Chapter 6: The Periodic Table
How did Mendeleev organize his
periodic table?
*arranged in order of increasing atomic mass.
*periodic table can be used to predict the properties of
undiscovered elements
The CURRENT periodic table has elements
arranged in order of increasing atomic number
Elements are in order of increasing atomic number
There are repeating patterns of properties
The properties change as you move from left to right
The pattern of properties repeats from one period to the next.
Metals
Nonmetals
Metalloids
METALS
•Good
conductors
•80% of all
elements
•High luster
•Ductile
•Malleable
NON-METALS
•Poor conductors
•Dull and brittle
•Most are gas at
room temperature
METALOIDS
•Properties of
both metals
and nonmetals
•Behavior can
be controlled
by changing
conditions
What type of information can be displayed in
a periodic table?
Symbols, names of elements, and information about the structure of the atom
Horizontal rows are called periods
BTW:
The period indicates
the number of
electron energy
levels
Vertical
columns
are called
families or
groups
BTW: elements have similar properties
The background colors in the squares are
used to distinguish groups of elements
Group 1A: Alkali metals
Group 2A: Alkaline earth metals
Group 7A: Halogens
Group 8A: Noble Gases
Color Code
your
Periodic Table
Use the periodic table in the inside back cover of your textbook or on page 162.
Noble Gases:
group 8A
Inner Transition
Metals:
Below the main
body of the
periodic table
Representative
Elements:
groups 1A to 7A
Transition
Metals:
group B
How can elements be classified based on their
electron configuration? BY GROUP!!
Noble Gas
Noble gases are elements in Group 8A
Noble Gases ALL have a full outer e- energy level (shell) (Valence Electrons)
The Representative Elements
●Elements in groups 1A through 7A are often
referred to as representative elements
because they display a wide range of
properties.
● The group number equals the number of
electrons in the highest occupied energy level
Valence e-
Group 1A: Alkali Metals
Group 1A: one electron in the highest occupied energy level
Group 4A
Group 4A: four electrons in the
highest occupied energy level
Blocks of elements
You are ready to complete:
Properties of
Metals and NonMetals Worksheet
Use your NEW and IMPROVED colorful periodic table!!
FLIP BOOK
• Fold Hamburger
Style
• Cut the ONLY the
cover page to
separate the
sections
• GLUE the back of
the booklet into
your lLB
(Interactive Lab
Book)
Periodic Table Trends
Metallic Properties .
Atomic Size .
Ion Size .
Ionization Energy .
Electronegativity . .
COVER
PAGE
FLIP BOOK Inside:
Diagram: Definition:
.
.
.
.
Metallic Character (Properties)
Definition:
Metals are: •Malleable
•Ductile
•High Luster
•Good conductors
•Usually solid at room temperature
Metallic Character
Metallic properties DECREASE from left to right
Atom Size
The atomic radius is one half of the distance
between the nuclei of two atoms of the same
element when the atoms are joined.
Definition: Distance between the 2 nuclei of
joined atoms (same element) divided by 2
In general, atomic size increases from top to
bottom within a group and decreases from left to
right across a period.
Size generally decreases from
Left to right Larger Smaller
Ions: During reactions between metals and nonmetals,
metal ions tend to lose electrons
and nonmetals tend to gain electron
• Cations are positive
ions, they lose
electrons
• Anions are negative
ions and they gain
electrons
Ionic Size
Cations are smaller than the atoms and
anions are larger than the atoms
Ionic Size Definition:
• Cations are smaller than the original atom
• Anions are larger than the original atom
• Ion: an atom that either gained an e- or lost an
e-
• Cation: positive charged ion (gave away e-)
• Anion: negative charged ion (Gained an e-)
Trends in ionic size:
Size of cation decreases
as you move right Size of anion increases
Definition: the energy required to remove an
electron from an atom. (make it an ion)
Trends in Ionization Energy
Energy generally increases
In general the ionization energy tends to
increase from left to right across a period and
decrease from top to bottom within a group.
Definition:
Electronegativity: the ability of an atom to attract
electrons when it is in a compound
Electronegativity
Electronegativity increases
In general, electronegativity decreases from top to
bottom within a group and increase from left to right
Practice: Use your flip book to answer these questions:
1. Which is more metallic, iron or zinc?
Practice: Use your flip book to answer these questions:
1. Which is more metallic, iron or zinc?
2. Which atom is smaller, silver or xenon?
Practice: Use your flip book to answer these questions:
1. Which is more metallic, iron or zinc?
2. Which atom is smaller, silver or xenon?
3. Does the phosphorus atom become smaller or
larger when it becomes an ion?
Practice: Use your flip book to answer these questions:
1. Which is more metallic, iron or zinc?
2. Which atom is smaller, silver or xenon?
3. Does the phosphorus atom become smaller or
larger when it becomes an ion?
4. Which is the smallest ion? K+, Ca2+, Na+ or Mg2+
Practice: Use your flip book to answer these questions:
1. Which is more metallic, iron or zinc?
2. Which atom is smaller, silver or xenon?
3. Does the phosphorus atom become smaller or
larger when it becomes an ion?
4. Which is the smallest ion? K+, Ca2+, Na+ or Mg2+
5. Which electron has the highest ionization energy,
the 1st or the 2nd?
Practice: Use your flip book to answer these questions:
1. Which is more metallic, iron or zinc?
2. Which atom is smaller, silver or xenon?
3. Does the phosphorus atom become smaller or
larger when it becomes an ion?
4. Which is the smallest ion? K+, Ca2+, Na+ or Mg2+
5. Which electron has the highest ionization energy,
the 1st or the 2nd?
6. Which atom has the highest electronegativity?
Practice: