Deck 7: Periodic Properties of the Elements

Question 1

The atomic radius of main-group elements generally increases down a group because ________.

A)effective nuclear charge increases down a group
B)effective nuclear charge decreases down a group
C)effective nuclear charge zigzags down a group
D)the principal quantum number of the valence orbitals increases
E)both effective nuclear charge increases down a group and the principal quantum number of the valence orbitals increases

Answer 1

the principal quantum number of the valence orbitals increases

Question 2

Of the following, which gives the correct order for atomic radius for Ca, K, As, Ge and Kr?

A)Ca > K > As > Ge > Kr
B)Kr > Ge > As > K > Ca
C)Ge > As > Kr > K > Ca
D)K > Ca > Ge > As > Kr
E)Kr > As > Ge > Ca > K

Answer 2

K > Ca > Ge > As > Kr

Question 3

Screening of the nuclear charge by core electrons in atoms is ________.

A)less efficient than that by valence electrons
B)more efficient than that by valence electrons
C)essentially identical to that by valence electrons
D)responsible for a general decrease in atomic radius going down a group
E)both essentially identical to that by valence electrons and responsible for a general decrease in atomic radius going down a group

Answer 3

more efficient than that by valence electrons

Question 4

In which set of elements would all members be expected to have very similar chemical properties?

A)O, S, Se
B)N, O, F
C)Na, Mg, K
D)S, Se, Si
E)Ne, Na, Mg

Question 5

Which of the following correctly represents the third ionization of aluminum?

A)Al²⁺ (g) + e^- → Al⁺ (g)
B)Al (g) → Al⁺ (g) + e^-
C)Al^2- (g) + e^- → Al^3- (g)
D)Al²⁺ (g) + e^- → Al³⁺ (g)
E)Al²⁺ (g) → Al³⁺ (g) + e^-

Question 6

In which set of elements would all members be expected to have very similar chemical properties?

A)P, Se, I
B)Cl, Br, Na
C)Si, As, Te
D)Ne, Na, Mg
E)Br, I, At

Question 7

Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ar?

A)Mg > Na > P > Si > Ar
B)Ar > Si > P > Na > Mg
C)Si > P > Ar > Na > Mg
D)Na > Mg > Si > P > Ar
E)Ar > P > Si > Mg > Na

Question 8

Atomic radius generally decreases as we move ________.

A)down a group and from right to left across a period
B)up a group and from left to right across a period
C)down a group and from left to right across a period
D)up a group and from right to left across a period
E)down a group; the period position has no effect

Question 9

Atomic radius generally increases as we move ________.

A)down a group and from right to left across a period
B)up a group and from left to right across a period
C)down a group and from left to right across a period
D)up a group and from right to left across a period
E)down a group; the period position has no effect

Question 10

The effective nuclear charge of an atom is primarily affected by ________.

A)inner electrons
B)outer electrons
C)nuclear charge
D)electron distribution
E)orbital radial probability

Question 11

Which of the following correctly represents the second ionization of aluminum?

A)Al⁺ (g) + e^- → Al (g)
B)Al (g) → (g) + e^-
C)Al^- (g) + e^- → Al^2- (g)
D)Al⁺ (g) + e^- → Al²⁺ (g)
E)Al⁺ (g) → Al²⁺ (g) + e^-

Question 12

Which isoelectronic series is correctly arranged in order of increasing radius?

A)K⁺ < Ca²⁺ < Ar < Cl^-
B) < Ar < K⁺ < Ca²⁺
C)Ca²⁺ < Ar < K⁺ < Cl^-
D)Ca²⁺ < K⁺ < Ar < Cl^-
E)Ca²⁺ < K⁺ < Cl^- < Ar

Question 13

Of the choices below, which gives the order for first ionization energies?

A)Kr > Se > Br > Ga > Ge
B)Kr > Br > Se > Ge > Ga
C)Ga > Br > Ge > Kr > Se
D)Ga > Ge > Se > Br > Kr
E)Br > Se > Ga > Kr > Ge

Question 14

________ have the lowest first ionization energies of the groups listed.

A)Alkali metals
B)Transition elements
C)Halogens
D)Alkaline earth metals
E)Noble gases

Question 15

Which equation correctly represents the first ionization of calcium?

A)Ca (g) → Ca⁺ (g) + e^-
B)Ca (g) → Ca^- (g) + e^-
C)Ca (g) + e^- → Ca^- (g)
D)Ca^- (g) → Ca (g) + e^-
E)Ca⁺ (g) + e^- → Ca (g)

Question 16

Which of the following correctly represents the second ionization of phosphorus?

A)P⁺ (g) + e^- → P²⁺ (g)
B)P (g) → P⁺ (g) + e^-
C)P^- (g) + e^- → P^2- (g)
D)P⁺ (g) → P²⁺ (g) + e^-
E)P⁺ (g) + e^- → P (g)

Question 17

Of the choices below, which gives the order for first ionization energies?

A)Cl > S > Al > Ar > Si
B)Ar > Cl > S > Si > Al
C)Al > Si > S > Cl > Ar
D)Cl > S > Al > Si > Ar
E)S > Si > Cl > Al > Ar

Question 18

Electrons in the 1s subshell are much closer to the nucleus in Ar than in He due to the larger ________ in Ar.

A)nuclear charge
B)paramagnetism
C)diamagnetism
D)Hund's rule
E)azimuthal quantum number

Question 19

Of the compounds below, ________ has the smallest ionic separation.

A)KF
B)K₂S
C)RbCl
D)SrBr₂
E)RbF

Question 20

Which of the following is an isoelectronic series?

A)B^5-, Si^4-, As^3-, Te^2-
B)F^-, Cl^-, Br^-, I^-
C)S, Cl, Ar, K
D)Si^2-, P^2-, S^2-, Cl^2-
E)O^2-, F^-, Ne, Na⁺

Question 21

Which of the following correctly represents the electron affinity of phosphorus?

A)P (g) → P⁺ (g) + e^-
B)P (g) + e^- → P^- (g)
C)P₄ (g) + e^- → P^- (g)
D)P₄ (g) + 4e^- → 4P^- (g)
E)P⁺ (g) + e^- → P (g)

Question 22

Which of the following correctly represents the second ionization of calcium?

A)Ca (g) → Ca⁺ (g) + e^-
B)Ca⁺ (g) → Ca²⁺ (g) + e^-
C)Ca^- (g) + e^- → Ca^2- (g)
D)Ca⁺ (g) + e^- → Ca²⁺ (g)
E)Ca⁺ (g) + e^- → Ca (g)

Question 23

Consider the following electron configurations to answer the questions that follow:
(i)1s² 2s² 2p⁶ 3s¹
(ii)1s² 2s² 2p⁶ 3s²
(iii)1s² 2s² 2p⁶ 3s² 3p¹
(iv)1s² 2s² 2p⁶ 3s² 3p⁴
(v)1s² 2s² 2p⁶ 3s² 3p⁵
Of the following elements, ________ has the most negative electron affinity.

A)P
B)Al
C)Si
D)Cl
E)B

Question 24

The list that correctly indicates the order of metallic character is ________.

A)B > N > C
B)F > Cl > S
C)Si > P > S
D)P > S > Se
E)Na > K > Rb

Question 25

Which equation correctly represents the electron affinity of calcium?

A)Ca (g) + e^- → Ca^- (g)
B)Ca (g) → Ca⁺ (g) + e^-
C)Ca (g) → Ca^- (g) + e^-
D)Ca^- (g) → Ca (g) + e^-
E)Ca⁺ (g) + e^- → Ca (g)

Question 26

Which of the following correctly represents the electron affinity of bromine?

A)Br (g) → Br⁺ (g) + e^-
B)Br (g) + e^- → Br^- (g)
C)Br₂ (g) + e^- → Br^- (g)
D)Br₂ (g) + 2e^- → 2Br^- (g)
E)Br⁺ (g) + e^- → Br (g)

Question 27

Consider the following electron configurations to answer the questions that follow:
(i)1s² 2s² 2p⁶ 3s¹
(ii)1s² 2s² 2p⁶ 3s²
(iii)1s² 2s² 2p⁶ 3s² 3p¹
(iv)1s² 2s² 2p⁶ 3s² 3p⁴
(v)1s² 2s² 2p⁶ 3s² 3p⁵
The electron configuration belonging to the atom with the highest second ionization energy is ________.

A)(i)
B)(ii)
C)(iii)
D)(iv)
E)(v)

Question 28

Which ion below has the largest radius?

A)Cl^-
B)K⁺
C)Br^-
D)F^-
E)Na⁺

Question 29

Consider the following electron configurations to answer the questions that follow:
(i)1s² 2s² 2p⁶ 3s¹
(ii)1s² 2s² 2p⁶ 3s²
(iii)1s² 2s² 2p⁶ 3s² 3p¹
(iv)1s² 2s² 2p⁶ 3s² 3p⁴
(v)1s² 2s² 2p⁶ 3s² 3p⁵
The electron configuration of the atom that is expected to have a positive electron affinity is ________.

A)(i)
B)(ii)
C)(iii)
D)(iv)
E)(v)

Question 30

Consider the following electron configurations to answer the questions that follow:
(i)1s² 2s² 2p⁶ 3s¹
(ii)1s² 2s² 2p⁶ 3s²
(iii)1s² 2s² 2p⁶ 3s² 3p¹
(iv)1s² 2s² 2p⁶ 3s² 3p⁴
(v)1s² 2s² 2p⁶ 3s² 3p⁵
The electron configuration that belongs to the atom with the lowest second ionization energy is ________.

A)(i)
B)(ii)
C)(iii)
D)(iv)
E)(v)

Question 31

Consider the following electron configurations to answer the questions that follow:
(i)1s² 2s² 2p⁶ 3s¹
(ii)1s² 2s² 2p⁶ 3s²
(iii)1s² 2s² 2p⁶ 3s² 3p¹
(iv)1s² 2s² 2p⁶ 3s² 3p⁴
(v)1s² 2s² 2p⁶ 3s² 3p⁵
The electron configuration of the atom with the most negative electron affinity is ________.

A)(i)
B)(ii)
C)(iii)
D)(iv)
E)(v)

Question 32

Of the elements below, ________ has the highest melting point.

A)Ca
B)K
C)Fe
D)Na
E)Ba

Question 33

Consider the following electron configurations to answer the questions that follow:
(i)1s² 2s² 2p⁶ 3s¹
(ii)1s² 2s² 2p⁶ 3s²
(iii)1s² 2s² 2p⁶ 3s² 3p¹
(iv)1s² 2s² 2p⁶ 3s² 3p⁴
(v)1s² 2s² 2p⁶ 3s² 3p⁵
Of the following elements, ________ has the most negative electron affinity.

A)O
B)K
C)B
D)Na
E)S

Question 34

In the generation of most anions, the energy change (kJ/mol)that _______ an electron is ________.

A)removes, positive
B)adds, positive
C)removes, negative
D)adds, negative
E)None of the above is correct.

Question 35

Consider the following electron configurations to answer the questions that follow:
(i)1s² 2s² 2p⁶ 3s¹
(ii)1s² 2s² 2p⁶ 3s²
(iii)1s² 2s² 2p⁶ 3s² 3p¹
(iv)1s² 2s² 2p⁶ 3s² 3p⁴
(v)1s² 2s² 2p⁶ 3s² 3p⁵
Of the following elements, ________ has the most negative electron affinity.

A)S
B)Cl
C)Se
D)Br
E)I

Question 36

Of the following species, ________ has the largest radius.

A)Rb⁺
B)Sr²⁺
C)Br^-
D)Kr
E)Ar

Question 37

The list that correctly indicates the order of metallic character is ________.

A)Sr > Ca > Mg
B)F > Cl > Br
C)C > Ge > Si
D)Li > Na > K
E)O > Se > S

Question 38

Sodium is much more apt to exist as a cation than is chlorine. This is because ________.

A)chlorine is a gas and sodium is a solid
B)chlorine has a greater electron affinity than sodium does
C)chlorine is bigger than sodium
D)chlorine has a greater ionization energy than sodium does
E)chlorine is more metallic than sodium

Question 39

Of the elements below, ________ is the most metallic.

A)sodium
B)barium
C)magnesium
D)calcium
E)cesium

Question 40

Which of the following correctly represents the second ionization of copper?

A)Cu (g) → Cu⁺ (g) + e^-
B)Cu⁺ (g) → Cu²⁺ (g) + e^-
C)Cu^- (g) + e^- → Cu^2- (g)
D)Cu⁺ (g) + e^- → Cu²⁺ (g)
E)Cu⁺ (g) + e^- → Cu (g)

Question 41

Consider the following properties of an element: (i)It is solid at room temperature.
(ii)It easily forms an oxide when exposed to air.
(iii)When it reacts with water, hydrogen gas evolves.
(iv)It must be stored submerged in oil.
Which element fits the above description the best?

A)sulfur
B)copper
C)mercury
D)sodium
E)magnesium

Question 42

When two elements combine to form a compound, the greater the difference in metallic character between the two elements, the greater the likelihood that the compound will be ________.

A)a gas at room temperature
B)a solid at room temperature
C)metallic
D)nonmetallic
E)a liquid at room temperature

Question 43

Of the following oxides, ________ is the most acidic.

A)CaO
B)CO₂
C)Al₂O₃
D)Li₂O
E)Na₂O

Question 44

Consider the general valence electron configuration of ns²np⁵ and the following statements: (i)Elements with this electron configuration are expected to form -1 anions.
(ii)Elements with this electron configuration are expected to have large
Positive electron affinities.
(iii)Elements with this electron configuration are nonmetals.
(iv)Elements with this electron configuration form acidic oxides.
Which statements are true?

A)(i)and (ii)
B)(i), (ii), and (iii)
C)(ii)and (iii)
D)(i), (iii,)and (iv)
E)All statements are true.

Question 45

Which of the following generalizations cannot be made with regard to reactions of alkali metals? (The symbol M represents any one of the alkali metals.)

A)M (s) + O₂ (g) → MO₂ (s)
B)2M (s) + 2H₂O (l) → 2MOH (aq) + H₂ (g)
C)2M (s) + H₂ (g) → 2MH (s)
D)2M (s) + Cl₂ (g) → 2MCl (s)
E)2M (s) + S (s) → M₂S (s)

Question 46

Transition metals within a period differ mainly in the number of ________ electrons.

A)s
B)p
C)d
D)f
E)all of the above

Question 47

The reaction of alkali metals with oxygen produce ________.

A)oxides
B)peroxides
C)superoxides
D)all of the above
E)none of the above

Question 48

Alkaline earth metals ________.

A)have the smallest atomic radius in a given period
B)form monoanions
C)form basic oxides
D)exist as triatomic molecules
E)form halides with the formula MX

Question 49

This element is more reactive than lithium and magnesium but less reactive than potassium. This element is ________.

A)Na
B)Rb
C)Ca
D)Be
E)Fr

Question 50

Which of the following is not a characteristic of metals?

A)acidic oxides
B)low ionization energies
C)malleability
D)ductility
E)These are all characteristics of metals.

Question 51

Between which two elements is the difference in metallic character the greatest?

A)Rb and O
B)O and I
C)Rb and I
D)Li and O
E)Li and Rb

Question 52

Nonmetals can be ________ at room temperature.

A)solid, liquid, or gas
B)solid or liquid
C)solid only
D)liquid only
E)liquid or gas

Question 53

The oxide of which element below can react with hydrochloric acid?

A)sulfur
B)selenium
C)nitrogen
D)sodium
E)carbon

Question 54

Of the following metals, ________ exhibits multiple oxidation states.

A)Al
B)Rb
C)Mg
D)Ni
E)Cs

Question 55

The acidity of carbonated water is due to the ________.

A)presence of sulfur
B)reaction of CO₂ and H₂O
C)addition of acid
D)nonmetal oxides
E)none of the above

Question 56

Alkali metals tend to be more reactive than alkaline earth metals because ________.

A)alkali metals have lower densities
B)alkali metals have lower melting points
C)alkali metals have greater electron affinities
D)alkali metals have lower ionization energies
E)Alkali metals are not more reactive than alkaline earth metals.

Question 57

Which of the following traits characterizes the alkali metals?

A)very high melting point
B)existence as diatomic molecules
C)formation of dianions
D)the lowest first ionization energies in a period
E)the smallest atomic radius in a period

Question 58

The element in the periodic table that looks like a metal, is a poor thermal conductor, and acts as an electrical semiconductor is ________.

A)Sn
B)B
C)As
D)Si
E)Ge

Question 59

Which one of the following is not true about the alkali metals?

A)They are low density solids at room temperature.
B)They all readily form ions with a +1 charge.
C)They all have 2 electrons in their valence shells.
D)They are very reactive elements.
E)They have the lowest first ionization energies of the elements.

Question 60

Which one of the following compounds would produce an acidic solution when dissolved in water?

A)Na₂O
B)CaO
C)MgO
D)CO₂
E)SrO

Question 61

Which one of the following beverages originally contained lithium salts?

A)Coca-Cola®
B)Pepsi-Cola®
C)Gatorade®
D)Kool-Aid®
E)Seven-Up®

Question 62

Which element is solid at room temperature?

A)Cl₂
B)F₂
C)Br₂
D)I₂
E)H₂

Question 63

In nature, sulfur is most commonly found in ________.

A)pure elemental sulfur
B)sulfur oxides
C)metal sulfides
D)sulfuric acid
E)H₂S

Question 64

Which alkaline earth metal will not react with liquid water or with steam?

A)Be
B)Mg
C)Ca
D)Ba
E)They all react with liquid water and with steam.

Question 65

Xenon has been shown to form compounds only when it is combined with ________.

A)something with a tremendous ability to remove electrons from other substances
B)another noble gas
C)something with a tremendous ability to donate electrons to other substances
D)an alkali metal
E)an alkaline earth metal

Question 66

Which of the following statements is not true for oxygen?

A)The most stable allotrope of oxygen is O₂.
B)The chemical formula of ozone is O₃.
C)Dry air is about 79% oxygen.
D)Oxygen forms peroxide and superoxide anions.
E)Oxygen is a colorless gas at room temperature.

Question 67

In nature, the noble gases exist as ________.

A)monatomic gaseous atoms
B)the gaseous fluorides
C)solids in rocks and in minerals
D)alkali metal salts
E)the sulfides

Question 68

Ozone is a a(n)________ of oxygen.

A)isotope
B)allotrope
C)precursor
D)peroxide
E)free radical

Question 69

The alkali metal that is used to treat manic-depressive illness is ________.

A)Na
B)K
C)Li
D)Rb
E)Cs

Question 70

The noble gases were, until relatively recently, thought to be entirely unreactive. Experiments in the early 1960s showed that Xe could, in fact, form compounds with fluorine. The formation of compounds consisting of Xe is made possible by ________.

A)the availability of xenon atoms
B)xenon's noble gas electron configuration
C)the stability of xenon atoms
D)xenon's relatively low ionization energy
E)xenon's relatively low electron affinity

Question 71

Of the following elements, which have been shown to form compounds? helium neon argon krypton xenon

A)xenon and argon
B)xenon only
C)xenon, krypton, and argon
D)xenon and krypton
E)None of the above can form compounds.

Question 72

All of the halogens ________.

A)exist under ambient conditions as diatomic gases
B)tend to form positive ions of several different charges
C)tend to form negative ions of several different charges
D)exhibit metallic character
E)form salts with alkali metals with the formula MX

Question 73

________ is credited with developing the concept of atomic numbers.

A)Dmitri Mendeleev
B)Lothar Meyer
C)Henry Moseley
D)Ernest Rutherford
E)Michael Faraday

Question 74

Astatine has a(n)________ density and a(n)________ atomic radius compared to iodine.

A)greater; greater
B)smaller; greater
C)smaller; smaller
D)greater; smaller
E)equal; equal

Question 75

The alkali metal that is naturally radioactive is ________.

A)rubidium
B)cesium
C)lithium
D)francium
E)sodium

Question 76

Which one of the following elements has an allotrope that is produced in the upper atmosphere by lightning?

A)N
B)O
C)S
D)Cl
E)He

Question 77

________ is a unique element and does not truly belong to any family.

A)Nitrogen
B)Radium
C)Hydrogen
D)Uranium
E)Helium

Question 78

Hydrogen is unique among the elements because ________. 1. It is not really a member of any particular group.
2. Its electron is not at all shielded from its nucleus.
3. It is the lightest element.
4. It is the only element to exist at room temperature as a diatomic gas.
5. It exhibits some chemical properties similar to those of groups 1A and 7A.

A)1, 2, 3, 5
B)1, 2, 3, 4, 5
C)1, 4, 5
D)3, 4
E)2, 3, 4, 5

Question 79

Hydrogen is unique among the elements because ________. 1. It has only one valence electron.
2. It is the only element that can emit an atomic spectrum.
3. Its electron is not at all shielded from its nucleus.
4. It is the lightest element.
5. It is the only element to exist at room temperature as a diatomic gas.

A)1, 2, 3, 4, 5
B)1, 3, 4
C)1, 2, 3, 4
D)2, 3, 4
E)3, 4

Question 80

Elements in the modern version of the periodic table are arranged in order of increasing ________.

A)oxidation number
B)atomic mass
C)average atomic mass
D)atomic number
E)number of isotopes