Deck 8: Periodic Relationships Among the Elements

Question 1

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.

Answer 1

gallium.

Question 2

The law of octaves was proposed by

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

Answer 2

John Newlands.

Question 3

Which one of the following elements is a transition element?

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

Answer 3

chromium

Question 4

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.

Question 5

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 6

The general electron configuration for atoms of all elements in Group 5A is

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

Question 7

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 8

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.

Question 9

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 10

The general electron configuration for noble gas atoms is

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

Question 11

The general electron configuration for atoms of the halogen group is

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

Question 12

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 13

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 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

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 17

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 18

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 19

Which one of the following elements is a transition element?

A)Sr
B)Pb
C)As
D)Fe
E)H

Question 20

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 21

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 22

How many valence electrons does a tin (Sn)atom have?

A)2
B)4
C)14
D)36
E)50

Question 23

How many electrons are in the 4p orbitals of selenium?

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

Question 24

How many valence electrons does an oxygen atom have?

A)2
B)4
C)6
D)7
E)8

Question 25

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

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

Question 26

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 27

What is the charge on the monatomic ion of nitrogen, the nitride ion?

A)+2
B)+1
C)-1
D)-2
E)-3

Question 28

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 29

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

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

Question 30

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 31

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 32

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 33

Which ion is isoelectronic with Ar?

A)Fe²⁺
B)F^-
C)Br^-
D)Ga³⁺
E)Ca²⁺

Question 34

The electron configuration of a copper(I)ion is

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

Question 35

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 36

What is the charge on the monatomic ion that calcium forms in its compounds?

A)+2
B)+1
C)-1
D)-2
E)-3

Question 37

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 38

Which one of the following is not isoelectronic with Kr?

A)As³⁺
B)Se^2-
C)Rb⁺
D)Sr²⁺
E)Br^-

Question 39

What is the charge on the stable ion formed by selenium?

A)+2
B)+1
C)-1
D)-2
E)-3

Question 40

How many electrons are in the 4p orbitals of vanadium?

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

Question 41

Which of the atoms listed below has the largest radius?

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

Question 42

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

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

Question 43

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 44

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 45

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 46

Which of the following ground-state ions has unpaired electrons?

A)P^3-
B)V⁵⁺
C)Mg²⁺
D)Sc²⁺
E)S²⁺

Question 47

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 48

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 49

Which one of the following ions has the largest radius?

A)Cl^-
B)K⁺
C)S^2-
D)Na⁺
E)O^2-

Question 50

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 51

Which of the following elements has the smallest ionization energy?

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

Question 52

Which of the following elements has the smallest first ionization energy?

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

Question 53

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

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

Question 54

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

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

Question 55

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

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

Question 56

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

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

Question 57

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 58

Which of the elements listed below has the greatest atomic radius?

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

Question 59

How many 3d electrons does an Fe³⁺ ion have?

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

Question 60

Which of the atoms listed below has the smallest radius?

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

Question 61

The electron affinity of fluorine is essentially equal to

A)the negative of the ionization energy F.
B)the ionization energy F^-.
C)the negative of the ionization energy F^-.
D)the ionization energy Ne.
E)the negative of the ionization energy Ne.

Question 62

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 63

Which of the following elements has the greatest metallic character?

A)Ca
B)Mg
C)Ba
D)As
E)Se

Question 64

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 65

Which of the following elements has the greatest metallic character?

A)Br
B)F
C)Ge
D)Mn
E)Sc

Question 66

Which of the following elements has the greatest metallic character?

A)Br
B)Se
C)Ni
D)As
E)Si

Question 67

The first ionization energy of mercury is 1006 kJ/mol. The energy change for the reaction Hg(l) $\rarr$ Hg⁺(g)+ e^- is therefore

A)1006 kJ/mol.
B)greater than 1006 kJ/mol.
C)less than 1006 kJ/mol.
D)is equal to the electron affinity of mercury.
E)is equal to the second ionization energy of mercury.

Question 68

If the radius of atom X is greater than the radius of atom Y, then it is also likely that

A)X has a larger electron affinity than Y does.
B)X has a larger effective nuclear charge than Y does.
C)X has greater metallic character than Y does.
D)X has a larger first ionization energy than Y does.
E)X is a poorer conductor of electricity than Y when in the solid state.

Question 69

Which of the following is a basic oxide?

A)CO₂
B)CaO
C)SO₂
D)H₂O
E)NO₂

Question 70

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

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

Question 71

Which of the following is an amphoteric oxide?

A)Na₂O
B)MgO
C)Al₂O₃
D)SO₂
E)Cl₂O₇

Question 72

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

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

Question 73

The first ionization energy of sodium is 495.9 kJ/mol. The energy change for the reaction Na(s) $\rarr$ Na⁺(g)+ e^- is therefore

A)495.9 kJ/mol.
B)less than 495.9 kJ/mol.
C)greater than 495.9 kJ/mol.
D)is equal to the electron affinity of sodium.
E)is equal to the second ionization energy of sodium.

Question 74

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 75

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 76

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 77

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

A)S
B)P
C)Ga
D)Li
E)Br

Question 78

In a surprisingly large number of their properties, beryllium resembles aluminum and boron resembles silicon. Such a relationship is called

A)amphoterism.
B)an allotropic relationship.
C)a diagonal relationship.
D)the periodic law.
E)an isoelectronic series.

Question 79

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 80

Which pair of elements from different groups resemble each other the most in their chemical properties?

A)Be and B
B)Al and Si
C)Li and Be
D)Al and Be
E)Be and C