Deck 7: Electron Configuration and the Periodic Table

Question 1

Who found that the atomic number was equal to the number of protons in the nucleus and to the number of electrons outside the nucleus in a neutral atom?

A)Meyer
B)Newlands
C)Moseley
D)Mendeleev
E)Thomson

Answer 1

Moseley

Question 2

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 determination of the electric charge of the electron.
E)the discovery of the law of octaves.

Answer 2

the measurement of the atomic numbers of the elements.

Question 3

Which element would be expected to have properties similar to argon?

A)F
B)Cl
C)H
D)Br
E)Kr

Answer 3

Kr

Question 4

Which of these elements exhibits chemical behavior similar to that of potassium?

A)magnesium
B)sodium
C)sulfur
D)chlorine
E)iron

Question 5

Which of these elements exhibits chemical behavior similar to that of oxygen?

A)magnesium
B)sodium
C)sulfur
D)chlorine
E)iron

Question 6

Which element would be expected to have properties similar to calcium?

A)Ba
B)K
C)Sc
D)Na
E)Rb

Question 7

What is the electron configuration for Fr?

A)[Xe]6s¹
B)[Rn]7s¹
C)[Rn]7s²
D)[Xe]6s²
E)[Kr]6s¹

Question 8

In 1864,the English chemist John Newlands noticed that when the elements were arranged in order of increasing atomic mass,every eighth element had similar properties.Newlands referred to this relationship as the

A)law of periodicity.
B)law of loopholes.
C)law of octaves.
D)law of orbitals.
E)law of proportionality.

Question 9

Which of these choices is the general electron configuration for the outermost electrons of elements in the alkaline earth group?

A)ns¹
B)ns²
C)ns²np⁴
D)ns²np
E)ns²np⁶ (n - 1)d⁶

Question 10

Which two electron configurations represent elements that would have similar chemical properties? (1) 1s²2s²2p⁴,(2)1s²2s²2p⁵,(3)[Ar]4s²3d¹⁰4p³,(4)[Ar]4s²3d¹⁰4p⁴

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

Question 11

Which one of these elements is a transition element?

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

Question 12

Which of these elements exhibits chemical behavior similar to that of silver?

A)nickel
B)gold
C)sulfur
D)chlorine
E)iron

Question 13

In what groups are transition metals located?

A)1A,7A,and 1B
B)2A,4A,and 7A
C)1B through 8B
D)2B and 3B through 6B
E)3A through 6A

Question 14

What elements and groups have properties that are most similar to those of chlorine?

A)F,Br,I,and nonmetals in Group 7A
B)Cl,K,C,and metals in Group 1B
C)N,P,As,and lanthanides
D)He,Ne,Xe,and nonmetals in Group 7A
E)O,S,and P

Question 15

Which one of these elements is a transition element?

A)Nickel
B)Tin
C)Sodium
D)Sulfur
E)Calcium

Question 16

The nineteenth century chemists arranged elements in the periodic table according to increasing

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

Question 17

Who noticed that the periodic table was arranged in order of atomic mass,where every eighth element had similar properties,and called this the law of octaves?

A)Meyer
B)Newlands
C)Moseley
D)Mendeleev
E)Thomson

Question 18

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 19

Which element would be expected to have properties similar to antimony?

A)Se
B)Sn
C)P
D)As
E)Pb

Question 20

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

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

Question 21

Each of the noble gases has a completely filled p subshell except for which one?

A)Xenon
B)Neon
C)Radon
D)Argon
E)Helium

Question 22

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

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

Question 23

The effective nuclear charge for an atom is less than the actual nuclear charge due to

A)shielding.
B)penetration.
C)paramagnetism.
D)electron-pair repulsion.
E)relativity.

Question 24

In what group of the periodic table is the element with the electron configuration [Ar]4s²3d¹⁰4p³?

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

Question 25

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

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

Question 26

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

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

Question 27

How many valence electrons does a carbon atom have?

A)1
B)2
C)3
D)4
E)6

Question 28

Which one of these ions has the smallest radius?

A)Cl^-
B)K⁺
C)S2^-
D)Na⁺
E)O2^-

Question 29

The energy states of atoms containing more than one electron arise from nucleus-electron and electronelectron interactions.Which of the following statements correctly describes these effects?

A)Larger nuclear charge lowers energy; more electrons in an orbital lowers energy.
B)Larger nuclear charge lowers energy; more electrons in an orbital increases energy.
C)Smaller nuclear charge lowers energy; more electrons in an orbital lowers energy.
D)Smaller nuclear charge lowers energy; more electrons in an orbital increases energy.
E)None of these statements is generally correct.

Question 30

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

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

Question 31

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 32

Which of these atoms has the smallest radius?

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

Question 33

An element with the electron configuration [noble gas]ns²(n - 1)d⁸ has ___________ valence electrons.

A)2
B)6
C)8
D)10
E)None of these choices is correct.

Question 34

An element with the electron configuration [noble gas]ns²(n - 1)d¹⁰np³ has ____________ valence electrons.

A)2
B)3
C)5
D)10
E)15

Question 35

Arrange P,S,and O in order of increasing atomic radius.

A)S < O < P
B)P < S < O
C)O < S < P
D)O < P < S
E)The answer cannot be determined from the data given.

Question 36

Which of these atoms has the largest radius?

A)B
B)Ga
C)Br
D)Si
E)Cl

Question 37

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

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

Question 38

The general electron configuration for noble gas atoms is

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

Question 39

How does atomic radius change as you move across the periodic table?

A)Atomic radius decreases moving from left to right across a period and increases from top to bottom.
B)Atomic radius increases moving left to right across a period and decreases from top to bottom.
C)Smaller nuclear charge lowers energy; more electrons in an orbital lowers energy.
D)Atomic radius increases diagonally across the periodic table.
E)None of the answers is correct.

Question 40

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 41

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

A)Na
B)Cl
C)Ca
D)Te
E)Br

Question 42

What is the correct characteristic of nonmetals?

A)They have low electron affinities (so they commonly form anions).
B)They have low ionization energies (so they commonly form cations).
C)They form ionic compounds with chlorine (metal chlorides).
D)They form basic,ionic compounds with oxygen (metal oxides).
E)They have high electron affinities (so they commonly form anions).

Question 43

Which of these elements has the greatest electron affinity?

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

Question 44

Which one of the following equations correctly represents the process involved in the electron affinity of X?

A)X(g)→ X⁺(g)+ e^-
B)X⁺(g)→ X⁺(aq)
C)X⁺(g)+ e^- → X(g)
D)X(g)+ e^- → X^-(g)
E)X⁺(g)+ Y^-(g)→ XY(s)

Question 45

Which of the following elements has the largest third ionization energy (IE₃)?

A)Li
B)B
C)Ne
D)Be
E)Al

Question 46

Which of these elements has the highest first ionization energy?

A)Cs
B)Ga
C)K
D)Bi
E)As

Question 47

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

A)Rb
B)Mg
C)I
D)As
E)F

Question 48

The first ionization energies of noble gases are _______________.

A)very positive
B)slightly negative
C)slightly positive
D)very negative
E)zero

Question 49

Which of the following elements has the smallest atomic size?

A)Na
B)Ar
C)K
D)Ca
E)Kr

Question 50

Select the element with the most negative electron affinity (i.e.,accepts an electron most readily).

A)H
B)Li
C)C
D)F
E)Ne

Question 51

Which of these elements has the smallest first ionization energy?

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

Question 52

Which of the following elements has the largest second ionization energy (IE₂)?

A)Li
B)B
C)O
D)F
E)Na

Question 53

Which of the following elements has the largest atomic size?

A)S
B)Ca
C)Ba
D)Po
E)Rn

Question 54

Elements with ________________ first ionization energies and ___________ electron affinities generally form cations.

A)low,very negative
B)high,positive or slightly negative
C)low,positive or slightly negative
D)high,very negative
E)None of these is generally correct.

Question 55

Elements with _______________ first ionization energies and ___________ electron affinities generally form anions.

A)low,very positive
B)high,positive or slightly negative
C)low,positive or slightly negative
D)high,very positive
E)None of these is generally correct.

Question 56

Elements with the highest first ionization energies are found in the ___________ region of the periodic table.

A)lower left
B)upper left
C)center
D)lower right
E)upper right

Question 57

Arrange these ions in order of increasing ionic radius: K⁺ ,P^3- ,S^2- ,Cl^-.

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

Question 58

The electron affinity of oxygen is equal to

A)the ionization energy of O^-.
B)the ionization energy of O^2-.
C)the second ionization energy of O.
D)twice the electron affinity of O⁺.
E)none of these.

Question 59

Which of these atoms has the greatest electron affinity?

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

Question 60

Which one of the following equations correctly represents the process relating to the ionization energy of X?

A)X(s)→ X⁺(g)+ e^-
B)X2(g)→ X⁺(g)+ X^-(g)
C)X(g)+ e^- → X^-(g)
D)X^-(g)→ X(g)+ e^-
E)X(g)→ X⁺(g)+ e-

Question 61

An oxide ion,O^2-,has

A)8 protons and 10 electrons.
B)10 protons and 8 electrons.
C)8 protons and 9 electrons.
D)8 protons and 7 electrons.
E)10 protons and 7 electrons.

Question 62

Which of these elements has the greatest metallic character?

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

Question 63

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 64

Consider the set of isoelectronic atoms and ions A^2-,B^-,C,D⁺,and E²⁺.Which arrangement of relative radii is correct?

A)A^2- > B^- > C > D⁺ > E²⁺
B)E²⁺ > D⁺ > C > B^- > A^2-
C)A^2- > B^- > C < D⁺ < E²⁺
D)A^2- < B^- < C > D⁺ > E²⁺
E)None of these relative radii statements is correct.

Question 65

Select the element with the greatest metallic character.

A)Li
B)Ca
C)Al
D)Pb
E)Cs

Question 66

Which of these choices is the electron configuration for the aluminum ion?

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

Question 67

Which ground-state ion does not have an electron configuration described by the following orbital diagram? [Ar]
↿
↿
↿
↿
4s
3d
4s 3d

A)V⁺
B)Cr²⁺
C)Mn³⁺
D)Co⁵⁺
E)Fe⁴⁺

Question 68

Which of these elements has the greatest metallic character?

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

Question 69

Which of these pairs consists of isoelectronic species?

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

Question 70

A sulfide ion,S^2-,has

A)16 protons and 16 electrons.
B)32 protons and 16 electrons.
C)16 protons and 14 electrons.
D)16 protons and 18 electrons.
E)32 protons and 18 electrons.

Question 71

An isoelectronic series is

A)a series that has two or more species that have identical nuclear charges,but have different electron configurations.
B)a series that has the same ionization potentials.
C)a series that can have only up to three species and have similar electron configuration and similar nuclear charges.
D)a series that has two or more species that have identical electron configurations,but different nuclear charges.
E)a series that has the same nuclear charge.

Question 72

The elements in a column of the periodic table are known as

A)metalloids.
B)a period.
C)noble gases.
D)a group.
E)nonmetals.

Question 73

Which one of these ions is not isoelectronic with Kr?

A)As³⁺
B)Se^2-
C)Rb⁺
D)Sr²⁺
E)Br^-

Question 74

How many protons and electrons are present in one Br^- ion?

A)35 protons,35 electrons
B)80 protons,81 electrons
C)35 protons,34 electrons
D)35 protons,36 electrons
E)80 protons,34 electrons

Question 75

A magnesium ion,Mg²⁺,has

A)12 protons and 13 electrons.
B)24 protons and 26 electrons.
C)12 protons and 10 electrons.
D)24 protons and 22 electrons.
E)12 protons and 14 electrons.

Question 76

Which ion is isoelectronic with Ar?

A)Fe²⁺
B)F^-
C)Br^-
D)Ga³⁺
E)Ca²⁺

Question 77

Which of these species 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 species are part of an isoelectronic series.

Question 78

Which one of these ions does not have [Xe] as its electronic configuration?

A)Te^2-
B)I^-
C)Cs⁺
D)Ba²⁺
E)Sn⁴⁺

Question 79

An aluminum ion,Al³⁺,has

A)13 protons and 13 electrons.
B)27 protons and 24 electrons.
C)16 protons and 13 electrons.
D)13 protons and 10 electrons.
E)10 protons and 13 electrons.

Question 80

Select the element with the least metallic character.

A)Sn
B)Sr
C)Tl
D)Ge
E)Ga