I II III

The Periodic Table

Chemical Reactivity

Alkali MetalsAlkaline Earth MetalsTransition MetalsHalogensNoble Gases

Chemical Reactivity

Period/RowFamilies/Groups/Columns

Elements in the same family has the SAME # of valence electrons

1

2

3

4 5

6

7

Atomic Radius is the distance from the nucleus to the outermost orbital

Increases to the LEFT and DOWN

Atomic Radius

Why larger going down?

Higher energy levels have larger orbitals

Why smaller to the right?

Increased nuclear charge

Atomic Radius

Which atom has the larger radius?

Be or Ba

Ca or Br

Ba

Ca

Examples

Ionization Energy- the energy required to remove 1 electron from the parent atom

Why opposite of atomic radius?

In small atoms, e- are close to the nucleus where the attraction is stronger

Ionization Energy

1

2

3

4

5

6

7

First Ionization Energy Increases UP and to the RIGHT

Ionization Energy

Which atom has the higher 1st I.E.?

N or Bi

Ba or Ne

N

Ne

Examples

1

2

3

4 5

6

7

Melting/Boiling Point – the temperature at which a substance changes states

Highest in the middle of a period.

Melting/Boiling Point

Which atom has the higher melting/boiling point?

Li or C

Cr or Kr

C

Cr

Examples

Ionic Radius

The distance between the center of the nucleus and the outer edge of the ion

Cations/Metals

-lose elections, so they have a positive charge

-small

Atoms

-neutrally charged elements

-medium

Anions/Nonmetals

-gain electrons, so they have a negative charge

-large

Electronegativity

*The measure of how strongly an atom attracts electrons when it is combined with another element

• Increases from left to right (except for noble gases) due to increased nuclear charge

• Increases as you move up a group due to the shorter distance between the nucleus and valence electrons.

Increases UP and to the RIGHT

1

2

3

4 5

6

7

Which particle has the largest electronegativity?

S or P

Al or Ga

S

Al

Examples