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Chapter 5 Section 1 History of the Periodic Table pages 133-137
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Modern ChemistryChapter 5
The Periodic Law
Sections 1-3History of the Periodic Table
Electron Configurations and the Periodic Table
Electron Configurations and Periodic Properties
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Chapter 5 Section 1 History of the Periodic Table pages 133-137
2Chapter 5 Section 3 Periodic Properties pages 150-164
Electron Configurations and periodic properties
Section 3
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Chapter 5 Section 1 History of the Periodic Table pages 133-137
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Sect
ion 3
Voca
bula
ryAtomic radiusIonIonizationIonization EnergyElectron affinityCationAnionValence electronsElectronegativity
Chapter 5 Section 3 Periodic Properties pages 150-164
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Atomic Radii• One half the distance between the nuclei
of identical atoms bonded together
Chapter 5 Section 3 Periodic Properties pages 150-164p.
150
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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 3 Periodic 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 3 Periodic Properties pages 150-164
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Atomic radius imagep.
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*
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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 3 Periodic Properties pages 150-164
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Chapter 5 Section 1 History of the Periodic Table pages 133-137
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ion
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Ionization Energy • First ionization energy = IE1 (energy
to remove one electron)• Diagram on Page 153 and 154• A + energy A+ + e-
Chapter 5 Section 3 Periodic Properties pages 150-164
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Ion
izait
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nerg
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icp.
## Chapter 5 Section 1 History of the
Periodic Table pages 133-137
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Ion
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nerg
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nim
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Ionization energy vs. atomic number graph
p. 1
54 Chapter 5 Section 1 History of the Periodic Table pages 133-137
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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 3 Periodic Properties pages 150-164
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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 3 Periodic Properties pages 150-164
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Ionization energy imagep.
153
*
Chapter 5 Section 1 History of the Periodic Table pages 133-137
Dec
reas
e
Increase
Ionization Energy
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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 3 Periodic Properties pages 150-164
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1st- 5th Ionization energy chartp.
55 Chapter 5 Section 1 History of the
Periodic Table pages 133-137
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Electron Affinity • The energy change that occurs when
an electron is acquired by a neutral atom
A + e- A- + energy orA + e- + energy A-
– Positive or less negative EA won’t likely gain electrons
– More negative EA will gain electrons easily Chapter 5 Section 3 Periodic
Properties pages 150-164
Energy is released negative number
Energy is absorbed positive number
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Ele
ctro
n A
ffinit
y a
nim
ati
on
Chapter 5 Section 1 History of the Periodic Table pages 133-137
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Electron affinity • Period Trend
– EA increases across the period (more neg.)
– Exception between group 14 and 16
Chapter 5 Section 3 Periodic Properties pages 150-164
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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 3 Periodic Properties pages 150-164
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Electron Affinity imagep.
157
*
Chapter 5 Section 1 History of the Periodic Table pages 133-137
Dec
reas
e
Increase
Electron Affinity
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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 3 Periodic Properties pages 150-164
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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
nucleusNa Na+
Chapter 5 Section 3 Periodic Properties pages 150-164
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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 3 Periodic Properties pages 150-164
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ions Cation - positive Anion - negative
Chapter 5 Section 3 Periodic Properties pages 150-164
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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 3 Periodic Properties pages 150-164
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Ionic Radii • Group Trend
– Ionic Radii increases down a group– More electrons in higher energy levels
Chapter 5 Section 3 Periodic Properties pages 150-164
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Ionic RADIUS Imagep.
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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 5 Section 3 Periodic Properties pages 150-164
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Vale
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ele
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an
imati
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p. #
# Chapter 5 Section 1 History of the Periodic Table pages 133-137
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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 3 Periodic Properties pages 150-164
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Electronegativities
p.16
1 Chapter 5 Section 1 History of the Periodic Table pages 133-137
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ele
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electronegativity• Period Trend
– EN increases across a period– There are exceptions.
Chapter 5 Section 3 Periodic Properties pages 150-164
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electronegativity• Group Trend
– EN decreases down a group
Practice Page 162
Chapter 5 Section 3 Periodic Properties pages 150-164
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Electronegativityp.
160
*
Chapter 5 Section 1 History of the Periodic Table pages 133-137
Dec
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Increase
Electronegativity
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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 3 Periodic Properties pages 150-164
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Sum
mary
of
tren
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Section 3 Homework
Chapter 5 Section 3 Periodic Properties pages 150-164