Chemistry 6/e
Steven S. Zumdahl
and Susan A. Zumdahl
Chapter 7:
ATOMIC
STRUCTURE &
PERIODICITY
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1
Atomic Structure & Periodicity
• Electromagnetic
Radiation
• React 1
• The Nature of Matter
• The Atomic Spectrum
of Hydrogen
• React 2
• The Bohr Model
• React 3 • 4 • 5
• The Quantum
Mechanical Model of
the Atom
• Orbital Shapes and
Energies
• React 6 • 7 • 8
• Periodic Trends in
Atomic Properties
• React 9 • 10 • 11 • 12
• React 13 • 14 • 15 • 16
• React 17 • 18 • 19 • 20
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2
Rutherford’s Model of the Atom
What does Rutherford’s atom “look like”?
We want models to explain our
observations.
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3
Rutherford’s Model of the Atom
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4
Electromagnetic Radiation
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5
Flame Tests
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6
Fireworks
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7
Questions to Consider
Why do the different chemicals give us
different colors?
Why do we get colors at all?
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8
Classification of Electromagnetic Radiation
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9
Draw three waves with relative
wavelengths of 1:2:4.
Compare the frequencies and energies of
these wavelengths.
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10
The Nature
of Waves
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11
Electromagnetic Wave
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12
The Nature of Matter
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13
Photoelectric Effect
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14
The Atomic Spectrum of
Hydrogen
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15
Refraction of White Light and
Hydrogen Line Spectrum
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16
Explain the hydrogen emission spectrum.
Why is it significant that the color emitted
is not white?
How does the emission spectrum support
the idea of quantized energy levels?
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17
The Bohr Model
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18
Determine the color of light emitted when
an excited electron in the hydrogen atom
falls from:
I. n = 5 to n = 2
II. n = 4 to n = 2
III. n = 3 to n = 2
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19
Electronic Transitions in the Bohr Model for
the Hydrogen Atom
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20
There are an infinite number of allowed
transitions in the hydrogen atom.
Why don’t we see more lines in the
emission spectrum for hydrogen?
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21
Does a gamma ray of wavelength
1.0 x 10-8 cm have enough energy to
remove an electron from a hydrogen
atom?
Support your answer with calculations.
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22
Let’s Think About It
What is the energy associated with a
gamma ray with a wavelength of
1.0 x 10-8 cm?
How much energy does it take to remove
an electron from a hydrogen atom?
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23
The Quantum Mechanical
Model of the Atom
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24
Probability
Distribution for the
1s Wave Function
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25
Radial Probability Distribution
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26
Orbital Shapes and Energies
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27
Two
Representations of
the Hydrogen 1s,
2s, and 3s Orbitals
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28
The Radial
Probability
Distribution for the
3s, 3p, and 3d
Orbitals
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29
The Boundary Surface Representations of
All Three 2p Orbitals
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30
The Boundary Surfaces of
All of the 3d Orbitals
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31
Representation of the 4f Orbitals in Terms of
Their Boundary Surfaces
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32
A Comparison of the Radial Probability
Distributions of the 2s and 2p Orbitals
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33
The Radial Probability Distribution for the
3s, 3p, and 3d Orbitals
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34
Sketch a general orbital-level diagram for
atoms other than hydrogen.
Explain why it differs
from hydrogen.
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35
Explain how you can use the periodic
table to determine the order in which
orbitals fill in polyelectronic atoms (so that
you do not have to memorize it).
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36
The Orbitals Being Filled for Elements in
Various Parts of the Periodic Table
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37
Determine the expected electron
configurations for each of the following:
• S
• Ba
• Ni2+
• Eu
• Ti+
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38
Periodic Trends in Atomic
Properties
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39
Which is larger, the hydrogen 1s orbital,
or the Li 1s orbital? Why?
Which is lower in energy, the hydrogen 1s
orbital, or the Li 1s orbital? Why?
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40
Which atom would require more energy to
remove an electron, Na or Cl? Why?
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41
Which atom would require more energy to
remove an electron, Li or Cs? Why?
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42
What is the general trend for ionization
energy across rows and down columns on
the periodic table?
Understand this trend; do not merely
memorize it.
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43
Which should be the larger atom,
Na or Cl? Why?
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44
Which should be the larger atom,
Li or Cs? Why?
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45
What is the general trend for atomic size
across rows and down columns on the
periodic table?
Explain this trend.
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46
Atomic Radii for
Selected Atoms
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47
Arrange the elements oxygen, fluorine,
and sulfur according to increasing
• Ionization energy
• Atomic size
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48
The Values of First Ionization Energy for the
Elements in the First Six Periods
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49
Explain why the graph of ionization
energy versus atomic number (across a
row) is not linear.
Where are the exceptions?
Why are there exceptions?
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50
The ionization energy of the magnesium atom requires 735
kJ/mol. Which of the following is the most accurate
statement about the second ionization energy of Mg?
I.
It is less than 735 kJ/mol because Mg wants to lose
the second electron to have the same electron
configuration as Ne.
II.
It is equal to 735 kJ/mol because both electrons are
being taken from the 3s orbital.
III.
It is greater than 735 kJ/mol because the second
electron is being taken from a positive ion.
IV.
Energy is released when the second electron comes
off because the Mg atom wants to lose the second
electron to have the same electron configuration as
Ne.
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51
Relative Ionization Energies for Elements
X
Y
First
170
200
Second
350
400
Third
1800
3500
Fourth
2500
5000
Identify the elements. Why can there be more
than one answer?
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52
Which has the larger second ionization
energy, lithium or beryllium?
Why?
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53
General decrease
Successive Ionization Energies in Kilojoules
per Mole for the Elements in Period 3
Element
I1
I2
I3
I4
I5
I6
I7
Na
495
4560
Mg
735
1445
7730
Core electrons*
Al
580
1815
2740
11,600
Si
780
1575
3220
4350
16,100
P
1060
1890
2905
4950
6270
21,200
S
1005
2260
3375
4565
6950
8490
27,000
Cl
1255
2295
3850
5160
6560
9360
11,000
Ar
1527
2665
3945
5770
7230
8780
12,000
* Note the large jump in ionization energy in going from removal of valence electrons to
removal of core electrons.
General increase
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54