Deck 9: The Periodic Table and Some Atomic Properties

Question 1

Which of the following pairs of elements are classified as metalloids?

A)aluminum and silicon
B)argon and neon
C)arsenic and germanium
D)bromine and sulfur
E)copper and silver

Answer 1

arsenic and germanium

Question 2

Why was Moseley so sure from his X-ray work that there were no other undiscovered elements besides the three that he predicted in the range of atomic numbers 13-79?

A)The rows on the periodic table were filled.
B)The columns of the periodic table were full.
C)All of the possible atomic weights were assigned.
D)All of the integer atomic numbers were assigned.
E)Mendeleev didn't predict any more.

Answer 2

All of the integer atomic numbers were assigned.

Question 3

Ions always adopt the electron configuration of a noble gas.

Answer 3

False

Question 4

Paramagnetic is not the same as magnetic.

Question 5

Most transition elements form monatomic ions that are not:

A)isoelectronic with any other cations
B)isoelectronic with any noble gas
C)isoelectronic with any neutral atom
D)isoelectronic with any other species
E)isoelectronic with any other transition metal ion

Question 6

An atom with an even number of electrons is always diamagnetic.

Question 7

The ion represented as Ti⁴⁺ has:

A)22 electrons
B)48 neutrons
C)26 protons
D)4 3d electrons
E)0 4s electrons

Question 8

Elements in the first two groups are part of the main-group elements along with which of the following groups?

A)d-block elements
B)s-block elements
C)actinides
D)lanthanides
E)p-block elements

Question 9

The electron affinity is opposite to the ionization energy.

Question 10

The inner transition elements include the actinides and the lanthanides.

Question 11

The ionization energy is the energy required for a gaseous atom to lose an electron.

Question 12

The similar chemical behavior of the elements in a given group in the periodic table is best accounted for by the fact that atoms of these elements have:

A)the same number of isotopes
B)the same number of electrons
C)the same number of electrons in the outermost (valence)shell
D)similar nuclear structures
E)the same number of protons

Question 13

Plutonium is among a group of elements referred to as:

A)actinides
B)alkalides
C)chalcocides
D)halides
E)lanthanides

Question 14

The electron affinity is the energy for an atom in its standard state to gain an electron.

Question 15

The actinides refer to what group of elements?

A)s-block elements
B)d-block elements
C)f-block elements of atomic number 58 through 71
D)f-block elements of atomic number 90 through 103
E)p-block elements

Question 16

The covalent radius,metallic radius,and the ionic radius are all equal.

Question 17

Moseley used X-rays to determine the atomic mass of each element.

Question 18

Which of the following could never be isoelectronic species?

A)anions of two different elements
B)cations of two different elements
C)an anion and a cation
D)an anion and an atom
E)atoms of two different elements

Question 19

Polarizability decreases with the size of the atom.

Question 20

The transition elements refer to what group of elements?

A)s-block elements
B)d-block elements
C)actinides
D)lanthanides
E)p-block elements

Question 21

Which of the following statements is INCORRECT?

A)The atomic radius decreases from left to right through a period of elements.
B)Cations are larger than the atoms from which they are formed.
C)The metallic character of elements decreases from left to right through a period of elements.
D)The ionization energy increases from left to right through a period of elements.
E)The atomic radius increases down the periodic table.

Question 22

Which of the following has the largest radius?

A)As^3-
B)Br
C)Sr²⁺
D)Cl^-
E)Se^2-

Question 23

Among the alkali metals,cesium reacts more rapidly than sodium because:

A)cesium has more electrons
B)cesium has more neutrons
C)the valence electron of cesium is at a greater average distance from the nucleus
D)cesium has a higher atomic weight
E)cesium has more protons

Question 24

The first ionization energy for rubidium is +403.0 kJ/mol.How much energy would be required to convert 17.1 g of gaseous rubidium to its gaseous +1 monatomic ion at constant temperature?

A)185 kJ
B)80.6 kJ
C)68.9 kJ
D)40.4 kJ
E)34.5 kJ

Question 25

What is the ground state electron configuration for iron(III)?

A)[Ar]3d⁵
B)[Ar]4s²3d³
C)[Ar]4s¹3d⁴
D)[Ar]4s²4p³
E)[Ar]4p⁵

Question 26

Which of the following has the smallest radius?

A)Yb³⁺
B)Ho³⁺
C)Nd³⁺
D)Gd³⁺
E)Ce³⁺

Question 27

Choose the INCORRECT statement.

A)Within a given subshell,each orbital is usually occupied by a single electron before any orbital has two electrons.
B)When a metallic element unites with a nonmetallic element,electrons are lost by atoms of the metal and gained by atoms of the nonmetals.
C)The noble gas atoms complete the filling of the p orbitals.
D)The ionization energy of Ca⁺ is greater than that for Ca²⁺.
E)The radius of Ba²⁺ is smaller than the radius of Ba⁺.

Question 28

Which comparison of atomic and/or ionic radii is correct?

A)K⁺ > K
B)K⁺ > Ca²⁺
C)S > Si
D)Kr > Xe
E)Cl > Cl^-

Question 29

Which ground state electronic configuration will most readily produce an ion with a charge of 2+?

A)1s²2s²2p⁶3s²3p⁶3d¹⁰4s²
B)1s²2s²2p⁶3s²3p⁶4s¹
C)1s²2s²2p⁶3s²3p⁴
D)1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p²
E)1s^2s22p⁶3s²3p⁶3d¹⁰4s²4p⁶

Question 30

Which series of elements shows the smallest difference in atomic radii?

A)Li......F
B)Be......Ra
C)He......Xe
D)C......Pb
E)Sc......Zn

Question 31

What is the general valence electronic configuration (where n = principal quantum number)that best describes the halogens as a group?

A)ns^1np6
B)ns^2np4
C)ns^2np5
D)ns^2np6
E)ns^2np3

Question 32

Choose the species from which one electron could most easily be removed.

A)Cl
B)K⁺
C)K
D)Ca⁺
E)Ar

Question 33

Which of the following isoelectronic species has the largest radius?

A)Ne
B)F^-
C)Mg²⁺
D)Na⁺
E)O^2-

Question 34

Which of the following has the largest radius?

A)Se^2-
B)Kr
C)Rb⁺
D)Br^-
E)Y³⁺

Question 35

Which of the following occurs for the representative elements going left to right across the period?

A)Electronegativity decreases.
B)Atomic size increases.
C)Forces of attraction between electron and nucleus increase because the effective nuclear charge increases.
D)The outer electrons are held more weakly.
E)none of these

Question 36

A is the sequence Na,Mg,Al,Si,and P.B is the sequence He,Ne,Ar,Kr,and Xe.Which statement below is true?

A)The members of A are decreasing in size.
B)The members of B have larger radii than those of A,respectively.That is He > Na,Ne > Mg,etc.
C)The members of A have larger radii than those of B,respectively.
D)The members of B are decreasing in size.
E)All the members of A are isoelectronic.

Question 37

The effective nuclear charge for sodium is:

A)+10
B)+9
C)+1
D)+11
E)0

Question 38

Which of the following has the largest atomic radius?

A)Rb
B)Br
C)Mo
D)I

Question 39

Which of the following has the largest radius?

A)Cl^-
B)Ar
C)Sc³⁺
D)K⁺
E)P^3-

Question 40

Which statement best describes relationships in a modern periodic table?

A)Each transition element is placed in the column of the main group element that it most closely resembles.
B)The fourteen elements in the "lanthanide" series form a new independent period.
C)Metalloids usually are the cations in ionic compounds.
D)Nonmetallic properties tend to predominate for elements at the far right portion of the table.
E)Elements are always arranged in order of increasing atomic weights.

Question 41

Which of the following has the greatest number of unpaired electrons?

A)Cr²⁺
B)Ti³⁺
C)Co²⁺
D)Ni

Question 42

Which species is diamagnetic?

A)atomic sodium
B)atomic fluorine
C)iron(III)ion
D)calcium(II)ion
E)cobalt(II)ion

Question 43

Which of the following has the smallest second ionization energy?

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

Question 44

List in order of increasing charge of the most common ion:
S,Na,F,Ca,Al

A)S^2-,Na^-,F⁺,Ca²⁺,Al³⁺
B)Ca^2-,F^-,Al⁺,Na²⁺,S³⁺
C)F^2-,S^-,Ca⁺,Al²⁺,Na³⁺
D)S^2-,F^-,Na⁺,Ca²⁺,Al³⁺
E)Al^2-,Ca^-,F⁺,Na²⁺,S³⁺

Question 45

The number of valence electrons for atomic potassium is ________.

A)1
B)5
C)6
D)15
E)19

Question 46

List in order of increasing size: Cl^-,Ar,K⁺,S^2-,Ca^2+.

A)Ca²⁺ < K⁺ < Ar < Cl^- < S^2-
B)S^2- < Cl^- < Ar < K⁺ < Ca²⁺
C)Ca²⁺ < S^2- < K⁺ < Ar < Cl^-
D)Cl^- < Ar < K⁺ < S^2- < Ca²⁺
E)K⁺ < S^2- < Ar < Cl^- < Ca²⁺

Question 47

If the formula of an oxide is X₂O₃,what is the formula of the chloride of X?

A)XCl
B)X₃Cl
C)XCl₃
D)XCl₆
E)X₂Cl₃

Question 48

Why is the electron affinity slightly positive for some of the group 2 elements?

A)The added electron would have to go into a new shell.
B)The added electron would have to be added into the half-filled p subshell.
C)The added electron would have to be added into the p subshell.
D)The groups 2 elements are diatomic elements.
E)Electrons can't be added to metals.

Question 49

Which of the following species is most likely to be diamagnetic?

A)Fe
B)I
C)Mn⁺
D)W³⁺
E)Zn²⁺

Question 50

Which of the following reactions gives a positive value for the electron affinity?

A)S^-(g)+ e^- → S^2-(g)
B)O(g)+ e^- → O^-(g)
C)S(g)+ e^- → S^-(g)
D)Br(g)+ e^- → Br^-(g)

Question 51

List in order of increasing atomic size: F,Na,K,Mg,Ne.

A)K < Mg < Ne < Na < F
B)Ne < Mg < K < Na < F
C)Ne < F < Mg < Na < K
D)Mg < F < Ne < Na < K
E)K < Na < Mg < F < Ne

Question 52

Which of the following species is diamagnetic?

A)F^-
B)C
C)Al
D)S^-
E)Na

Question 53

What is the relationship between ionization energy and atomic radii?

A)Energy increases as radii increase.
B)Energy is negative for all large radii.
C)Energy decreases as radii decrease.
D)Energy decreases as radii increase
E)Energy increases as radii decrease

Question 54

The first ionization potential for S is lower than the first ionization potential for P because:

A)Hund's rule is violated
B)P has a p³ configuration
C)ionization potentials decrease across a representative period
D)P is to the right of S on the periodic table
E)P is below S on the periodic table

Question 55

Can alkali metal atoms form negative ions in the gaseous state? Explain.

A)No,an electron cannot be added.
B)No,only a liquid can be ionized.
C)Yes,an electron can be added to a Li half-filled 2s orbital.
D)Yes,an electron can be removed from a Li half-filled 2s orbital.
E)No,the 2s orbital is completely filled.

Question 56

Which of the following atoms has the smallest atomic radius: Br,K,Fe,Cu,Bi?

A)Br
B)K
C)Fe
D)Cu
E)Bi

Question 57

Which comparison of ionization energies is correct?

A)Cs > Na
B)Na > Mg
C)Ca > Mg
D)Ca⁺ > Ca
E)Ar > He

Question 58

Why is the electron affinity so positive for the noble gas elements?

A)The added electron would have to go into a new shell.
B)The added electron would have to be added into the half-filled p subshell.
C)The added electron would have to be added into the p subshell.
D)The noble gas elements are diatomic elements.
E)Electrons can't be added to gases.

Question 59

Which of the following elements is likely to have the largest second ionization energy?

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

Question 60

What is the general relationship between electron affinity and atomic radii for neutral atoms in their ground electronic states?

A)Electron affinity becomes more negative as radii increases.
B)Electron affinity becomes more negative as radii decreases.
C)Electron affinity becomes positive as radii decreases.
D)Electron affinity becomes positive as radii increases.
E)The two quantities are unrelated.

Question 61

List in order of increasing ionization energy: Na,K,F,Mg,Ne.

A)Na < K < F < Ne < Mg
B)K < Na < Mg < F < Ne
C)Ne < Mg < F < K < Na
D)F < Mg < Ne < K < Na
E)Ne < Na < Mg < F < K

Question 62

List in order of increasing ionization potential: O,Mg,Rb,S,Si.

A)Si < O < Mg < Rb < S
B)Si < S < Rb < Mg < O
C)Mg < O < Rb < S < Si
D)Rb < Mg < Si < S < O
E)S < Si < Mg < O < Rb

Question 63

Which of the following has the smallest value of the first ionization energy: Ar,Cs,N,Cu,Rb?

A)Ar
B)Cs
C)N
D)Cu
E)Rb

Question 64

Arrange the following in order of increasing ionization energy: Li,Cs,K.

A)K < Li < Cs
B)Cs < K < Li
C)Li < Cs < K
D)Cs < Li < K
E)K < Cs < Li

Question 65

List in order of more negative electron affinity: F,Br,Sb,Rb,Se.
(more positive → more negative)

A)Br < Se < Sb < Rb < F
B)Se < Rb < Sb < Br < F
C)Sb < Br < Rb < Se < F
D)Br < F < Rb < Sb < Se
E)Rb < Sb < Se < Br < F

Question 66

How much energy,in joules,must be absorbed to convert all the atoms present in 1.00 mg of gaseous Na into Na⁺? The first ionization energy of Na is 495.8 kJ/mol.

A)21.6 J
B)0.0464 J
C)46.4 J
D)0.0216 J
E)1.14 × 10⁴ J

Question 67

Which main group atom or ion should be included in the following list?
Br^-,Se^2-,Kr,Sr²⁺

A)As^3-
B)Ar
C)K⁺
D)S^2-

Question 68

Which 1+ ion is isoelectronic with S^2-?

Question 69

List in order of increasing atomic size: Sr,Se,Cs,Ga,In.

A)Se < Ga < In < Sr < Cs
B)Ga < In < Se < Cs < Sr
C)Sr < In < Ga < Se < Cs
D)In < Ga < Cs < Se < Sr
E)Cs < Ga < Se < Sr < In

Question 70

The energy difference between atomic cesium and its most stable ion,in the gaseous state,is referred to as ________.

A)atomic energy
B)electron affinity
C)entropy of vaporization
D)ionization energy
E)magnetic moment

Question 71

List in order of increasing size: K⁺,Se^2-,Cl^-,Na⁺,S^2-.

A)Cl^- < S^2- < K⁺ < Na⁺ < Se^2-
B)Na⁺ < K⁺ < Cl^- < S^2- < Se^2-
C)S^2- < Na⁺ < Cl^- < Se^2- < ^K+
D)Cl^- < Se^2- < K⁺ < Na⁺ < S^2-
E)K⁺ < Na⁺ < Cl^- < Se^2- < S^2-

Question 72

Choose the paramagnetic atom or ion: Ca,Ne,Sc³⁺,Cl^-,Na.

A)Ca
B)Ne
C)Sc³⁺
D)Cl^-
E)Na

Question 73

List in order of increasing number of unpaired electrons: N,Na,Si,Cr,Ar.

A)Cr < Si < Na < N < Ar
B)Ar < Cr < N < Na < Si
C)Ar < Cr < Si < Na < N
D)N < Na < Cr < Si < Ar
E)Ar < Na < Si < N < Cr

Question 74

Which of the following has the highest first ionization potential: Sb,I,In,Xe,Rb?

A)Sb
B)I
C)In
D)Xe
E)Rb

Question 75

Which of the following has the highest first ionization potential: K,Ge,Kr,Ca,Br?

A)K
B)Ge
C)Kr
D)Ca
E)Br

Question 76

Which of the following has the most negative electron affinity: Li,Be,N,O,F?

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

Question 77

Which of the following has the most unpaired electrons: Na,Mn²⁺ ,S,N,Ar?

A)Na
B)Mn²⁺
C)S
D)N
E)Ar

Question 78

Arrange the following elements in order of increasing ionization energy: Cs,Sc,Mn.

A)Sc < Mn < Cs
B)Sc < Cs < Mn
C)Cs < Mn < Sc
D)Cs < Sc < Mn
E)Mn < Cs < Sc

Question 79

Which of the following has the largest number of unpaired electrons: S,Cr²⁺ ,N,K,Ne?

A)S
B)Cr²⁺
C)N
D)K
E)Ne

Question 80

Choose the paramagnetic atom or ion: Zn,Zn²⁺,Mn²⁺,Ar,Al³⁺.

A)Zn
B)Zn²⁺
C)Mn²⁺
D)Ar
E)Al³⁺