General Chemistry
Principles & Modern Applications
9th Edition
Petrucci/Harwood/Herring/Madura
Chapter 8
Electrons in Atoms
Dr. Travis D. Fridgen
Memorial University of Newfoundland
© 2007 Pearson Education
Based on the diagram
and equations below
which of the following
statements is true?
c = 
E = h
1. The energy of radio waves are greater than the energy of visible waves.
2. The greater the wavelength, the greater the energy of the light.
3. The energy of ultraviolet waves are greater than the energy of infrared waves.
4. The energy of gamma waves are smaller than the energy of X-Ray waves.
Based on the diagram
and equations below
which of the following
statements is true?
c = 
E = h
1. The energy of radio waves are greater than the energy of visible waves.
2. The greater the wavelength, the greater the energy of the light.
3. The energy of ultraviolet waves are greater than the energy of infrared waves.
4. The energy of gamma waves are smaller than the energy of X-Ray waves.
Based on the diagram
and the equation
below which of the
following statements is
true?
c = 
1. The frequencies of radio waves are greater than the frequencies of visible waves.
2. The frequencies of ultraviolet waves are greater than the frequencies of infrared
waves.
3. The frequencies of gamma waves are smaller than the frequencies of X-ray
waves.
4. None of the above statements are true.
Based on the diagram
and the equation
below which of the
following statements is
true?
c = 
1. The frequencies of radio waves are greater than the frequencies of visible waves.
2. The frequencies of ultraviolet waves are greater than the frequencies of infrared
waves.
3. The frequencies of gamma waves are smaller than the frequencies of X-ray
waves.
4. None of the above statements are true.
To the right is a schematic of the
apparatus used for photoelectric
effect measurements where 0 is
called the threshold frequency.
True or false, if light of a higher
frequency is shone on the metal
a larger current will be
measured?
1. True
2. False
To the right is a schematic of the
apparatus used for photoelectric
effect measurements where 0 is
called the threshold frequency.
True or false, if light of a higher
frequency is shone on the metal
a larger current will be
measured?
1. True
2. False
Without the use of a calculator,
indicate which of the following
transitions in the hydrogen atom
results in the emission of light of
the greatest energy?
 1
1 
E   2  2 
nf 
 ni
1. n=4 to n=3
2. n=1 to n=2
3. n=3 to n=2
4. n=2 to n=1
5. n=1 to n=3
Without the use of a calculator,
indicate which of the following
transitions in the hydrogen atom
results in the emission of light of
the greatest energy?
 1
1 
E   2  2 
nf 
 ni
1. n=4 to n=3
2. n=1 to n=2
3. n=3 to n=2
4. n=2 to n=1
5. n=1 to n=3
Without the use of a calculator,
indicate which of the following
transitions in the hydrogen atom
results in the emission of light of
the longest wavelength?
 1
1 
E   2  2 
nf 
 ni
1. n=4 to n=3
2. n=1 to n=2
3. n=3 to n=2
4. n=2 to n=1
5. n=1 to n=3
Without the use of a calculator,
indicate which of the following
transitions in the hydrogen atom
results in the emission of light of
the longest wavelength?
 1
1 
E   2  2 
nf 
 ni
1. n=4 to n=3
2. n=1 to n=2
3. n=3 to n=2
4. n=2 to n=1
5. n=1 to n=3
The best experimental evidence for the existence of discrete (quantized)
energy levels in an atom comes from
1. Diffraction of
electrons by
crystals.
3. Atomic Line Spectra.
2. Dispersion of light by matter.
4. The Stern-Gerlach
Experiment
The best experimental evidence for the existence of discrete (quantized)
energy levels in an atom comes from
1. Diffraction of
electrons by
crystals.
3. Atomic Line Spectra.
2. Dispersion of light by matter.
4. The Stern-Gerlach
Experiment
Which of the following orbital designations is impossible?
1. n=2, l = 0, ml = 0
2. n=3, l = 0, ml = 0
3. n=3, l = 1, ml = 1
4. n=3, l = 2, ml = -1
5. n=3, l = 3, ml = -3
Which of the following orbital designations is impossible?
1. n=2, l = 0, ml = 0
2. n=3, l = 0, ml = 0
3. n=3, l = 1, ml = 1
4. n=3, l = 2, ml = -1
5. n=3, l = 3, ml = -3
Which of the following sets of quantum numbers
is not matched with the orbital designation.
1. n=1, l = 0: a 1s orbital
2. n=2, l = 0: a 2p orbital
3. n=3, l = 0: a 3s orbital
4. n=3, l = 1: a 3p orbital
5. n=3, l = 2: a 3d orbital
Which of the following sets of quantum numbers
is not matched with the orbital designation.
1. n=1, l = 0: a 1s orbital
2. n=2, l = 0: a 2p orbital
3. n=3, l = 0: a 3s orbital
4. n=3, l = 1: a 3p orbital
5. n=3, l = 2: a 3d orbital
In the hydrogen atom, the orbitals in a
given shell are degenerate. For
multiple electron atoms what is the
main reason for the splitting of, say,
the 2s and 2p orbital energies?
Hydrogen atom
1. Higher nuclear charge.
2. The greater distance of the
electrons from the nucleus.
3. Penetration of the nucleus by the 2s electron.
4. The presence of an angular node for the 2p orbital.
Many electron
atom
In the hydrogen atom, the orbitals in a
given shell are degenerate. For
multiple electron atoms what is the
main reason for the splitting of, say,
the 2s and 2p orbital energies?
Hydrogen atom
1. Higher nuclear charge.
2. The greater distance of the
electrons from the nucleus.
3. Penetration of the nucleus by the 2s electron.
4. The presence of an angular node for the 2p orbital.
Many electron
atom
Below are radial probability distributions for the 1s, 2s, 2p, 3s and 3p orbitals
in random order. Which one is the radial probability distribution for the 3s
orbital?
1.
2.
4.
3.
5.
Below are radial probability distributions for the 1s, 2s, 2p, 3s and 3p orbitals
in random order. Which one is the radial probability distribution for the 3s
orbital?
1.
2.
4.
3.
5.
Below are radial probability distributions for the 2s, 2p, 3s, 3p and 3d orbitals
in random order. Which one is the radial probability distribution for the 3d
orbital?
1.
2.
4.
3.
5.
Below are radial probability distributions for the 2s, 2p, 3s, 3p and 3d orbitals
in random order. Which one is the radial probability distribution for the 3d
orbital?
1.
2.
4.
3.
5.
Which of numbers in the periodic table below corresponds to the group of
elements in which the 2p orbitals are being filled.
3
1
4
2
5
Which of numbers in the periodic table below corresponds to the group of
elements in which the 2p orbitals are being filled.
3
1
4
2
5
Which of numbers in the periodic table below corresponds to the group of
elements in which the 4d orbitals are being filled.
1
2
3
4
5
Which of numbers in the periodic table below corresponds to the group of
elements in which the 4d orbitals are being filled.
1
2
3
4
5
Which of the following is the condensed electron configuration for chlorine?
1. [Ne]3p7
2. [Ne]3s23p5
3.
[Ne]3s23p6
4. [Ne]3s23d5
5.
[Ne]3s23p33d2
Cl2(g)
Cl2(l)
Which of the following is the condensed electron configuration for chlorine?
1. [Ne]3p7
2. [Ne]3s23p5
3.
[Ne]3s23p6
4. [Ne]3s23d5
5.
[Ne]3s23p33d2
Cl2(g)
Cl2(l)
Which of the following is the condensed electron configuration for bismuth?
[Xe] accounts for 54 electrons.
1. [Xe]6s24f145d106p3
2. [Xe]6s26f146d106p3
3. [Xe]5s24f144d105p3
4. [Xe]6s24f124d106p5
5. [Xe]5s24f124d105p5
Which of the following is the condensed electron configuration for bismuth?
[Xe] accounts for 54 electrons.
1. [Xe]6s24f145d106p3
2. [Xe]6s26f146d106p3
3. [Xe]5s24f144d105p3
4. [Xe]6s24f124d106p5
5. [Xe]5s24f124d105p5
Which of the following is the condensed electron configuration for copper?
[Xe] accounts for 54 electrons.
1. [Ar]3s23d9
2. [Ar]4s22d9
3. [Ar]3s14d10
4. [Ar]4s14d10
5. [Ar]4s13d10
Which of the following is the condensed electron configuration for copper?
[Xe] accounts for 54 electrons.
1. [Ar]3s23d9
2. [Ar]4s22d9
3. [Ar]3s14d10
4. [Ar]4s14d10
5. [Ar]4s13d10