combined with protons.

c. in the highest energy level.

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. increasing atomic number.

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.

c. neon.

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.

c. s electrons.

In Group 2 elements, the valence electrons are in sublevel a. d. c. s. b. p. d. f.

c. s.

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. sublevels being filled with electrons.

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. the actinides

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. 17.

In compounds, d-block elements most often form ions with charge a. 2-. c. 1+. b. 1-. d. 2+.

d. 2+.

A negative ion is known as a(n) a. ionic radius. c. cation. b. valence electron. d. anion.

d. anion.

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.

d. are largely unreactive.

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. are less metallic.

The period of an element can be determined from its a. reactivity. c. symbol. b. density. d. electron configuration.

d. electron configuration.

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. have the highest ionization energies.

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.

d. ionization energy.

For Groups 13 through 18, the number of valence electrons is equal to the group number a. plus 1. c. minus the period number. b. plus the period number. d. minus 10.

d. minus 10.

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. minus 10.

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. p orbitals.

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. properties.

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 noble gas configuration has been reached.

Mendeleev predicted that the spaces in his periodic table represented a. isotopes. c. permanent gaps. b. radioactive elements. d. undiscovered elements.

d. undiscovered elements.

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. nonmetals.

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. numbers.

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. atomic number.

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. generally decrease.

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. lanthanides.

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. 18

The number of valence electrons in Group 2 elements is a. 2. c. 18. b. 8. d. equal to the period number.

a. 2.

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. 54

The number of valence electrons in Group 17 elements is a. 7. c. 17. b. 8. d. equal to the period number.

a. 7.

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. Group 2

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. Mendeleev.

The person whose work led to a periodic table based on increasing atomic number was a. Moseley. c. Rutherford. b. Mendeleev. d. Cannizzaro.

a. Moseley.

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. Ca2+.

The elements in Group 1 are also known as the a. alkali metals. c. Period 1 elements. b. rare-earth series. d. actinide series.

a. alkali metals.

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.

a. are less reactive.

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.

a. atomic radius.

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. decreases.

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. electron affinity.

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. generally increases

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. gradually decrease.

As with main-group elements, ionization energies of d-block elements generally ____ across a period. a. increase c. remain constant b. decrease d. drop to zero

a. increase

For each successive electron removed from an atom, the ionization energy a. increases. c. remains the same. b. decreases. d. shows no pattern.

a. increases.

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. noble gases

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. ns1.

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. periodic table.

The alkali metals belong to the ____-block in the periodic table. a. s c. d b. p d. f

a. s

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. weak.

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. are not assigned group numbers.

Argon, krypton, and xenon are a. alkaline earth metals. c. actinides. b. noble gases. d. lanthanides.

b. noble gases.

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. 2.