Transcript Periodic trends

Modern Chemistry
Chapter 5
The Periodic Law
Sections 1-3
History of the Periodic Table
Electron Configurations and the Periodic Table
Electron Configurations and Periodic Properties
Chapter 5 Section 1 History of the
Periodic Table pages 133-137
1
Section 3
Electron
Configurations and
periodic properties
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
150-164
2
Section 3 Vocabulary
Atomic radius
Ion
Ionization
Ionization Energy
Electron affinity
Cation
Anion
Valence electrons
Electronegativity
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
150-164
3
p. 150
Atomic Radii
• One half the distance between the nuclei
of identical atoms bonded together
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
150-164
4
Atomic Radii
• Period Trend 
– Atomic radii decreases across a period
– Electrons are added to the s and p in the
same energy level
– Protons are added to the nucleus
– The nucleus is stronger and pulls in the
electrons making the atom smaller
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
150-164
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Atomic Radii
• Group Trend 
– Atomic radii increases down a group
– Exeption Al to Ga in group 13
– Electrons exist in higher energy levels
further from the nucleus
Practice on page 152
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
150-164
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p. 151*
Atomic radius image
Chapter 55 Section
Section 11 History
History of
of the
the
Chapter
Periodic Table
Table pages
pages 133-137
133-137
Periodic
7
Ionization Energy
• Ion: an atom or group of bonded atoms
that has a positive or negative charge
• Ionization: any process that results in
the formation of an ion
• Ionization energy: The energy required
to remove one electron from a neutral
atom.
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
150-164
8
ion animation
Chapter 55 Section
Section 11 History
History of
of the
the
Chapter
Periodic Table
Table pages
pages 133-137
133-137
Periodic
9
Ionization Energy
• First ionization energy = IE1 (energy to
remove one electron)
• Diagram on Page 153 and 154
• A + energy  A+ + e-
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
150-164
10
Ionizaiton Energy Comic
p. ##
Chapter 55 Section
Section 11 History
History of
of the
the
Chapter
Periodic Table
Table pages
pages 133-137
133-137
Periodic
11
Ionization energy
animation
Chapter 55 Section
Section 11 History
History of
of the
the
Chapter
Periodic Table
Table pages
pages 133-137
133-137
Periodic
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p. 154
Ionization energy vs. atomic number graph
Chapter 55 Section
Section 11 History
History of
of the
the
Chapter
Periodic Table
Table pages
pages 133-137
133-137
Periodic
13
Ionization Energy
• Period Trend 
– IE increases across a period
– Increased nuclear charge holds e- thighter
– Elements with low IE lose e- easily
– Elements with high IE do not lose e– Generally nonmetals have higher IE than
metals
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
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Ionization Energy
• Group Trend 
– IE decreases down a group
– An electron is removed from higher energy
levels further from the nucleus
– In elements with many electron, the inner
electrons in lower energy levels shield the
outer electrons in the higher energy levels
from the attraction of the nucleus
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
150-164
15
Ionization energy image
Decrease
Ionization Energy
p. 153*
Increase
Chapter 55 Section
Section 11 History
History of
of the
the
Chapter
Periodic Table
Table pages
pages 133-137
133-137
Periodic
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Ionization Energy
• Removing electrons from positive ions
– More than one electron can be removed
from an atom
– Second ionization energy = IE2
– IE2 is higher than IE1
– Because few electrons remain to shield the
outer electrons from the nucleus
– Table on page 155
Practice page 156
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
150-164
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p. 55
1st- 5th Ionization energy chart
Chapter 55 Section
Section 11 History
History of
of the
the
Chapter
Periodic Table
Table pages
pages 133-137
133-137
Periodic
18
Electron Affinity
• The energy change that occurs when an
electron is acquired by a neutral atom
A + e-  A- + energy Energy is released
negative number
or
A + e- + energy Energy is absorbed
 Apositive number
– Positive or less negative EA won’t likely
gain electrons
– More negative EA will gain electrons easily
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
150-164
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Electron Affinity
animation
Chapter 55 Section
Section 11 History
History of
of the
the
Chapter
Periodic Table
Table pages
pages 133-137
133-137
Periodic
20
Electron affinity
• Period Trend 
– EA increases across the period (more neg.)
– Exception between group 14 and 16
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
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Electron affinity
• Group Trend 
– EA decreases down a group (less neg.)
– An increase in protons increases EA but an
increase in radius decreases EA
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
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Electron Affinity image
Decrease
Electron Affinity
p. 157*
Increase
Chapter 55 Section
Section 11 History
History of
of the
the
Chapter
Periodic Table
Table pages
pages 133-137
133-137
Periodic
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Electron affinity
• Adding electrons to negative ions
• More difficult to add a second eletron
• All second EA are positive
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
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Properties
pages
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Ionic Radii
• Positive Ions
– Cation
– Loss of electron
– Smaller electron cloud; loss of highest
energy level
– Electrons are drawn closer to the nucleus
Na
Na+
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
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Properties
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Ionic Radii
• Negative ion
– Anions
– Gaining of electrons
– The electron cloud spreads out because of
the repeling of electrons
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
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ions
Cation - positive
Anion - negative
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
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Ionic Radii
• Period Trend 
– Ionic radii decreases across a period
– As protons increase the electrons are
pulled in
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
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Ionic Radii
• Group Trend 
– Ionic Radii increases down a group
– More electrons in higher energy levels
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
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p. 159*
Ionic RADIUS Image
Chapter 55 Section
Section 11 History
History of
of the
the
Chapter
Periodic Table
Table pages
pages 133-137
133-137
Periodic
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Valence electrons
• Electrons available to be lost, gained or
shared in the formation of compounds.
• Located in the incompletely filled main
energy level
• For main group elements – outer s & p
sublevels
Chapter
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1 History
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3 Periodic
Periodic
Table
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Properties
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Valence electrons
animation
p. ##
Chapter 55 Section
Section 11 History
History of
of the
the
Chapter
Periodic Table
Table pages
pages 133-137
133-137
Periodic
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electronegativity
• A measure of an atom in a compound to
attract electrons from another atom in
the compound
• Linus Pauling devised a scale from 0-4.
• Fluorine is the most electronegative EN
= 4.0
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
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p.161
Electronegativities
Chapter 55 Section
Section 11 History
History of
of the
the
Chapter
Periodic Table
Table pages
pages 133-137
133-137
Periodic
34
electronegativity
animation
Chapter 55 Section
Section 11 History
History of
of the
the
Chapter
Periodic Table
Table pages
pages 133-137
133-137
Periodic
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electronegativity
• Period Trend 
– EN increases across a period
– There are exceptions.
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
150-164
36
electronegativity
• Group Trend 
– EN decreases down a group
Practice Page 162
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
150-164
37
Electronegativity
Decrease
Electronegativity
p. 160*
Increase
Chapter 55 Section
Section 11 History
History of
of the
the
Chapter
Periodic Table
Table pages
pages 133-137
133-137
Periodic
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Periodic Properties of
the d and F block elements
• Many exceptions in atomic radii, IE,
and EN
• Most d block elements from 2+ ions
• Group 3 from 3+ ions
• Copper forms 1+ and 2+ ions
• Iron forms 2+ and 3+ ions
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
150-164
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Summary of trends Image
Chapter 55 Section
Section 11 History
History of
of the
the
Chapter
Periodic Table
Table pages
pages 133-137
133-137
Periodic
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Section 3 Homework
Chapter
5 Section
1 History
of the
Chapter
5 Section
3 Periodic
Periodic
Table
pages
133-137
Properties
pages
150-164
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