Periodic Table and
Trends
Explore
the origins of the periodic table while learning the importance of arranging
elements by atomic number. Vividly colored graphics and insightful narration
illustrate how the shape of the periodic table relates to elemental properties.
The description of electron configurations shows the systematic organization of
elements into groups, periods, and blocks. Discussions of trends in properties
such as atomic radii and electronegativity remove the complexities of
periodicity, while revealing the organization of the periodic table.
OUTLINE:
I. Introduction
A. Program Overview
B. The Periodic Table
Organizes the
Elements
II. Atomic Structure Review
III. Historical Steps Leading to the Development of the Periodic Table
A. Early Tables were
Based
on Atomic Mass
1.
Determining Atomic Masses
B. Identifying New Elements Created
a Need
for Organization
C. Dobereiner's Triads
D. Newlands' Octaves
E. Mendeleev - The Father of
the Modern Periodic Table
1.
Mendeleev's Table Allowed Predictions
2.
Problems with Mendeleev's
Table
F. Moseley Determined Atomic
Number
G. The Modern Periodic Table
is Based on Atomic
Number
1.
Periodic Law
IV. The Modern Periodic Table
A. Each Element is Depicted by
Its Symbol
B. Boxes, or Tags, Give Information About
Elements
1.
Atomic Number
2.
Atomic Mass
a.
Atomic Mass is an Average
of All
Naturally Occurring Isotopes
C. Periodic Table
Arrangement
1.
Groups and Periods
2.
Different Labeling schemes
a American,
European, and
IUPAC Versions
3.
Similar Element Groupings
a.
Representative Elements
b.
Transition Metals
c.
Inner Transition
Metals
1)
Lanthanides
2)
Actinides
d.
Alkali Metals and Alkaline Earth
Metals
e.
Halogens and Noble
Gases
4.
Periods and Electron Configurations
a.
Energy Levels and Types of
Orbitals
b.
Periods One Through
Three
c.
The s,p,d, and f Blocks
d.
Valence Electrons and
the Octet
1)
Filled Valence Shells are
Stable
2)
New Periods Begin
After Valence Shells
are Filled
e.
Periods Four and Five
- s, p, and
d Orbitals
f.
Periods Six and Seven
- s, p, d, and
f Orbitals
V. Periodic Trends
A. State of Matter and Metallic Character
1.
Metal Properties
a.
Luster and Conductivity
b.
Malleability and Ductility
2.
Nonmetal Properties
a.
Nonmetals Exist in a Variety
of Physical States
3.
Semimetal Properties
a.
Semiconductors
B. Atomic Radii
1.
Determining Atomic Radii
2.
Trends in Atomic Radii
a.
Moving Down a Group
b.
Moving Across a Period
C. Ionic Radii
1.
Ions Defined: Cations and Anions
a.
Cations are Always Smaller
and Anions are
Always Larger Than
the Noncharged Atom
2.
Trends in Ionic Radii
a.
Moving Down Groups and
Across Periods
b.
Elements in the Same Group
Tend to Form Ions
with the Same Charge
c.
Variations in Ionic Radii
D. Ionization Energy
1.
Determining and Reporting Ionization
Energies
2.
Trends in Ionization Energy:
Groups and Periods
3.
Successive Ionization Energies
a.
Jumps in Ionization Energies
Represent Pulling
Electrons from
Closed Shells
b.
Atoms on the Left of the
Periodic Table Tend to
Lose Electrons
E. Electron Affinity
1.
Determining and Reporting Electron
Affinity
2.
Trends in Electron Affinity: Groups
and Periods
F. Electronegativity
1.
Electronegativity Described
2.
Electronegativity Values have
no Units
3.
Trends in Electronegativity:Groups
and Periods
VI. Conclusion
