Periodic Definitions & Trends Table of Contents Lecture/Lab/Activity Date Pg# 14. The History of...
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![Page 1: Periodic Definitions & Trends Table of Contents Lecture/Lab/Activity Date Pg# 14. The History of Atomic Models 9/14/10 31 15. Structure of the Atom 9/15/10.](https://reader035.fdocuments.us/reader035/viewer/2022070413/5697bfc71a28abf838ca7ed7/html5/thumbnails/1.jpg)
Periodic Definitions & Trends
Table of ContentsLecture/Lab/Activity Date Pg#
14. The History of Atomic Models 9/14/10 3115. Structure of the Atom 9/15/10 3516. Isotopes 9/16/10 3717. Beanium Lab 9/17/10 18. Electron Probability Lab 9/20/10 3919. Electron Configuration 9/21/10 4120. Orbital Diagrams 9/22/10 4321. Electron Config Practice 9/23/10 4522. The Periodic Table 9/24/10 4723. Periodic Def & Trends 9/27/10 49
Objective:The student will label a periodic table to identify and explain periodic trends including atomic radius, electronegativity and ionization energy.
Agenda:The Periodic Table– Lecture
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How to read the Periodic Table
6
CCarbon
12.011
Atomic Number
Elemental Symbol
Elemental Name
Atomic Mass
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Definitions
• Atomic Number• Is the same as the number of protons in an element.• If this number changes the element name must change
as well.• Atomic # = # of protons = # of electrons
• Atomic Mass• Is a weighted average of all the atoms in a naturally
occurring sample of an element (mass & relative abundance)
• 1 amu – one tweflth the mass of a carbon-12 atom
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Calculating Neutrons
• Round the Atomic Mass Atomic Mass
- Atomic Number
(difference = # neutrons)
6
C
Carbon
12.011
Example:
Atomic Mass = 12
Atomic # = 6
Difference = 6
Difference = # neutrons
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Calculating Atomic Mass
• 3 values required:• # of stable isotopes of an element
• The mass of each isotope
• The natural percent abundance of each isotope
• ? If Element X has 2 naturally occurring isotopes, what is its atomic mass? Mass 1 = 10.012 amu and has a relative abundance of 19.91 % , Mass 2 = 11.009 amu and has a relative abundance of 80.09%
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Periodic Law
• When elements are arranged in order of increasing atomic #, elements with similar properties appear at regular intervals.
0
50
100
150
200
250
0 5 10 15 20
Ato
mic
Ra
diu
s (
pm
)
Atomic Number
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Chemical Reactivity
• Families• Similar valence e- within a group result in similar
chemical properties
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Periodic Trends
• Atomic Radius• size of atom• Increases to the LEFT and DOWN
1
2
3
4 5
6
7
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Atomic Radius
• Why larger going down?• Higher energy levels have larger orbitals
• Shielding - core e- block the attraction between the nucleus and the valence e-
• Why smaller to the right? • Increased nuclear charge without additional
shielding pulls e- in tighter
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Periodic Trends
• First Ionization Energy• Energy required to remove one e- from a
neutral atom.• Increases going UP and to the RIGHT
1
2
3
4 5
6
7
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Ionization Energy
• Why opposite of atomic radius?
• In small atoms, e- are close to the nucleus where the attraction is stronger
• Why small jumps within each group?
• Stable e- configurations don’t want to lose e-
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Electronegativity
• The attraction an element has on a shared paired of electrons
1
2
3
4 5
6
7
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Periodic Trends
• Melting/Boiling Point• Highest in the middle of a period.
1
2
3
4 5
6
7
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Ionic Radius
• Cations (+)• lose e-• smaller
• Anions (–)• gain e-• larger
© 2002 Prentice-Hall, Inc.