Name: 
 

C4 Arrangement of e- in Atoms


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

1. 
The product of the frequency and the wavelength of a wave equals the
a.
number of waves passing a  point in a second.
b.
speed of the wave.
c.
distance between wave crests.
d.
time for one full wave to pass.
 

2. 
For electromagnetic radiation, c (the speed of light) equals
a.
frequency minus wavelength.
c.
frequency divided by wavelength.
b.
frequency plus wavelength.
d.
frequency times wavelength.
 

3. 
As it travels through space, electromagnetic radiation
a.
exhibits wavelike behavior.
c.
varies in speed.
b.
loses energy.
d.
releases photons.
 

4. 
A quantum of electromagnetic energy is called a(n)
a.
photon.
c.
excited atom.
b.
electron.
d.
orbital.
 

5. 
The wave model of light did not explain
a.
the frequency of light.
c.
interference.
b.
the continuous spectrum.
d.
the photoelectric effect.
 

6. 
Planck's constant
a.
depends on the frequency of the radiation.
b.
depends on the mass of the radiation.
c.
depends on the wavelength of the radiation.
d.
is the same for all forms of radiation.
 

7. 
When the pink-colored light of glowing hydrogen gas passes through a prism, it is possible to see
a.
all the colors of the rainbow.
c.
four lines of different colors.
b.
only lavender-colored lines.
d.
black light.
 

8. 
Bohr's model of the atom works best in explaining
a.
the spectra of the first ten elements.
b.
only the spectrum of hydrogen.
c.
only the spectra of atoms with electrons in an s orbital.
d.
the entire visible spectra of atoms.
 

9. 
The drop of an electron from a high energy level to the ground state in a hydrogen atom would be most closely associated with
a.
long-wavelength radiation.
c.
infrared radiation.
b.
low-frequency radiation.
d.
high-frequency radiation.
 

10. 
The electron in a hydrogen atom has its lowest total energy when the electron is in its
a.
neutral state.
c.
ground state.
b.
excited state.
d.
quantum state.
 
 
2007chapter4_files/i0120000.jpg
 

11. 
According to Bohr, electrons cannot reside at ____ in the figure above.
a.
point A
c.
point C
b.
point B
d.
point D
 

12. 
The French scientist Louis de Broglie believed
a.
electrons could have a dual wave-particle nature.
b.
light waves did not have a dual wave-particle nature.
c.
the natures of light and quantized electron orbits were not similar.
d.
Bohr's model of the hydrogen atom was completely correct.
 

13. 
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.
 

14. 
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.
 

15. 
A three-dimensional region around a nucleus where an electron may be found is called a(n)
a.
spectral line.
c.
orbital.
b.
electron path.
d.
orbit.
 

16. 
Quantum numbers are sets of numbers that describe the properties of
a.
the atomic nucleus.
c.
atoms.
b.
atomic orbitals.
d.
molecules.
 

17. 
The main energy levels of an atom are indicated by the
a.
orbital quantum numbers.
c.
spin quantum numbers.
b.
magnetic quantum numbers.
d.
principal quantum numbers.
 

18. 
The possible values of an electron's spin quantum number are
a.
–1, 0, or 1.
c.
+1 or –1.
b.
2007chapter4_files/i0200000.jpg
d.
0 or 1.
 

19. 
The number of sublevels within each energy level of an atom is equal to the value of the
a.
principal quantum number.
c.
magnetic quantum number.
b.
angular momentum quantum number.
d.
spin quantum number.
 

20. 
What values can the angular momentum quantum number have when n = 2?
a.
2007chapter4_files/i0220000.jpg
c.
0, 1, 2
b.
2007chapter4_files/i0220001.jpg
d.
0, 1
 

21. 
A spherical electron cloud surrounding an atomic nucleus would best represent
a.
an s orbital.
c.
a combination of px and py orbitals.
b.
a px orbital.
d.
a combination of an s and a px orbital.
 

22. 
How many orientations can an s orbital have about the nucleus?
a.
1
c.
3
b.
2
d.
5
 

23. 
How many electrons are needed to fill the third main energy level if it already contains 8 electrons?
a.
0
c.
10
b.
8
d.
22
 

24. 
At n = 1, the total number of electrons that could be found is
a.
1.
c.
6.
b.
2.
d.
18.
 

25. 
The statement that an electron occupies the lowest available energy orbital is
a.
Hund's rule.
c.
Bohr's law.
b.
the Aufbau principle.
d.
the Pauli exclusion principle.
 

26. 
"Orbitals of equal energy are each occupied by one electron before any is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin" is a statement of
a.
the Pauli exclusion principle.
c.
the quantum effect.
b.
the Aufbau principle.
d.
Hund's rule.
 

27. 
Which of the following rules requires that each of the p orbitals at a particular energy level receive one electron before any of them can have two electrons?
a.
Hund's rule
c.
the Aufbau principle
b.
the Pauli exclusion principle
d.
the quantum rule
 

28. 
Two electrons in the 1s orbital must have different spin quantum numbers to satisfy
a.
Hund's rule.
c.
the Pauli exclusion principle.
b.
the magnetic rule.
d.
the Aufbau principle.
 

29. 
The atomic sublevel with the next highest energy after 4p is
a.
4d.
c.
5p.
b.
4f.
d.
5s.
 

30. 
In the electron configuration for scandium (atomic number 21), what is the notation for the three highest-energy electrons?
a.
3d1 4s2
c.
3d3
b.
4s3
d.
4s2 4p1
 

31. 
Both copper (atomic number 29) and chromium (atomic number 24) appear to break the pattern in the order of filling the 3d and 4s orbitals. This change in pattern is expressed by
a.
an increase in the number of electrons in both the 3d and 4s orbitals.
b.
a reduction in the number of electrons in both the 3d and 4s orbitals.
c.
a reduction in the number of electrons in the 3d orbital and an increase in the 4s orbital.
d.
a reduction in the number of electrons in the 4s orbital and an increase in the 3d orbital.
 

32. 
In the ground state, the 3d and 4s sublevels of the chromium atom (atomic number 24) may be represented as
a.
3d6 4s1.
c.
3d5 4s1.
b.
3d4 4s2.
d.
4s2 3d4.
 

33. 
The electron configuration for the carbon atom (C) is 1s2 2s2 2p2. The atomic number of carbon is
a.
3.
c.
11.
b.
6.
d.
12.
 

34. 
The electron notation for aluminum (atomic number 13) is
a.
1s2 2s2 2p3 3s2 3p3 3d1.
c.
1s2 2s2 2p6 3s2 3p1.
b.
1s2 2s2 2p6 3s2 2d1.
d.
1s2 2s2 2p9.
 

35. 
If an element has an octet of electrons in its highest main energy level, there are ____ electrons in this level.
a.
2
c.
10
b.
8
d.
32
 



 
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