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: