Deck 8: Periodic Relationships Among the Elements

Question 1

Which of the following elements is found as a monatomic species in its most stable form

A) sulfur
B) oxygen
C) hydrogen
D) argon
E) phosphorus

Answer 1

argon

Question 2

Consider the element with the electron configuration [Kr]5s²4d⁷. This element is

A) a representative element.
B) a transition metal.
C) a nonmetal.
D) an actinide element.
E) a noble gas.

Answer 2

a transition metal.

Question 3

As opposed to early periodic tables based on the law of octaves, modern periodic tables arrange the elements in order of increasing

A) nuclear binding energy.
B) number of neutrons.
C) atomic mass.
D) atomic number.
E) atomic size.

Answer 3

atomic number.

Question 4

Which of the following elements is found as a diatomic species in its most stable form

A) bromine
B) neon
C) sulfur
D) xenon
E) phosphorus

Question 5

In what row and group of the periodic table would you find the element with the electron configuration [Kr]5s²4d¹⁰5p²

A) row 4, group 4A
B) row 4, group 5A
C) row 5, group 4A
D) row 5, group 5A
E) none of the above

Question 6

Which of the following is the general electron configuration for the outermost electrons of the halogens

A) ns²np⁶
B) ns²np⁵
C) ns²np⁶(n -1)d⁷
D) ns¹
E) ns²np⁷

Question 7

The elements in Group 7A are known by what name

A) transition metals
B) halogens
C) alkali metals
D) alkaline earth metals
E) noble gases

Question 8

Mendeleev proposed the existence of an unknown element that he called eka-aluminum. This element is now called

A) gallium.
B) silicon.
C) magnesium.
D) boron.
E) germanium.

Question 9

Which of the following is the general electron configuration for the outermost electrons of elements in the alkaline earth group

A) ns¹
B) ns²
C) ns²np⁴
D) ns²np⁵
E) ns²np⁶(n -1)d⁶

Question 10

The law of octaves states that every eighth element has similar properties when arranged in order of increasing

A) nuclear binding energy.
B) number of electrons.
C) number of neutrons.
D) atomic mass.
E) atomic number.

Question 11

Which of the following is the general electron configuration for the outermost electrons of the noble gases

A) ns²np⁶
B) ns²np⁵
C) ns²np⁴
D) ns²np³
E) ns²

Question 12

Which one of the following elements is a Lanthanide

A) U
B) Ce
C) Os
D) Bi
E) Cs

Question 13

The law of octaves was proposed by

A) G. N. Lewis.
B) John Newlands.
C) Dmitri Mendeleev.
D) J. J. Thompson.
E) Ernest Rutherford.

Question 14

The elements in Group 2A are known by what name

A) transition metals
B) halogens
C) alkali metals
D) alkaline earth metals
E) noble gases

Question 15

An element with the general electron configuration for its outermost electrons of ns²np¹ would be in which element group

A) 2A
B) 3A
C) 4A
D) 5A
E) 8A

Question 16

Which of the following elements is found as a monatomic species in its most stable form

A) nitrogen
B) neon
C) sulfur
D) chlorine
E) fluorine

Question 17

The chief contribution of physicist Henry Moseley to atomic theory was

A) the discovery of the periodic law.
B) the determination of the charge of the proton.
C) the measurement of the atomic numbers of the elements.
D) the scientist who determined the electric charge of the electron.
E) the discovery of the law of octaves.

Question 18

The alkali metal elements are found in _______ of the periodic table.

A) Group 1A
B) Group 2A
C) Group 3A
D) Period 7
E) Period 1

Question 19

Which of the following is the general electron configuration for the outermost electrons of the elements in Group 5A

A) ns²np⁶
B) ns²np⁵
C) ns²np⁴
D) ns²np³
E) ns²np¹

Question 20

Which one of the following elements is a transition element

A) antimony
B) barium
C) chromium
D) potassium
E) selenium

Question 21

Which of the following make an isoelectronic pair: Cl^-, O^2-, F, Ca²⁺, Fe³⁺

A) Ca²⁺ and Fe³⁺
B) O^2- and F
C) F and Cl^-
D) Cl^- and Ca²⁺
E) None of the above.

Question 22

Consider the element with the electron configuration [Kr]5s²4d¹⁰5p⁵. This element is

A) a representative element
B) a transition metal
C) an alkali metal
D) an actinide element
E) a noble gas

Question 23

The representative elements are those with unfilled energy levels in which the "last electron" was added to

A) an s orbital.
B) an s or p orbital.
C) a d orbital.
D) a p or d orbital.
E) an f orbital.

Question 24

How many core electrons does a silicon atom have

A) 14
B) 10
C) 4
D) 8
E) 2

Question 25

Which one of the following elements forms a stable 3- anion

A) P
B) S
C) Cl
D) Al
E) Mg

Question 26

Which one of the following elements forms a stable 1- anion

A) K
B) Be
C) Al
D) O
E) I

Question 27

How many electrons does a sulfur atom need to fill its outermost s and p subshells

A) 6
B) 8
C) 4
D) 2
E) 1

Question 28

How many electrons are in the 4p subshell of selenium

A) 0
B) 2
C) 4
D) 5
E) 6

Question 29

Which one of the following elements forms a stable 2+ cation

A) Kr
B) I
C) Se
D) Al
E) Ba

Question 30

How many electrons does a nitrogen atom need to fill its outermost s and p subshells

A) 5
B) 3
C) 1
D) 8
E) 0

Question 31

Concerning the electron configuration of sulfur, 1s²2s²2p⁶3s²3p⁴, which of the following represents the core electrons only

A) 1s²
B) 1s²2s²
C) 1s²2s²2p⁶
D) 1s²2s²2p⁶3s²
E) 3s²3p⁴

Question 32

Which two electron configurations represent elements that would have similar chemical properties
(1) 1s²2s²2p⁴ (2) 1s²2s²2p⁵ (3) [Ar]4s²3d⁵ (4) [Ar]4s²3d¹⁰4p⁵

A) (1) and (2)
B) (1) and (3)
C) (2) and (3)
D) (2) and (4)
E) (3) and (4)

Question 33

Concerning the electron configuration of fluorine, 1s²2s²2p⁵ which of the following represents the core electrons only

A) 1s²
B) 1s²2s²
C) 1s²2s²2p⁵
D) 2s²2p⁵
E) 2p⁵

Question 34

How many electrons does a bromine atom need to fill its outermost s and p subshells

A) 8
B) 7
C) 5
D) 3
E) 1

Question 35

How many core electrons does a chlorine atom have

A) 17
B) 7
C) 10
D) 18
E) 8

Question 36

How many electrons are in the 4p subshell of vanadium

A) 0
B) 2
C) 4
D) 5
E) 6

Question 37

Consider the element with the electron configuration [Xe]6s²4f⁷. This element is

A) a representative element
B) a lanthanide element
C) a nonmetal
D) an actinide element
E) a noble gas

Question 38

How many valence electrons does S^2- have

A) 2
B) 4
C) 6
D) 16
E) 8

Question 39

How many valence electrons does P^3- have

A) 3
B) 8
C) 15
D) 1
E) 18

Question 40

Concerning the electron configuration of aluminum, 1s²2s²2p⁶3s²3p¹, which of the following represents the valence electrons only

A) 1s²
B) 1s²2s²
C) 1s²2s²2p⁶
D) 1s²2s²2p⁶3s²
E) 3s²3p¹

Question 41

The effective nuclear charge (Z_eff) felt by the outermost electrons is the strongest for which of the following elements

A) B
B) C
C) N
D) O
E) F

Question 42

Which one of the following does not have [Kr] as its electronic configuration

A) Se^2-
B) Br^-
C) Rb⁺
D) Y³⁺
E) Zn²⁺

Question 43

The effective nuclear charge (Z_eff) felt by the outermost electrons is the strongest for which of the following elements

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

Question 44

Which of the following is the electron configuration for the bromide ion

A) [Ar]
B) [Ar]4s²3d¹⁰4p⁷
C) [Kr]
D) [Kr]5s²4d¹⁰5p⁷
E) [Xe]

Question 45

Which one of the following does not have [Xe] as its electronic configuration

A) Te^2-
B) I^-
C) Cs⁺
D) Ba²⁺
E) Sn⁴⁺

Question 46

How many 3d electrons does the manganese(II) ion, Mn²⁺, have

A) 3
B) 4
C) 5
D) 6
E) 7

Question 47

Which of the following is the electron configuration for the aluminum ion

A) 1s²2s²2p⁶3s²
B) 1s²2s²2p⁶3s²3p²
C) 1s²2s²2p⁶3s²3p¹
D) 1s²2s²2p⁶
E) 1s²2s²2p⁶3s²3p⁴

Question 48

Which of the following is the electron configuration of the iron(III) ion

A) [Ar]3d⁵
B) [Ar]4s¹3d⁵
C) [Ar]4s²3d³
D) [Ar]3d⁶
E) [Ar]4s²3d⁹

Question 49

How many 3d electrons does an Fe³⁺ ion have

A) 9
B) 6
C) 5
D) 4
E) 3

Question 50

The cobalt(III) ion, Co³⁺, has how many 3d electrons

A) 0
B) 7
C) 6
D) 5
E) 4

Question 51

Which of the atoms listed below has the smallest radius

A) Al
B) P
C) As
D) Te
E) Na

Question 52

Which of the following ground-state ions has unpaired electrons

A) P^3-
B) V⁵⁺
C) Mg²⁺
D) Sc²⁺
E) S²⁺

Question 53

Which one of the following is not isoelectronic with the others: Br^-, Rb⁺, Se^2-, Sr²⁺, Te^2-

A) Br^-
B) Rb⁺
C) Se^2-
D) Sr²⁺
E) Te^2-

Question 54

Which of the following ground-state ions has the largest number of unpaired electrons

A) Cr²⁺
B) Mn²⁺
C) Ni²⁺
D) Cu⁺
E) Co²⁺

Question 55

Which one of the following pairs are isoelectronic

A) Mn²⁺ and Ar
B) Zn²⁺ and Cu²⁺
C) Na⁺ and K⁺
D) Cl^- and S
E) K⁺ and Cl^-

Question 56

Which of the following is the electron configuration of a sulfide ion

A) [Ne]3s²3p⁴
B) [Ne]
C) [Ne]3s²3p¹
D) [Ar]
E) [Ne]3s²3p²

Question 57

The electron configuration of a copper(I) ion is

A) [Ar]4s²3d⁸.
B) [Ar]4s¹3d⁹.
C) [Ar]3d¹⁰.
D) [Ar]4s²3d⁶4p².
E) [Kr].

Question 58

Which ion is isoelectronic with Ar

A) Fe²⁺
B) F^-
C) Br^-
D) Ga³⁺
E) Ca²⁺

Question 59

Which one of the following is not isoelectronic with Kr

A) As³⁺
B) Se^2-
C) Rb⁺
D) Sr²⁺
E) Br^-

Question 60

The sulfide ion, S^2-, is isoelectronic with which one of the following

A) O^2-
B) F^-
C) Na⁺
D) Al³⁺
E) K⁺

Question 61

Arrange the following ions in order of increasing ionic radius: K⁺, P^3- , S^2-, Cl^- increasing radius $\rarr$

A) K⁺ < Cl^- < S^2- < P^3-
B) K⁺ < P^3- < S^2- < Cl^-
C) P^3- < S^2- < Cl^- < K⁺
D) Cl^- < S^2- < P^3- < K⁺
E) Cl^- < S^2- < K⁺ < P^3-

Question 62

Which element will display an unusually large jump in ionization energy values between I₃ and I₄, its third and fourth ionization energies

A) Na
B) Mg
C) Al
D) Si
E) P

Question 63

Which of the elements listed below has the smallest first ionization energy

A) C
B) Ge
C) P
D) O
E) Se

Question 64

Which of the following elements has the greatest electron affinity (largest positive value)

A) K
B) Br
C) As
D) Ar
E) I

Question 65

For which of the following reactions is the enthalpy change equal to the second ionization energy of nitrogen

A) N²⁺(g) $\rarr$ N³⁺(g) + e^-
B) N²⁺(g) + e^- $\rarr$ N⁺(g)
C) N(g) $\rarr$ N²⁺(g) + 2e^-
D) N^-(g) + e^- $\rarr$ N^2-(g)
E) N⁺(g) $\rarr$ N²⁺(g) + e^-

Question 66

For which of the following reactions is the enthalpy change equal to the third ionization energy of vanadium

A) V²⁺(g) $\rarr$ V³⁺(g) + e^-
B) V³⁺(g) + e^- $\rarr$ V²⁺(g)
C) V(g) $\rarr$ V³⁺(g) + 3e^-
D) V^2-(g) + e^- $\rarr$ V^3-(g)
E) V³⁺(g) $\rarr$ V⁴⁺(g) + e^-

Question 67

Which of the following elements has the smallest first ionization energy

A) Cl
B) Na
C) Be
D) K
E) As

Question 68

Which one of the following ions has the largest radius

A) Cl^-
B) K⁺
C) S^2-
D) Na⁺
E) O^2-

Question 69

Which of the elements listed below has the greatest atomic radius

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

Question 70

The successive ionization energies of a certain element are I₁= 589.5 kJ/mol, I₂ =1145 kJ/mol, I₃= 4900 kJ/mol, I₄ = 6500 kJ/mol, and I₅ = 8100 kJ/mol. This pattern of ionization energies suggests that the unknown element is

A) K
B) Si
C) As
D) Ca
E) S

Question 71

Which of the following elements has the greatest electron affinity (largest positive value)

A) Mg
B) Al
C) Si
D) P
E) S

Question 72

Arrange the following ions in order of decreasing ionic radius: Al³⁺, Mg²⁺, Na⁺, O^2-.decreasing radius $\rarr$

A) Al³⁺ > Mg²⁺ > O^2- > Na⁺
B) Al³⁺ > Mg²⁺ > Na⁺ > O^2-
C) Na⁺ > Mg²⁺ > Al³⁺ > O^2-
D) O^2- > Al³⁺ > Mg²⁺ > Na⁺
E) O^2- > Na⁺ > Mg²⁺ > Al³⁺

Question 73

Which of the following elements has the smallest ionization energy

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

Question 74

Which of the elements listed below has the highest first ionization energy

A) He
B) Ne
C) Ar
D) Kr
E) Xe

Question 75

Which of the elements listed below has the following pattern for its first six ionization energies (I₁ = first ionization energy, I₂ = second ionization energy, etc.)

A) Ca
B) Si
C) Al
D) Se
E) P

Question 76

For phosphorus atoms, which ionization energy will show an exceptionally large increase over the previous ionization energy

A) 2nd
B) 3rd
C) 4th
D) 5th
E) 6th

Question 77

The successive ionization energies of a certain element are I₁= 577.9 kJ/mol, I₂ = 1820 kJ/mol, I₃= 2750 kJ/mol, I₄ = 11,600 kJ/mol, and I₅ = 14,800 kJ/mol. This pattern of ionization energies suggests that the unknown element is

A) K
B) Al
C) Cl
D) Se
E) Kr

Question 78

Which of the atoms listed below has the largest radius

A) Cl
B) I
C) P
D) Sb
E) Se

Question 79

For silicon atoms, which ionization energy will show an exceptionally large increase over the preceding ionization energy

A) 2nd
B) 3rd
C) 4th
D) 5th
E) 6th

Question 80

Which of the elements listed below has the highest first ionization energy

A) C
B) Ge
C) P
D) O
E) Se