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Chapter 4 Exam

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

 1. 
Visible light, X rays, infrared radiation, and radio waves all have the same
a.
energy.
c.
speed.
b.
wavelength.
d.
frequency.
 

 2. 
The speed of an electromagnetic wave is equal to the product of its wavelength and its
a.
mass.
c.
velocity.
b.
color.
d.
frequency.
 

 3. 
A line spectrum is produced when an electron moves from one energy level
a.
to a higher energy level.
b.
to a lower energy level.
c.
into the nucleus.
d.
to another position in the same sublevel.
 

 4. 
Because excited hydrogen atoms always produce the same line-emission spectrum, scientists concluded that hydrogen
a.
had no electrons.
b.
did not release photons.
c.
released photons of only certain energies.
d.
could only exist in the ground state.
 

 5. 
The equation E = hn helped Louis de Broglie determine
a.
how protons and neutrons behave in the nucleus.
b.
how electron wave frequencies correspond to specific energies.
c.
whether electrons behave as particles.
d.
whether electrons exist in a limited number of orbits with different energies.
 

 6. 
Which model of the atom explains the orbitals of electrons as waves?
a.
the Bohr model
c.
Rutherford's model
b.
the quantum model
d.
Planck's theory
 

 7. 
All of the following describe the Heisenberg uncertainly principle except
a.
it states that it is impossible to determine simultaneously both the position and velocity of an electron or any other particle.
b.
it is one of the fundamental principles of our present understanding of light and matter.
c.
it helped lay the foundation for the modern quantum theory.
d.
it helps to locate an electron in an atom.
 

 8. 
A spherical electron cloud surrounding an atomic nucleus would best represent
a.
an s orbital.
b.
a px orbital.
c.
a combination of px and py orbitals.
d.
a combination of an s and a px orbital.
 

 9. 
The p orbitals are shaped like
a.
electrons.
c.
dumbbells.
b.
circles.
d.
spheres.
 

 10. 
An orbital that can never exist according to the quantum description of the atom is
a.
3d.
c.
6d.
b.
8s.
d.
3f.
 

 11. 
The total number of orbitals that can exist at the second main energy level is
a.
2.
c.
4.
b.
3.
d.
8.
 

 12. 
How many orbitals can exist at the third main energy level?
a.
3
c.
9
b.
6
d.
18
 

 13. 
How many electrons can occupy the s orbitals at each energy level?
a.
two, if they have opposite spins
b.
two, if they have the same spin
c.
one
d.
no more than eight
 

 14. 
How many electrons are needed to completely fill the fourth energy level?
a.
8
c.
32
b.
18
d.
40
 

 15. 
At n = 1, the total number of electrons that could be found is
a.
1.
c.
6.
b.
2.
d.
18.
 

 16. 
A single orbital in the 3d level can hold ____ electrons.
a.
10
c.
3
b.
2
d.
6
 

 17. 
The statement that no two electrons in the same atom can have the same four quantum numbers is
a.
the Pauli exclusion principle.
c.
Bohr's law.
b.
Hund's rule.
d.
the Aufbau principle.
 

 18. 
Two electrons in the 1s orbital must have different spin quantum numbers to satisfy
a.
quantum rule.
c.
the Pauli exclusion principle.
b.
the magnetic rule.
d.
the Aufbau principle.
 

 19. 
The sequence in which energy sublevels are filled is specified by
a.
the Pauli exclusion principle.
c.
Lyman's series.
b.
the orbital rule.
d.
the Aufbau principle.
 

 20. 
The Aufbau principle states that an electron
a.
can have only one spin number.
b.
occupies the lowest available energy level.
c.
must be paired with another electron.
d.
must enter an s orbital.
 

 21. 
In the ground state, the 3d and 4s sublevels of the chromium atom (atomic number 24) are represented as
a.
3d6 4s1.
c.
3d5 4s1.
b.
3d4 4s2.
d.
4s2 3d4.
 

 22. 
The element with electron configuration 1s2 2s2 2p6 3s2 3p2 is
a.
Mg (Z = 12).
c.
S (Z = 16).
b.
C (Z = 6).
d.
Si (Z = 14).
 

 23. 
What is the electron configuration for nitrogen, atomic number 7?
a.
1s2 2s2 2p3
b.
1s2 2s3 2p2
c.
1s2 2s3 2p1
d.
1s2 2s2 2p2 3s1
 

 24. 
The electron notation for aluminum (atomic number 13) is
a.
1s2 2s2 2p3 3s2 3p3 3d1.
b.
1s2 2s2 2p6 3s2 2d1.
c.
1s2 2s2 2p6 3s2 3p1.
d.
1s2 2s2 2p9.
 

 25. 
If the s and p orbitals of the highest main energy level of an atom are filled with electrons, the atom has a(n)
a.
electron pair.
c.
empty d orbital.
b.
octet.
d.
electron in an excited state.
 



 
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