6) Give the electron configuration for O.
A) 1s22s22p4
B) 1s22p4
C) 1s22s22p3
D) 1s22s22p5
E) 1s22s12p1
7) The element that corresponds to the electron configuration 1s22s22p6 is ________.
A) sodium
B) magnesium
C) lithium
D) beryllium
E) neon
8) The element that corresponds to the electron configuration 1s22s22p63s23p64s23d3 is ________.
A) scandium
B) manganese
C) vanadium
D) iron
E) cobalt
9) The complete electron configuration of argon, element 18, is ________.
A) 1s22s22p63s23p6
B) 1s22s22p103s23p2
C) 1s42s42p63s4
D) 1s42s42p10
E) 1s62s62p23s4
10) The complete electron configuration of gallium, element 31, is ________.
A) 1s22s22p103s23p104s23d3
B) 1s22s22p63s23p63d104s24p1
C) 1s42s42p63s43p64s43d3
D) 1s22s42p103s43p9
E) 1s22s42p83s43p84s3
11) The condensed electron configuration of silicon, element 14, is ________.
A) [He]2s42p6
B) [Ne]2p10
C) [Ne]3s23p2
D) [He]2s4
E) [He]2s62p2
12) The condensed electron configuration of krypton, element 36, is ________.
A) [Kr]4s23d8
B) [Ar]4s4
C) [Kr]4s43d8
D) [Ar]3d104s24p6
E) [Ar]4s43d4
13) Which element has the ground-state electron configuration [Xe]6s24f 7?
A) Re
B) Ir
C) Eu
D) Gd
14) Give the number of valence electrons for Cl.
A) 8
B) 6
C) 5
D) 3
E) 7
15) Give the number of core electrons for Se.
A) 26
B) 30
C) 28
D) 32
E) 34
16) Give the number of valence electrons for Se.
A) 0
B) 8
C) 2
D) 4
E) 6
17) Give the number of valence electrons for Si.
A) 4
B) 2
C) 28
D) 12
E) 26
18) How many unpaired electrons are present in the ground state As atom?
A) 0
B) 3
C) 1
D) 2
E) 4
19) How many unpaired electrons are present in the ground state Kr atom?
A) 1
B) 2
C) 0
D) 3
E) 5
20) How many unpaired electrons are present in the ground state C atom?
A) 5
B) 3
C) 1
D) 2
E) 4
21) How many unpaired electrons are there in the ground state of Cl?
A) 5
B) 4
C) 3
D) 2
E) 1
22) How many of the following elements have 2 unpaired electrons in the ground state?
C Te Hf Si
A) 1
B) 2
C) 3
D) 4
23) How many of the following elements have 1 unpaired electron in the ground state?
B Al O F
A) 1
B) 2
C) 3
D) 4
24) Identify the number of valence electrons for Ti.
A) 8
B) 7
C) 4
D) 2
25) How many valence electrons does an atom of As have?
A) 3
B) 5
C) 8
D) 4
E) 6
26) How many valence electrons does an atom of Mg possess?
A) 2
B) 1
C) 8
D) 5
E) 3
27) How many valence electrons does an atom of Ti possess?
A) 2
B) 4
C) 6
D) 8
E) 0
28) How many valence electrons does an atom of Ag possess?
A) 2
B) 5
C) 11
D) 3
E) 1
29) How many valence shell electrons does an atom of indium have?
A) 1
B) 4
C) 3
D) 49
E) 2
30) An element that has the valence electron configuration 6s26p6 belongs to which period and group?
A) period 6; group 6A
B) period 6; group 8A
C) period 7; group 6A
D) period 7; group 8A
31) Which of the following have their valence electrons in the same shell?
A) Li, N, F
B) B, Si, As
C) N, As, Bi
D) He, Ne, F
32) Which of the following have the same number of valence electrons?
A) Rb, Sb, I
B) Ga, Sn, Bi
C) As, Sb, Bi
D) Ar, Kr, Br
33) What is the general valence-electron ground-state electron configuration for neutral alkaline earth
metals?
A) ns1
B) ns2
C) 1s22s1
D) 1s22s2
34) How many valence electrons does a neutral tellurium atom have?
A) 2
B) 4
C) 6
D) 52
35) Place the following elements in order of decreasing atomic radius.
Xe Rb Ar
A) Ar > Xe > Rb
B) Xe > Rb > Ar
C) Ar > Rb > Xe
D) Rb > Xe > Ar
E) Rb > Ar > Xe
36) Of the following, which atom has the largest atomic radius?
A) Rb
B) I
C) Cs
D) At
37) Of the following, which atom has the smallest atomic radius?
A) K
B) As
C) Rb
D) Sb
38) Which atom in each group (I and II) has the smallest atomic radius?
(I) Ba, Hf, At (II) As, Sb, Bi
A) Ba; As
B) Ba; Bi
C) At; As
D) At; Bi
39) Give the number of core electrons for Cl–.
A) 22
B) 30
C) 17
D) 12
E) 10
40) Give the number of valence electrons for Br–.
A) 34
B) 36
C) 6
D) 8
E) 7
23
41) Choose the ground state electron configuration for Hf2⁺.
A) [Xe]6s2
B) [Xe]6s25d2
C) [Xe]5d2
D) [Xe]
E) [Xe]6s25d4
42) How many electrons are in the outermost shell of the Ga3+ ion in its ground state?
A) 2
B) 3
C) 6
D) 18
43) Place the following in order of increasing radius.
Ba2⁺ Te2⁻ I⁻
A) Ba2⁺ < I⁻ < Te2⁻
B) I⁻ < Ba2⁺ < Te2⁻
C) Te2⁻ < I⁻ < Ba2⁺
D) Ba2⁺ < Te2⁻ < I⁻
E) I⁻ < Te2⁻ < Ba2⁺
44) Choose the paramagnetic species from below.
A) Ca
B) O2⁻
C) Zn2⁺
D) Cd
E) Nb3⁺
45) Choose the diamagnetic species from below.
A) Sn2⁺
B) I
C) N
D) Cr
E) None of the above are diamagnetic.
46) Choose the paramagnetic species from below.
24
A) Ti4⁺
B) Se
C) Ar
D) All of the above are paramagnetic.
E) None of the above are paramagnetic.
47) How many of the following species are paramagnetic?
Sc3⁺ Cl⁻ Ba2⁺ Se
A) 0
B) 2
C) 1
D) 4
E) 3
48) How many of the following species are diamagnetic?
Fr Zr2⁺ Al3⁺ Hg2⁺
A) 1
B) 3
C) 0
D) 2
E) 4
49) Which ion does not have a noble gas configuration in its ground state?
A) Sc3+
B) Al3+
C) Ga3+
D) As3-
50) Of the following, which element has the highest first ionization energy?
A) beryllium
B) boron
C) carbon
D) lithium
51) Of the following, which element has the highest first ionization energy?
A) Al
B) Cl
C) Na
D) P
52) Of the following, which element has the highest first ionization energy?
A) barium
B) lead
C) cesium
D) thallium
53) Of the following, which element has the highest first ionization energy?
A) Sr
B) Rb
C) Na
D) Ca
54) Of the following, which element has the highest first ionization energy?
A) Sr
B) Br
C) K
D) Te
55) Which ionization process requires the most energy?
A) W(g) → W+(g) + e–
B) W+(g) → W2+(g) + e–
C) W2+(g) → W3+(g) + e–
D) W3+(g) → W4+(g) + e–
56) Which ionization process requires the most energy?
A) O(g) → O+(g) + e–
B) O+(g) → O2+(g) + e–
C) F(g) → F+(g) + e–
D) F+(g) → F2+(g) + e–
57) Which of the following species will have the highest ionization energy?
A) K+
B) Ar
C) Cl–
D) S2-
58) Which of the following represents the change in electronic configuration that is associated with the
first ionization energy of strontium?
A) [Kr]5s15p1 → [Kr]5s1 + e–
B) [Kr]5s2 → [Kr]5s15p1
C) [Kr]5s2 → [Kr]5s1 + e–
D) [Kr]5s2 + e– → [Kr]5s25p1
59) Give the set of four quantum numbers that could represent the electron gained to form the Br ION
from the Br atom.
A) n = 4, l = 1, ml = 1, ms = +
B) n = 4, l = 0, ml = -1, ms = +
C) n = 4, l = 1, ml = 1, ms = –
D) n = 3, l = 2, ml = 1, ms = +
E) n = 5, l = 1, ml =-1, ms = –
60) Give the set of four quantum numbers that could represent the electron lost to form the K ION from
the K atom.
A) n = 3, l = 1, ml = 1, ms = –
B) n = 4, l = 0, ml = 0, ms = –
C) n = 4, l = 4, ml = 0, ms = –
D) n = 4, l = 0, ml = 0, ms = +
E) n = 3, l = 0, ml = -1, ms = –
61) Give the set of four quantum numbers that could represent the electron lost to form the Rb ION
from the Rb atom.
A) n = 6, l = 0, ml = -1 ms = –
B) n = 4, l = 1, ml = 1, ms = +
C) n = 5, l = 0, ml = 0, ms = –
D) n = 4, l = 1, ml = 0, ms = –
E) n = 5, l = 0, ml = 0, ms = +
62) Place the following in order of decreasing metallic character.
C O N F
A) O > N > F > C
B) F > O > N > C
C) C > N > O > F
D) F > N > O > C
E) N > C > O > F
63) Which element has the highest first electron affinity?
A) Na
B) Mg
C) O
D) Ne
64) Identify the states of the halogens at room temperature.
A) Fluorine, chlorine, bromine, and iodine are solids.
B) Fluorine, chlorine, and bromine are solids, and iodine is a solid.
C) Fluorine and iodine are solids, chlorine and bromine are gases.
D) Fluorine is a gas, chlorine and bromine are liquids, and iodine is a solid.
E) Fluorine and chlorine are gases, bromine is a liquid, and iodine is a solid.
Matching Questions
Match the following.
A) electrons in the outermost shell
B) 1
C) electrons in completed shells
D) 2
E) number of unpaired electrons in Zn2+
1) valence electrons
Diff: 1 Page Ref: 8.4
2) core electrons
Diff: 1 Page Ref: 8.4
3) number of unpaired electrons in Na
Diff: 1 Page Ref: 8.4
4) 0
Diff: 1 Page Ref: 8.7
5) number of unpaired electrons in Ti2+
Diff: 1 Page Ref: 8.7
29
Short Answer Questions
1) Why does the size of the transition elements stay roughly the same across a period?
2) Define paramagnetic.
3) Define ionization energy.
4) List the noble gas that has the highest ionization energy.
5) Below is a list of successive ionization energies (in kJ/mol) for a period 3 element. Identify the
element and explain how you came to that conclusion.
IE2 = 2250 IE3 = 3360 IE4= 4560 IE5= 7010 IE6= 8500 IE7 = 27,100
6) Why do successive ionization energies increase?
7) Why is the first ionization energy of sulfur smaller than the first ionization energy of phosphorus?
8) Give the ground state electron configuration for Cd+2.
9) Give the number of core electrons for Mg2+.
10) Give the number of valence electrons for Mg2+.
11) Define electron affinity.
12) Why do Li, Na, and K have similar chemical properties?