The Periodic Table

1
Chapter 12

• The Periodic Table

2
Why make the periodic table?

• Organization As the number of known elements
  grew, lists became hard to use
• Predicting properties elements in the same
  group share properties
• Periodic having a regular, repeating pattern
• Periodic Law Properties of elements are
  periodic functions of their atomic number

3
Areas on the Periodic Table

• Metals/Nonmetals/Metalloids
• Groups
• Periods

4
Metal or Nonmetal?

• Metals, nonmetals, and metalloids are together on
  the periodic table

5
Periods

• Horizontal rows
• Same row same of electron shells
• As you go down the PT, the of electron shells
  increase so the size of atoms increases

6
Groups or Families

• Vertical columns
• Same group same number of valence (outer)
  electrons
• Similar chemical properties

7
Alkali Metals

• Group 1
• 1 valence electron
• Lose during bonding
• Very reactive

8
Alkaline-Earth Metals

• Group 2
• 2 valence electrons
• Lose during bonding
• Very reactive

9
Transition Metals

• Groups 3-12
• Can gain or lose electrons during bonding

10
Groups 13-16

• Named for the top element
• Boron lose 3 electrons
• Carbon gain or lose 4 electrons
• Nitrogen gain 3 electrons
• Oxygen gain 2 electrons
• Most reactive

11
Halogens

• Group 17
• 7 outer electrons
• Gain one during bonding
• Very Reactive

12
Noble Gases

• Group 18
• Full outer shell
• Unreactive

13
Lanthanides Actinides

• Found at bottom of periodic table
• Radioactive

14
Trends on the Periodic Table

• Top to bottom size and mass increase
• Left to right melting and boiling point
  decrease
• Groups on the sides of the periodic table are
  most reactive
• Except Noble Gases