unit 5

Question 89 100 pts The number of valence electrons in Group 1 elements is 1. 2. 8. equal to the period number.

1

Question 20 100 pts The atomic number of lithium, the first element in Group 1, is 3. The atomic number of the second element in this group is 4. 10. 11. 18.

11

Question 34 100 pts Period 4 contains 18 elements. How many of these elements have electrons in the d sublevel? 8 10 16 18

16

Question 46 100 pts The elements whose electron configurations end with s2 p5 in the highest occupied energy level belong to Group 3. 7. 10. 17.

17

Question 21 100 pts How much greater is the atomic number of the fourth element in groups 1, 2 and 18 than the preceding element? 3 4 18 20

18

Question 24 100 pts For elements in groups 1, 2, and 18, the increase in atomic number for successive elements follows the pattern 8, 8, 18, ?, 32. What number completes the pattern? 18 20 24 26

18

Question 32 100 pts Because the first energy level contains only the 1s sublevel, the number of elements in this period is 1. 2. 4. 8.

2

Question 28 100 pts The electron configuration of aluminum, atomic number 13, is [Ne] 3s2 3p1. Aluminum is in Period 2. 3. 6. 13.

3

Question 22 100 pts Krypton, atomic number 36, is the fourth element in Group 18. What is the atomic number of xenon, the fifth element in Group 18? 54 68 72 90

54

Question 53 100 pts Bromine, atomic number 35, belongs to Group 17. How many electrons does bromine have in its outermost energy level? 7 17 18 35

7

Question 91 100 pts The number of valence electrons in Group 17 elements is 7. 8. 17. equal to the period number.

7

Question 30 100 pts How many elements are in a period in which only the s and p sublevels are filled? 2 8 18 32

8

Question 23 100 pts Barium, atomic number 56, is the fifth element in Group 2. What is the atomic number of radium, the next element in Group 2? 64 74 88 103

88

Question 65 100 pts Which represents a neutral atom acquiring an electron in a process where energy is released? A + e- + energy ® A- A + e- ® A- - energy A + e- ® A- + energy A- + energy ® A + e-

A + e- ® A- + energy

Question 81 100 pts 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 Ca+. Ca2+. Ca3+. Ca4+.

Ca2+.

Question 51 100 pts Nitrogen's electron configuration is 1s2 2s2 2p3. To what group does nitrogen belong? Group 2 Group 7 Group 15 Group 17

Group 15

Question 54 100 pts Magnesium, atomic number 12, has the electron configuration [Ne] 3s2. To what group does magnesium belong? Group 2 Group 3 Group 5 Group 12

Group 2

Question 50 100 pts Titanium, atomic number 22, has the configuration [Ar] 3d2 4s2. To what group does titanium belong? Group 2 Group 3 Group 4 Group 5

Group 4

Question 52 100 pts The electron configuration of an element is [Kr] 4d6 5s1. To what group does this element belong? Group 4 Group 5 Group 7 Group 9

Group 7

Question 85 100 pts 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? It generally increases. It generally decreases. It does not change. It varies unpredictably.

It generally increases.

Question 1 100 pts The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed to Mendeleev. Moseley. Bohr. Ramsay.

Mendeleev

Question 2 100 pts Mendeleev left spaces in his periodic table and predicted the existence of three elements and their atomic numbers. colors. properties. radioactivity.

Properties

Question 80 100 pts Which is the best reason that the atomic radius generally increases with atomic number in each group of elements? The nuclear charge increases. The number of neutrons increases. The number of occupied energy levels increases. A new octet forms.

The number of occupied energy levels increases.

Question 56 100 pts The elements in Group 1 are also known as the alkali metals. rare-earth series. Period 1 elements. actinide series.

alkali metals.

Question 59 100 pts The group of soft, silvery, reactive metals, all of which have one electron in an s orbital, is known as the alkaline-earth metals. transition metals. alkali metals. metalloids.

alkali metals.

Question 69 100 pts What is removed when the ionization energy is supplied to an atom of an element? the electron cloud the nucleus an electron an ion

an electron

Question 73 100 pts A negative ion is known as a(n) ionic radius. valence electron. cation. anion.

anion.

Question 61 100 pts The most characteristic property of the noble gases is that they have low boiling points. are radioactive. are gases at ordinary temperatures. are largely unreactive.

are largely unreactive.

Question 42 100 pts Within the p-block elements, the elements at the top of the table, compared with those at the bottom, have larger radii. are more metallic. have lower ionization energies. are less metallic.

are less metallic

Question 62 100 pts Compared to the alkali metals, the alkaline-earth metals are less reactive. have lower melting points. are less dense. combine more readily with nonmetals.

are less reactive.

Question 3 100 pts Mendeleev noticed that properties of elements usually repeated at regular intervals when the elements were arranged in order of increasing atomic number. density. reactivity. atomic mass.

atomic mass

Question 7 100 pts 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 atomic mass. density. radioactivity. atomic number.

atomic number

Question 9 100 pts Evidence gathered since Mendeleev's time indicates that a better arrangement than atomic mass for elements in the periodic table is an arrangement by mass number. atomic number. group number. series number.

atomic number

Question 68 100 pts One-half the distance between the nuclei of identical atoms that are bonded together is called the atomic radius. atomic diameter. atomic volume. electron cloud.

atomic radius.

Question 72 100 pts A positive ion is known as a(n) ionic radius. valence electron. cation. anion

cation.

Question 55 100 pts In nature, the alkali metals occur as elements. compounds. complex ions. gases.

compounds.

Question 74 100 pts In a row in the periodic table, as the atomic number increases, the atomic radius generally decreases. remains constant. increases. becomes immeasurable.

decreases.

Question 64 100 pts When an electron is added to a neutral atom, a certain amount of energy is always absorbed. always released. either released or absorbed. transferred to the more electronegative element

either released or absorbed.

Question 70 100 pts When an electron is acquired by a neutral atom, the energy change is called electron affinity. electronegativity. ionization energy. electron configuration.

electron affinity.

Question 35 100 pts The period of an element can be determined from its reactivity. density. symbol. electron configuration

electron configuration

Question 67 100 pts A measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound is called electron affinity. electron configuration. electronegativity. ionization potential.

electronegativity.

Question 39 100 pts Neutral atoms with an s2p6 electron configuration in the highest energy level belong to which block of the periodic table? s block p block d block f block

f block

Question 45 100 pts To which block do the actinide elements belong? d block s block f block p block

f block

Question 71 100 pts The element that has the greatest electronegativity is oxygen. sodium. chlorine. fluorine.

fluorine.

Question 84 100 pts As you move left to right in Period 4 from gallium through bromine, atomic radii generally increase. generally decrease. do not change. vary unpredictably.

generally decrease.

Question 83 100 pts As you move down Group 14 in the periodic table from carbon through lead, atomic radii generally increase. generally decrease. do not change. vary unpredictably.

generally increase.

Question 78 100 pts Across a period in the periodic table, atomic radii gradually decrease. gradually decrease, then sharply increase. gradually increase. gradually increase, then sharply decrease.

gradually decrease.

Question 48 100 pts Strontium's highest occupied energy level is 5s2. To what group does strontium belong? Group 2 Group 5 Group 6 Group 8

group 2

Question 96 100 pts Which groups in the main group have lower electronegativity than d-block elements? groups 1 and 2 groups 13 through 18 groups 17 and 18 groups 13 through 17

groups 1 and 2

Question 25 100 pts Refer to the figure below. To which group do fluorine and chlorine belong? alkaline-earth metals transition elements halogens actinides

halogens

Question 58 100 pts The most reactive group of the nonmetals is the lanthanides. transition elements. halogens. noble gases.

halogens

Question 44 100 pts Hydrogen is placed separately from other elements in the periodic table because it is a gas. does not exist as a free element in nature. has atomic number one. has many unique properties.

has many unique properties

Question 76 100 pts In the alkaline-earth group, atoms with the smallest radii are the most reactive. have the largest volume. are all gases. have the highest ionization energies.

have the highest ionization energies.

Question 88 100 pts Valence electrons are those s and p electrons closest to the nucleus. in the lowest energy level. in the highest energy level. combined with protons.

in the highest energy level

Question 94 100 pts Across a period, ionization energies of d-block elements generally increase. decrease. remain constant. drop to zero.

increase

Question 97 100 pts Among the d-block elements, as atomic radii decrease, electronegativity values remain constant. increase. decrease. drop to zero.

increase

Question 75 100 pts Within a group of elements, as the atomic number increases, the atomic radius increases. remains approximately constant. decreases regularly. varies unpredictably.

increases.

Question 77 100 pts As the atomic number of the metals of Group 1 increases, the ionic radius increases. decreases. remains the same. cannot be determined.

increases.

Question 82 100 pts For each successive electron removed from an atom, the ionization energy increases. decreases. remains the same. shows no pattern.

increases.

Question 66 100 pts The energy required to remove an electron from an atom is the atom's electron affinity. electron energy. electronegativity. ionization energy.

ionization energy.

Question 41 100 pts The group of 14 f block elements in the sixth period is the actinides. lanthanides. transition elements. metalloids.

lanthanides

Question 40 100 pts Elements in which the d-sublevel is being filled have the properties of metals. nonmetals. metalloids. gases.

metals

Question 47 100 pts For groups 13 through 18, the total number of electrons in the highest occupied level equals the group number plus 1. minus 1. plus 5. minus 10.

minus 10

Question 92 100 pts For groups 13 through 18, the number of valence electrons is equal to the group number plus 1. plus the period number. minus the period number. minus 10.

minus 10

Question 6 100 pts The person whose work led to a periodic table based on increasing atomic number was Moseley. Mendeleev. Rutherford. Cannizzaro.

moseley

Question 60 100 pts The first member of the noble gas family, whose highest energy level consists of an octet of electrons, is helium. argon. neon. krypton.

neon.

Question 10 100 pts The discovery of what elements added a new column to Mendeleev's periodic table? noble gases radioactive elements transition elements metalloids

noble gases

Question 13 100 pts Argon, krypton, and xenon are alkaline earth metals. noble gases. actinides. lanthanides.

noble gases

Question 38 100 pts Elements to the right side of the periodic table (p-block elements) have properties most associated with gases. nonmetals. metals. metalloids.

nonmetals

Question 49 100 pts If n stands for the highest occupied energy level, the outer configuration for all Group 1 elements is ns1. 2n. n - s. np1.

ns1.

Question 15 100 pts The periodic law states that the properties of elements are periodic functions of their atomic numbers. What determines the position of each element in the periodic table? mass number number of neutrons number of protons number of isotopes

number of protons

Question 14 100 pts The periodic law states that the physical and chemical properties of elements are periodic functions of their atomic masses. numbers. radii. charges.

numbers

Question 63 100 pts When determining the size of an atom by measuring the distance between bonded, identical, adjacent nuclei, the radius of an atom is equal to the distance between nuclei. one-half the distance between nuclei. twice the distance between nuclei. one-fourth the distance between nuclei.

one-half the distance between nuclei.

Question 43 100 pts The electron configurations of the noble gases from neon to radon in the periodic table make these elements part of the f block. d block. s block. p block.

p block

Question 26 100 pts A horizontal row of blocks in the periodic table is called a(n) group. period. family. octet.

period

Question 27 100 pts Refer to the figure above. Potassium and bromine belong to Period 4. Group 4. Period 1. Group 1.

period 4

Question 36 100 pts Calcium, atomic number 20, has the electron configuration [Ar] 4s2. In what period is calcium? Period 2 Period 4 Period 8 Period 20

period 4

Question 31 100 pts The electron configuration of cesium, atomic number 55, is [Xe] 6s1. In what period is cesium? Period 1 Period 6 Period 8 Period 55

period 6

Question 8 100 pts The periodic table permits the properties of an element to be predicted before the element is discovered. will be completed with element 118. has been of little use to chemists since the early 1900s. was completed with the discovery of the noble gases.

permits the properties of an element to be predicted before the element is discovered.

Question 17 100 pts The periodic law allows some properties of an element to be predicted based on its position in the periodic table. number of isotopes. symbol. color.

position in the periodic table.

Question 4 100 pts Mendeleev did not always list elements in his periodic table in order of increasing atomic mass because he grouped together elements with similar properties. atomic numbers. densities. colors.

properties

Question 19 100 pts Elements in a group or column in the periodic table can be expected to have similar atomic masses. atomic numbers. numbers of neutrons. properties.

properties.

Question 57 100 pts Which block in the periodic table contains the alkali metals? s p d f

s

Question 90 100 pts In Group 2 elements, the valence electrons are in sublevel d. p. s. f.

s

Question 33 100 pts In Period 3 there are 8 elements. What sublevel(s) is (are) being filled? s s and d s and p d and f

s and p

Question 93 100 pts In groups 13 through 18, valence electrons may be in sublevels s and d. s and p. d and f. p and d.

s and p

Question 95 100 pts The first electrons to be removed when d-block elements form ions are the d electrons. p electrons. s electrons. f electrons.

s electrons

Question 29 100 pts Identify the sublevels in a period that contains 32 elements. s, f s, p s, p, d s, p, d, f

s, p, d, f

Question 11 100 pts What are the radioactive elements with atomic numbers from 90 to 103 called? the noble gases the lanthanides the actinides the rare-earth elements Flag this Question

the actinides

Question 12 100 pts What are the elements with atomic numbers from 58 to 71 called? the lanthanides the noble gases the actinides the alkali metals

the lanthanides

Question 79 100 pts 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 sodium has four or five electrons. the atomic radius has increased. a d electron has been removed. the noble gas configuration has been reached.

the noble gas configuration has been reached.

Question 16 100 pts The principle that states that the physical and chemical properties of the elements are periodic functions of their atomic numbers is the periodic table. the periodic law. the law of properties. Mendeleev's law.

the periodic law.

Question 18 100 pts The periodic law states that no two electrons with the same spin can be found in the same place in an atom. the physical and chemical properties of the elements are functions of their atomic numbers. electrons exhibit properties of both particles and waves. the chemical properties of elements can be grouped according to periodicity but physical properties cannot.

the physical and chemical properties of the elements are functions of their atomic numbers.

Question 5 100 pts Mendeleev predicted that the spaces in his periodic table represented isotopes. radioactive elements. unstable elements. undiscovered elements

undiscovered elements

Question 87 100 pts The electrons available to be lost, gained, or shared when atoms form compounds are called ions. valence electrons. d electrons. electron clouds.

valence electrons

Question 37 100 pts In the elements shown in the figure below, the s sublevel of the highest occupied energy level always contains one electron. always contains two electrons. varies in the number of electrons it contains. is always empty.

varies in the number of electrons it contains.

Question 86 100 pts The force of attraction by Group 1 metals for their valence electrons is weak. zero. strong. greater than that for inner shell electrons.

weak