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Quantum Number & Periodic Trend

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

 1. 
From the Bohr model of the hydrogen atom we can conclude that the energy required to excite an electron from n = 2 to n = 3 is ___________ the energy to excite an electron from n = 3 to n = 4. (Hint: Ionization energy)
a.
less than
b.
greater than
c.
equal to
d.
either equal to or less than
e.
either ezual to or greater than
 

 2. 
Which quantum number distinguishes the different shapes of the orbitals?
a.
n
b.
l
c.
ml
d.
ms
e.
c and d are both correct
 

 3. 
How many values are there for the magnetic quantum number (ml) when the value of the angular momentum quantum number is 3?
a.
1
b.
3
c.
5
d.
7
e.
9
 

 4. 
Which of the following statements is (are) true? (Research this.)
1.      An excited atom can return to a higher energy level by emitting light energy.
2.      An atom can be excited to a higher energy level by absorption of light energy.
3.      The frequency and wavelength of light are inversely proportional.
a.
1
b.
2
c.
1 and 2
d.
2 and 3
e.
all statements are correct.
 

 5. 
Which of the following sets of quantum numbers is NOT permissible?
a.
n = 1, l = 0, ml = 0, ms = + 1/2
b.
n = 4, l = 0, ml = 0, ms = + 1/2
c.
n = 3, l = 3, ml = –3, ms = – 1/2
d.
n = 2, l = 1, ml = 1, ms = – 1/2
e.
n = 2, l = 0, ml = 0, ms = + 1/2
 

 6. 
n = 2, l = 0, ml = 0, ms = + All the following statements are true EXCEPT
a.
the n = 2 energy level has d orbitals.
b.
the 2p orbitals can have a maximum of 6 electrons.
c.
the s orbital has a spherical shape.
d.
there are 5 d orbitals in a set.
e.
the fourth major energy level has one set of f orbitals.
 

 7. 
The principle/first quantum number of the valence electrons in an atom of arsenic is
a.
2
b.
3
c.
4
d.
5
e.
6
 

 8. 
The n and l quantum numbers of the “last” electron of an element are
n = 5 and l = 1. The element could be a
1.   metal.
2.   nonmetal.
3.   metalloid.
a.
1 only
b.
2 only
c.
3 only
d.
1 and 2 only
e.
1, 2, and 3
 

 9. 
The maximum number of electrons that can occupy one i orbital is (the order of orbitals is as follows: s, p, d, f, g, h, i, j, k)
a.
9
b.
18
c.
26
d.
34
e.
50
 

 10. 
Which of the following orbital diagrams represents a paramagnetic atom?
mc010-1.jpg
a.
1
b.
2
c.
3
d.
1 and 2
e.
2 and 3
 

 11. 
The ground-state electron configuration of a Fe2+ ion is 1s2 2s2 2p6 3s2 3p6 3d6. Therefore, Fe2+ is
a.
diamagnetic.
b.
paramagnetic with one unpaired electron.
c.
paramagnetic with two unpaired electrons.
d.
paramagnetic with four unpaired electrons.
e.
paramagnetic with five unpaired electrons.
 

 12. 
Which of the following statements about different elements are true?
1.      As is a metalloid and Se is a nonmetal.
2.      Cu is a transition element and Ge is a metalloid.
3.      Both F and I are halogens.
a.
1 only
b.
2 only
c.
3 only
d.
1 and 2 only
e.
1, 2, and 3.
 

 13. 
A section of the periodic table with all identification features removed is shown below.
       mc013-1.jpg

Which element has the smallest atomic radius?
a.
V
b.
W
c.
X
d.
Z
e.
X and Z will have the same radius because they are the furthest to the right.
 

 14. 
Which of the following atoms has the LARGEST atomic radius?
a.
Sr
b.
Mg
c.
P
d.
I
e.
Kr
 

 15. 
Which of the following atoms designated by electronic configurations has the highest ionization energy?
a.
[Ne] 3s2 3p2   
b.
[Ne] 3s2 3p3   
c.
[Ar] 3d10 4s2 4p3    
d.
[Kr] 4d10 5s2 5p3     
e.
[Xe] 4f14 5d10 6s2 6p3
 

 16. 
Which of the following has the highest ionization energy for the removal of the second electron?
a.
Na
b.
Be
c.
Mg
d.
P
e.
Ne
 

 17. 
Which one of the following elements would be expected to have the SMALLEST atomic radius?
a.
Li
b.
Cs
c.
F
d.
Br
e.
I
 

 18. 
Which of the following represent ionization energy.

      a.      I + e-    ->    I–
      b.      I2    ->    2I
      c.      I    ->    I+ + e-
      d.      Na + I    ->     NaI
      e.      2Na + I2    ->     2NaI(s)
a.
A
b.
B
c.
C
d.
D
e.
E
f.
A and C
g.
none of the above.
 

 19. 
Refer to the reactions in question 18.

Which represent electron affinity?
a.
A
b.
B
c.
C
d.
D
e.
E
f.
A and C
g.
none of the above.
 

 20. 
Which of the following properties, in general, increase as we move left to right across a period in the periodic table?
1.      atomic radius
2.      ionization energy
3.      reactivity
a.
1 only
b.
2 only
c.
3 only
d.
1 and 2 only
e.
2 and 3 only
 

 21. 
If atoms were placed in order according to their masses, which of the following would trend from beginning to end?
a.
ionization energy
b.
atomic radii
c.
electron configurations
d.
electron affinity
e.
atomic masses
f.
all of the above.
 

 22. 
Elements R and T are covalently bonded together.  R is slightly positive and T is slightly negative.  They are both in the same energy level.

What can you conclude about R and T?
a.
R has a greater effective nuclear charge than T.
b.
T will be slightly smaller than R.
c.
T is more reactive than R.
d.
T will “steal” an electron from R.
e.
both choices a and c are true.
 

 23. 
You will need to research this question.

What is the wavelength of light associated with the radiation of 7.26*10–19 J/photon? (h = 6.63*10–34 J • s.) (h is a measure of frequency)
a.
137 nanometers
b.
231 nanometers
c.
274 nanometers
d.
548 nanometers
e.
684 nanometers
 



 
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