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Chapter 7: Periodic Trends

Multiple Choice
Identify the choice that best completes the statement or answers the question.
 

 1. 
Elements in the modern version of the periodic table are arranged in order of increasing __________.
a.
oxidation number
b.
atomic mass
c.
average atomic mass
d.
atomic number
e.
number of isotopes
 

 2. 
An electron in a(n) __________ subshell experiences the greatest effective nuclear charge in a many-electron atom.
a.
3f
b.
3p
c.
3d
d.
3s
e.
4s
 

 3. 
In which orbital does an electron in a phosphorus atom experience the greatest shielding?
a.
2p
b.
3s
c.
3p
d.
3s
e.
1s
 

 4. 
The first ionization energies of the elements __________ as you go from left to right across a period of the periodic table, and __________ as you go from the bottom to the top of a group in the table.
a.
increase, increase
b.
increase, decrease
c.
decrease, increase
d.
decrease, decrease
e.
are completely unpredictable
 

 5. 
The __________ have the most negative electron affinities.
a.
alkaline earth metals
b.
alkali metals
c.
halogens
d.
transition metals
e.
chalcogens
 

 6. 
In general, as you go across a period in the periodic table from left to right:
(1)  the atomic radius __________;
(2)  the electron affinity becomes __________ negative; and
(3)  the first ionization energy __________.
a.
decreases, decreasingly, increases
b.
increases, increasingly, decreases
c.
increases, increasingly, increases
d.
decreases, increasingly, increases
e.
decreases, increasingly, decreases
 

 7. 
Element M reacts with chlorine to form a compound with the formula MCl2.  Element M is more reactive than magnesium and has a smaller radius than barium.  This element is __________.
a.
Sr
b.
K
c.
Na
d.
Ra
e.
Be
 

 8. 
Na reacts with element X to form an ionic compound with the formula Na3X.  Ca will react with X to form __________.
a.
CaX2
b.
CaX
c.
Ca2X3
d.
Ca3X2
e.
Ca3X
 

 9. 
Oxides of the active metals combine with water to form __________.
a.
metal hydroxides
b.
metal hydrides
c.
hydrogen gas
d.
oxygen gas
e.
water and a salt
 

 10. 
Oxides of most nonmetals combine with water to form __________.
a.
an acid
b.
a base
c.
water and a salt
d.
water
e.
hydrogen gas
 

 11. 
The reaction of a metal with a nonmetal produces a(n) __________.
a.
base
b.
salt
c.
acid
d.
oxide
e.
hydroxide
 

 12. 
In which set of elements would all members be expected to have very similar chemical properties?
a.
O, S, Se
b.
N, O, F
c.
Na, Mg, K
d.
S, Se, Si
e.
Ne, Na, Mg
 

 13. 
Electrons in the 1s subshell are much closer to the nucleus in Ar than in He due to the larger __________ in Ar.
a.
nuclear charge
b.
paramagnetism
c.
diamagnetism
d.
Hund's rule
e.
azimuthal quantum number
 

 14. 
The atomic radius of main-group elements generally increases down a group because __________.
a.
effective nuclear charge increases down a group
b.
effective nuclear charge decreases down a group
c.
effective nuclear charge zigzags down a group
d.
the principal quantum number of the valence orbitals increases
e.
both effective nuclear charge increases down a group and the principal quantum number of the valence orbitals increases
 

 15. 
Screening of the nuclear charge by core electrons in atoms is __________.
a.
less efficient than that by valence electrons
b.
more efficient than that by valence electrons
c.
essentially identical to that by valence electrons
d.
responsible for a general decrease in atomic radius going down a group
e.
both essentially identical to that by valence electrons and responsible for a general decrease in atomic radius going down a group
 

 16. 
Which of the following is an isoelectronic series?
a.
B5-, Si4-, As3-, Te2-
b.
F-, Cl-, Br-, I-
c.
S, Cl, Ar, K
d.
Si2-, P2-, S2-, Cl2-
e.
O2-, F-, Ne, Na+
 

 17. 
Of the following elements, which has the largest first ionization energy?
a.
Na
b.
Al
c.
Se
d.
Cl
e.
Br
 

 18. 
Of the elements below, __________ has the largest first ionization energy.
a.
Li
b.
K
c.
Na
d.
H
e.
Rb
 

 19. 
Which of the following has the largest second ionization energy?
a.
Si
b.
Mg
c.
Al
d.
Na
e.
P
 

 20. 
Which equation correctly represents the first ionization of aluminum?
a.
Al- (g) ® Al (g)  +  e-
b.
Al (g)  ® Al- (g)  +  e-
c.
Al (g)  +  e- ® Al- (g)
d.
Al (g) ® Al+ (g)  +  e-
e.
Al+ (g)  +  e- ® Al (g)
 

 21. 
Which of the following correctly represents the second ionization of aluminum?
a.
Al+ (g)  +  e- ® Al (g)
b.
Al (g) ® Al+ (g)  +  e-
c.
Al- (g)  +  e- ® Al2- (g)
d.
Al+ (g)  +  e- ® Al2+ (g)
e.
Al+ (g) ® Al2+ (g)  +  e-
 

 22. 
Of the following elements, __________ has the most negative electron affinity.
a.
Na
b.
Li
c.
Be
d.
N
e.
F
 

 23. 
Of the following elements, __________ has the most negative electron affinity.
a.
P
b.
Al
c.
Si
d.
Cl
e.
B
 

 24. 
Chlorine is much more apt to exist as an anion than is sodium.  This is because __________.
a.
chlorine is bigger than sodium
b.
chlorine has a greater ionization energy than sodium does
c.
chlorine has a greater electron affinity than sodium does
d.
chlorine is a gas and sodium is a solid
e.
chlorine is more metallic than sodium
 

 25. 
Sodium is much more apt to exist as a cation than is chlorine.  This is because __________.
a.
chlorine is a gas and sodium is a solid
b.
chlorine has a greater electron affinity than sodium does
c.
chlorine is bigger than sodium
d.
chlorine has a greater ionization energy than sodium does
e.
chlorine is more metallic than sodium
 

 26. 
Which of the following correctly represents the electron affinity of bromine?
a.
Br (g) ® Br+ (g)  +  e-
b.
Br (g)  +  e- ® Br- (g)
c.
Br2 (g)  +  e- ® Br- (g)
d.
Br2 (g)  +  2 e- ® 2 Br- (g)
e.
Br+ (g)  +  e- ® Br (g)
 



 
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