Chemistry: A Molecular Approach, 3e (Tro)
Chapter 8 Periodic Properties of the Elements
Multiple Choice Questions
1) No two electrons can have the same four quantum numbers is known as the
A) Pauli exclusion principle
B) Hund’s rule
C) Aufbau principle
D) Heisenberg uncertainty principle
2) Only two electrons, with opposing spins, are allowed in each orbital is known as the
A) Pauli exclusion principle
B) Hund’s rule
C) Aufbau principle
D) Heisenberg uncertainty principle
3) When filling degenerate orbitals, electrons fill them singly first, with parallel spins is known as
A) Pauli exclusion principle
B) Hund’s rule
C) Aufbau principle
D) Heisenberg uncertainty principle
4) Choose the orbital diagram that represents the ground state of N.
A)
B)
C)
D)
E)
5) Choose the valence orbital diagram that represents the ground state of Zn.
A)
B)
C)
D)
E)
6) Which of the following statements is TRUE?
A) An orbital that penetrates into the region occupied by core electrons is less shielded from nuclear
charge than an orbital that does not penetrate and therefore has a lower energy.
B) An orbital that penetrates into the region occupied by core electrons is more shielded from nuclear
charge than an orbital that does not penetrate and therefore has a lower energy.
C) It is possible for two electrons in the same atom to have identical values for all four quantum
numbers.
D) Two electrons in the same orbital can have the same spin.
E) None of the above are true.
7) The element that corresponds to the electron configuration 1s22s22p63s23p64s13d5 is ________.
A) titanium
B) vanadium
C) chromium
D) manganese
E) iron
8) Give the ground state electron configuration for Se.
A) [Ar]4s23d104p4
B) [Ar]4s24d104p4
C) [Ar]4s23d104p6
D) [Ar]4s23d10
E) [Ar]3d104p4
9) Give the ground state electron configuration for I.
A) [Kr]5s24d105p6
B) [Kr]5s24d105p5
C) [Kr]4d105p6
D) [Kr]5s25p6
E) [Kr]5s25d105p6
10) Give the ground state electron configuration for Sr.
A) [Kr]5s24d2
B) [Kr]5s24d105p2
C) [Kr]5s2
D) [Kr]5s25d105p2
E) [Kr]5s24d10
11) Give the ground state electron configuration for Pb.
A) [Xe]6s26p2
B) [Xe]6s25d106p2
C) [Xe]6s25f146d106p2
D) [Xe]6s24f145d106p2
E) [Xe]6s24f145d106s26p2
12) Give the ground state electron configuration for Cd.
A) [Kr]5s25d10
B) [Kr]5s24d105p2
C) [Kr]4d10
D) [Kr]5s24d8
E) [Kr]5s24d10
13) Give the complete electronic configuration for Mn.
A) 1s22s22p63s23p64s24d5
B) 1s22s22p63s23p64s13d6
C) 1s22s22p63s23p64s23d5
D) 1s22s22p63s23p64s24p5
14) Identify the element that has a ground state electronic configuration of [Kr]5s24d5.
A) Tc
B) Mn
C) Nb
D) Ru
15) Give the number of core electrons for Cd.
A) 44
B) 48
C) 46
D) 45
E) 47
16) Give the number of valence electrons for Cd.
A) 8
B) 10
C) 12
D) 2
E) 6
17) How many valence electrons does an atom of Al possess?
A) 1
B) 2
C) 5
D) 3
E) 8
18) How many valence electrons do the halogens possess?
A) 5
B) 6
C) 2
D) 1
E) 7
19) How many valence electrons do the alkali earth metals possess?
A) 1
B) 2
C) 7
D) 6
E) 8
20) How many valence electrons do the alkali metals possess?
A) 1
B) 2
C) 7
D) 6
E) 8
21) How many valence electrons do the noble gases possess?
A) 1
B) 2
C) 7
D) 6
E) 8
22) Place the following elements in order of increasing atomic radius.
P Ba Cl
A) Ba < P < Cl
B) P < Cl < Ba
C) Cl < P < Ba
D) Cl < Ba < P
E) Ba < Cl < P
23) Place the following in order of increasing atomic radius.
As O Br
A) As < Br < O
B) O < As < Br
C) Br < As < O
D) As < O < Br
E) O < Br < As
24) A cation of +2 indicates that an element has
A) lost two electrons.
B) lost two protons.
C) lost two neutrons.
D) gained two electrons.
E) gained two protons.
25) Place the following in order of increasing radius.
Br⁻ Na⁺ Rb⁺
A) Br⁻ < Rb⁺ < Na⁺
B) Na⁺ < Rb⁺ < Br⁻
C) Rb⁺ < Br⁻ < Na⁺
D) Br⁻ < Na⁺ < Rb⁺
E) Rb⁺ < Na⁺ < Br⁻
26) Place the following in order of decreasing radius.
Te2⁻ F⁻ O2⁻
A) F⁻ > O2⁻ > Te2⁻
B) F⁻ > Te2⁻ > O2⁻
C) Te2⁻ > O2⁻ > F⁻
D) Te2⁻ > F⁻ > O2⁻
E) O2⁻ > F⁻ > Te2⁻
27) Choose the statement that is TRUE.
A) Outer electrons efficiently shield one another from nuclear charge.
B) Core electrons effectively shield outer electrons from nuclear charge.
C) Valence electrons are most difficult of all electrons to remove.
D) Core electrons are the easiest of all electrons to remove.
E) All of the above are true.
28) Which reaction below represents the first ionization of O?
A) O⁺(g) + e⁻ → O(g)
B) O(g) + e⁻ → O⁻(g)
C) O⁻(g) → O(g) + e⁻
D) O(g) → O⁺(g) + e⁻
E) O⁻(g) + e⁻ → O2⁻(g)
29) Which reaction below represents the second ionization of Sr?
A) Sr(g) → Sr⁺(g) + e⁻
B) Sr2⁺(g) + e⁻ → Sr⁺(g)
C) Sr⁺(g) + e⁻ → Sr(g)
D) Sr⁻(g) + e⁻ → Sr2⁻(g)
E) Sr⁺(g) → Sr2⁺(g) + e⁻
30) What period 3 element having the following ionization energies (all in kJ/mol)?
IE1 = 1012 IE2 = 1900 IE3= 2910 IE4= 4960 IE5= 6270 IE6 = 22,200
A) Si
B) S
C) P
D) Cl
E) Mg
31) Place the following in order of increasing IE1.
N F As
A) N < As < F
B) As < N < F
C) F < N < As
D) As < F < N
E) F < As < N
32) Place the following in order of decreasing IE1.
Cs Mg Ar
A) Cs > Mg > Ar
B) Mg > Ar > Cs
C) Ar > Mg > Cs
D) Cs > Ar > Mg
E) Mg > Cs > Ar
33) Place the following in order of increasing IE1.
K Ca Rb
A) Ca < K < Rb
B) Rb < Ca < K
C) Ca < Rb < K
D) Rb < K < Ca
E) K < Ca < Rb
34) Identify the species that has the smallest radius.
A) cation
B) anion
C) neutral
D) they are all the same size
35) Identify the species that has the smallest radius.
A) N-5
B) N-2
C) N0
D) N+1
E) N+3
36) Identify the number of valence electrons in Cl-1.
A) 6
B) 7
C) 8
D) 5
E) 4
37) Give the ground state electron configuration for Br⁻.
A) [Ar]4s23d104p6
B) [Ar]4s23d104p5
C) [Ar]4s24p6
D) [Ar]4s24d104p6
E) [Ar]4s23d104p4
38) Give the ground state electron configuration for Mg2⁺.
A) 1s22s22p63s2
B) 1s22s22p6
C) 1s22s22p63s23p2
D) 1s22s22p63s23p6
E) 1s22s22p63s1
39) Give the ground state electron configuration for Rb⁺.
A) [Ar]4s24p6
B) [Kr]5s1
C) [Ar]4s23d104p6
D) [Kr]5s2
E) [Kr]5s24d2
40) Give the ground state electron configuration for Se2⁻.
A) [Ar]4s23d104p4
B) [Ar]4s23d104p2
C) [Ar]4s24p6
D) [Ar]4s23d104p6
E) [Ar]4s23d84p6
41) Give the ground state electron configuration for the ion of Ba.
A) [Kr]5s25p6
B) [Kr]5s24d105p66s26p2
C) [Kr]5s24d105p66s1
D) [Kr]5s24d105p66s2
E) [Kr]5s24d105p6
42) Choose the ground state electron configuration for Ti2⁺.
A) [Ar]3d2
B) [Ar]4s2
C) [Ar]4s23d2
D) [Ar]4s23d4
E) [Ar]3d4
43) Choose the ground state electron configuration for Zn2⁺.
A) [Ar]4s23d8
B) [Ar]3d10
C) [Ar]4s23d6
D) [Ar]
E) [Ar]3d8
44) Choose the ground state electron configuration for Cr3⁺.
A) [Ar]4s13d2
B) [Ar]
C) [Ar]4s23d6
D) [Ar]3d3
E) [Ar]4s23d1
45) Choose the valence orbital diagram that represents the ground state of Sr2⁺.
A)
B)
C)
D)
E)
46) Choose the valence orbital diagram that represents the ground state of Se2⁻.
A)
B)
C)
D)
E)
47) Which reaction below represents the electron affinity of Li?
A) Li(g) + e⁻ → Li⁻(g)
B) Li(g) → Li⁺(g) + e⁻
C) Li(g) + e⁻ → Li⁺(g)
D) Li⁺(g) → Li(g) + e⁻
E) Li⁺(g) + e⁻ → Li(g)
48) Which reaction below represents the second electron affinity of S?
A) S(g) + e⁻ → S⁻(g)
B) S⁻(g) + e⁻ → S2⁻(g)
C) S(g) → S⁺(g) + e⁻
D) S⁻(g) → S(g) + e⁻
E) S2⁻(g) → S⁻(g) + e⁻
49) Place the following in order of decreasing metallic character.
P As K
A) P > As > K
B) As > P > K
C) K > P > As
D) As > K > P
E) K > As > P
50) Place the following in order of increasing metallic character.
Rb Cs K Na
A) K < Cs < Na < Rb
B) Na < K < Rb < Cs
C) Cs < Rb < K < Na
D) K < Cs < Rb < Na
E) Na < Rb < Cs < K
51) Describe the reaction of the noble gases with metals.
A) inert
B) vigorous
C) mild reaction
D) forms water
E) dissolves
52) Describe the reaction of the alkali metals with non-metals.
A) inert
B) vigorous
C) mild reaction
D) forms water
E) dissolves
53) Identify the most reactive alkali metal with water.
A) Cs
B) Rb
C) K
D) Na
E) Li
54) Identify a characteristic of halogens.
A) powerful reducing agents
B) forms water in reactions
C) powerful oxidizing agents
D) absorbs water in reactions
E) inert
55) Halogens can react with each other to form
A) covalent bonds.
B) ionic bonds.
C) salts.
D) hydrogen halides.
E) metal halides.
56) The U.S. Food and Drug Administration recommends the ingestion of recommended doses of
________ in the event of a nuclear emergency.
A) sodium bromide
B) sodiuim chloride
C) potassium iodide
D) potassium bromide
E) sodium iodide
Algorithmic Questions
1) Give the set of four quantum numbers that could represent the last electron added (using the Aufbau
principle) to the Cl atom.
A) n = 3, l = 1, ml = 1, ms = +
B) n = 3, l = 0, ml = 1, ms = –
C) n = 3, l = 2, ml =1, ms = +
D) n = 2, l = 1, ml = 1, ms = –
E) n = 3, l =1, ml = 1, ms = –
2) Give the set of four quantum numbers that could represent the last electron added (using the Aufbau
principle) to the Ne atom.
A) n = 2, l = 1, ml = 1, ms = +
B) n = 3, l = 0, ml = 1, ms = +
C) n = 3, l = 2, ml =1, ms = +
D) n = 2, l = 1, ml = 1, ms = –
E) n = 3, l =2, ml = 1, ms = –
3) Give the set of four quantum numbers that could represent the last electron added (using the Aufbau
principle) to the Sr atom.
A) n = 5, l = 0, ml = 0, ms = –
B) n = 4, l = 1, ml = 1 ms = –
C) n = 5, l = 0, ml = 0, ms = +
D) n = 4, l = 1, ml = -1, ms = +
E) n = 5, l = 1, ml =1, ms = +
4) Give the set of four quantum numbers that represent the last electron added (using the Aufbau
principle) to the Zn atom.
A) n = 4, l = 3, ml = 3, ms = +
B) n = 3, l = 2, ml = 2, ms = –
C) n = 3, l = 1, ml = 1, ms = –
D) n = 3, l = 2, ml = 2, ms = +
E) n = 4, l = 1 ml = 0, ms = +
5) Identify the element that has a ground state electronic configuration of [Ar]4s23d104p1.
A) Al
B) In
C) Ga
D) B