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