Chemistry Chapter 5A (Prentice)
 
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Chemistry Chapter 5A (Prentice)

Matching
 
 
Match each item with the correct statement below.
a.
atomic orbital
d.
ground state
b.
aufbau principle
e.
Pauli exclusion principle
c.
electron configuration
f.
Heisenberg uncertainty principle
 

 1. 

 region of high probability of finding an electron
 

 2. 

 states the impossibility of knowing both velocity and position of a moving particle at the same time
 

 3. 

 lowest energy level
 

 4. 

 tendency of electrons to enter orbitals of lowest energy first
 

 5. 

 arrangement of electrons around atomic nucleus
 

 6. 

 each orbital has at most two electrons
 

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

 7. 
In Bohr's model of the atom, where are the electrons and protons located?
a.
The electrons move around the protons, which are at the center of the atom.
b.
The electrons and protons move throughout the atom.
c.
The electrons occupy fixed positions around the protons, which are at the center of the atom.
d.
The electrons and protons are located throughout the atom, but they are not free to move.
 

 8. 
In the Bohr model of the atom, an electron in an orbit has a fixed ____.
a.
position
c.
energy
b.
color
d.
size
 

 9. 
How does the energy of an electron change when the electron moves closer to the nucleus?
a.
It decreases.
c.
It stays the same.
b.
It increases.
d.
It doubles.
 

 10. 
The principal quantum number indicates what property of an electron?
a.
position
c.
energy level
b.
speed
d.
electron cloud shape
 

 11. 
What is the shape of the 3p atomic orbital?
a.
sphere
c.
bar
b.
dumbbell
d.
two perpendicular dumbbells
 

 12. 
How many energy sublevels are in the second principal energy level?
a.
1
c.
3
b.
2
d.
4
 

 13. 
What is the maximum number of f orbitals in any single energy level in an atom?
a.
1
c.
5
b.
3
d.
7
 

 14. 
What is the maximum number of d orbitals in a principal energy level?
a.
1
c.
3
b.
2
d.
5
 

 15. 
What is the maximum number of orbitals in the p sublevel?
a.
2
c.
4
b.
3
d.
5
 

 16. 
What is the maximum number of electrons in the second principal energy level?
a.
2
c.
18
b.
8
d.
32
 

 17. 
When an electron moves from a lower to a higher energy level, the electron ____.
a.
always doubles its energy
b.
absorbs a continuously variable amount of energy
c.
absorbs a quantum of energy
d.
moves closer to the nucleus
 

 18. 
The shape (not the size) of an electron cloud is determined by the electron's ____.
a.
energy sublevel
c.
speed
b.
position
d.
principal quantum number
 

 19. 
The letter "p" in the symbol 4pmc019-1.jpg indicates the ____.
a.
spin of an electron
c.
principle energy level
b.
orbital shape
d.
speed of an electron
 

 20. 
If the spin of one electron in an orbital is clockwise, what is the spin of the other electron in that orbital?
a.
zero
c.
counterclockwise
b.
clockwise
d.
both clockwise and counterclockwise
 

 21. 
What types of atomic orbitals are in the third principal energy level?
a.
s and p only
c.
s, p, and d only
b.
p and d only
d.
s, p, d, and f
 

 22. 
What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p?
a.
2d
c.
3f
b.
3d
d.
4s
 

 23. 
According to the aufbau principle, ____.
a.
an orbital may be occupied by only two electrons
b.
electrons in the same orbital must have opposite spins
c.
electrons enter orbitals of highest energy first
d.
electrons enter orbitals of lowest energy first
 

 24. 
What is the number of electrons in the outermost energy level of an oxygen atom?
a.
2
c.
6
b.
4
d.
8
 

 25. 
What is the electron configuration of potassium?
a.
1smc025-1.jpg2smc025-2.jpg2pmc025-3.jpg3smc025-4.jpg3pmc025-5.jpg4smc025-6.jpg
c.
1smc025-12.jpg2smc025-13.jpg3smc025-14.jpg3pmc025-15.jpg3dmc025-16.jpg
b.
1smc025-7.jpg2smc025-8.jpg2pmc025-9.jpg3smc025-10.jpg3pmc025-11.jpg
d.
1smc025-17.jpg2smc025-18.jpg2pmc025-19.jpg3smc025-20.jpg3pmc025-21.jpg4smc025-22.jpg
 

 26. 
If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the three orbitals?
a.
one electron in each orbital
b.
two electrons in one orbital, one in another, none in the third
c.
three in one orbital, none in the other two
d.
Three electrons cannot fill three empty 2p atomic orbitals.
 

 27. 
How many unpaired electrons are in a sulfur atom (atomic number 16)?
a.
0
c.
2
b.
1
d.
3
 

Numeric Response
 

 28. 
How many electrons are in the highest occupied energy level of a neutral chlorine atom?

 

 29. 
How many electrons are in the highest occupied energy level of a neutral strontium atom?

 

 30. 
How many electrons are in the highest occupied energy level of copper?

 



 
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