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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. Section 3. Electron Configurations and periodic properties. - PowerPoint PPT Presentation
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Chapter 5 Section 1 History of the Periodic Table pages 133-137
1
Modern ChemistryChapter 5
The Periodic Law
Sections 1-3History 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
2Chapter 5 Section 3 Periodic Properties pages 150-164
Electron Configurations and periodic properties
Section 3
Chapter 5 Section 1 History of the Periodic Table pages 133-137
3
Sect
ion 3
Voca
bula
ryAtomic radiusIonIonizationIonization EnergyElectron affinityCationAnionValence electronsElectronegativity
Chapter 5 Section 3 Periodic Properties pages 150-164
Chapter 5 Section 1 History of the Periodic Table pages 133-137
4
Atomic Radii• One half the distance between the nuclei
of identical atoms bonded together
Chapter 5 Section 3 Periodic Properties pages 150-164p.
150
Chapter 5 Section 1 History of the Periodic Table pages 133-137
5
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
Chapter 5 Section 1 History of the Periodic Table pages 133-137
6
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
Chapter 5 Section 1 History of the Periodic Table pages 133-137
7
Atomic radius imagep.
151
*
Chapter 5 Section 1 History of the Periodic Table pages 133-137
Chapter 5 Section 1 History of the Periodic Table pages 133-137
8
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
Chapter 5 Section 1 History of the Periodic Table pages 133-137
9
ion
anim
ati
on
Chapter 5 Section 1 History of the Periodic Table pages 133-137
Chapter 5 Section 1 History of the Periodic Table pages 133-137
10
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
Chapter 5 Section 1 History of the Periodic Table pages 133-137
11
Ion
izait
on E
nerg
y C
om
icp.
## Chapter 5 Section 1 History of the
Periodic Table pages 133-137
Chapter 5 Section 1 History of the Periodic Table pages 133-137
12
Ion
izati
on e
nerg
y a
nim
ati
on
Chapter 5 Section 1 History of the Periodic Table pages 133-137
Chapter 5 Section 1 History of the Periodic Table pages 133-137
13
Ionization energy vs. atomic number graph
p. 1
54 Chapter 5 Section 1 History of the Periodic Table pages 133-137
Chapter 5 Section 1 History of the Periodic Table pages 133-137
14
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
Chapter 5 Section 1 History of the Periodic Table pages 133-137
15
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
Chapter 5 Section 1 History of the Periodic Table pages 133-137
16
Ionization energy imagep.
153
*
Chapter 5 Section 1 History of the Periodic Table pages 133-137
Dec
reas
e
Increase
Ionization Energy
Chapter 5 Section 1 History of the Periodic Table pages 133-137
17
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
Chapter 5 Section 1 History of the Periodic Table pages 133-137
18
1st- 5th Ionization energy chartp.
55 Chapter 5 Section 1 History of the
Periodic Table pages 133-137
Chapter 5 Section 1 History of the Periodic Table pages 133-137
19
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
Chapter 5 Section 1 History of the Periodic Table pages 133-137
20
Ele
ctro
n A
ffinit
y a
nim
ati
on
Chapter 5 Section 1 History of the Periodic Table pages 133-137
Chapter 5 Section 1 History of the Periodic Table pages 133-137
21
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
Chapter 5 Section 1 History of the Periodic Table pages 133-137
22
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
Chapter 5 Section 1 History of the Periodic Table pages 133-137
23
Electron Affinity imagep.
157
*
Chapter 5 Section 1 History of the Periodic Table pages 133-137
Dec
reas
e
Increase
Electron Affinity
Chapter 5 Section 1 History of the Periodic Table pages 133-137
24
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
Chapter 5 Section 1 History of the Periodic Table pages 133-137
25
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
Chapter 5 Section 1 History of the Periodic Table pages 133-137
26
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
Chapter 5 Section 1 History of the Periodic Table pages 133-137
27
ions Cation - positive Anion - negative
Chapter 5 Section 3 Periodic Properties pages 150-164
Chapter 5 Section 1 History of the Periodic Table pages 133-137
28
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
Chapter 5 Section 1 History of the Periodic Table pages 133-137
29
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
Chapter 5 Section 1 History of the Periodic Table pages 133-137
30
Ionic RADIUS Imagep.
159
*
Chapter 5 Section 1 History of the Periodic Table pages 133-137
Chapter 5 Section 1 History of the Periodic Table pages 133-137
31
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
Chapter 5 Section 1 History of the Periodic Table pages 133-137
32
Vale
nce
ele
ctro
ns
an
imati
on
p. #
# Chapter 5 Section 1 History of the Periodic Table pages 133-137
Chapter 5 Section 1 History of the Periodic Table pages 133-137
33
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
Chapter 5 Section 1 History of the Periodic Table pages 133-137
34
Electronegativities
p.16
1 Chapter 5 Section 1 History of the Periodic Table pages 133-137
Chapter 5 Section 1 History of the Periodic Table pages 133-137
35
ele
ctro
negati
vit
y a
nim
ati
on
Chapter 5 Section 1 History of the Periodic Table pages 133-137
Chapter 5 Section 1 History of the Periodic Table pages 133-137
36
electronegativity• Period Trend
– EN increases across a period– There are exceptions.
Chapter 5 Section 3 Periodic Properties pages 150-164
Chapter 5 Section 1 History of the Periodic Table pages 133-137
37
electronegativity• Group Trend
– EN decreases down a group
Practice Page 162
Chapter 5 Section 3 Periodic Properties pages 150-164
Chapter 5 Section 1 History of the Periodic Table pages 133-137
38
Electronegativityp.
160
*
Chapter 5 Section 1 History of the Periodic Table pages 133-137
Dec
reas
e
Increase
Electronegativity
Chapter 5 Section 1 History of the Periodic Table pages 133-137
39
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
Chapter 5 Section 1 History of the Periodic Table pages 133-137
40
Sum
mary
of
tren
ds
Imag
e
Chapter 5 Section 1 History of the Periodic Table pages 133-137
Chapter 5 Section 1 History of the Periodic Table pages 133-137
41
Section 3 Homework
Chapter 5 Section 3 Periodic Properties pages 150-164
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