UNIT 5 - THE PERIODIC TABLE & PERIODIC LAW
The Periodic Table
I. Development of the Periodic Table
A. Mendeleev
B. Moseley
II. Groups of the Periodic Table
A. Octet Rule
B. For each group
1. # of
electrons in outermost energy level
2. outer
electron configuration
3. outer
orbital notation
4. definition
of ion
5. lose or
gain electrons?
6. charge of
ion?
7. electron
dot diagram
The Periodic Law
I. Atomic Radius Trend
A. Across a period
1. effective nuclear charge
B. Down a group
II. Ionization Energy Trend
A. Across a period
B. Down a group
1. shielding effect
III. Electronegativity/Electron Affinity Trend
A. Across a period
B. Down a group
IV. Periodic Law
A. The chemical and physical properties of the
elements are periodic functions of their atomic numbers.
B. What this statement really means
North Carolina Essential Standards and Clarifying Objectives:
Chm. 1.2
Understand the bonding that occurs in simple compounds in terms of bond
type,
strength, and properties.
1.2.1 Compare the relative strengths of ionic,
covalent, and metallic bonds.
•
Predict
ionic charges for representative elements based on valence electrons.
Chm. 1.3
Understand the physical and chemical properties of atoms based on their
position on
the Periodic Table.
1.3.1 Classify the components of a periodic table.
•
Identify
groups as vertical columns on the periodic table.
•
Know that
main group elements in the same group have similar properties, the same number
of valence electrons, and the same oxidation number.
•
Summarize
that reactivity increases as you go down within a group for metals and
decreases for nonmetals.
•
Identify
periods as horizontal rows on the periodic table.
•
Identify
regions of the periodic table where metals, nonmetals, and metalloids are
located.
•
Classify
elements as metals/nonmetals/metalloids based on location.
•
Identify
representative (main group) elements as groups 1, 2, 13-18.
•
Identify
alkali metals, alkaline earth metals, halogens, and noble gases based on
location on periodic table.
•
Identify
transition elements as groups 3-12.
1.3.2 Infer the physical properties of an element
based on its position on the Periodic Table.
•
Define
atomic radius and ionic radius.
•
Know group
and period general trends for atomic radius.
•
Apply trends
to arrange elements in order of increasing or decreasing atomic radius. Explain the reasoning behind the trends.
•
Compare
cation and anion radius to neutral atom.
•
Compare the
metallic character of elements.
•
Use electron
configuration and behavior to justify metallic character.
•
Relate
metallic character to ionization energy, electron affinity, and
electronegativity.
•
Identify s,
p, d, f blocks on Periodic Table.
•
Predict the
number of electrons lost or gained and the oxidation number based on the
electron configuration of an atom.
•
Define
ionization energy and know group and period general trends for ionization
energy. Explain reasoning behind the
trend.
•
Apply trends
to arrange elements in order of increasing or decreasing ionization energy.
•
Define
electronegativity and know group and period trends for electronegativity. Explain the reasoning behind the trend.
•
Apply trends
to arrange elements in order of increasing or decreasing electronegativity.