The Periodic Table

1
The Periodic Table

• Proposed by Mendeleev

2
Dmitri Ivanovich Mendeleev1834-1907
Born in Siberia, the last of at least 14
children, Dmitri Mendeleev revolutionized our
understanding of the properties of atoms and
created a table that probably adorns every
chemistry classroom in the world.
3
Arrangements

• Periods Rows determines the number of energy
  levels in an atom
• Lanthanide Series (57-71) rare earth elements
• Actinide Series (89-109) radioactive elements

4
Lanthanide Series Rare Earth Elements
                 
                                               
      

• Not as rare as once thought
• The lanthanides have many scientific and
  industrial uses. Their compounds are used as
  catalysts in the production of petroleum and
  synthetic products. Lanthanides are used in
  lamps, lasers, magnets, phosphors, motion picture
  projectors, and X-ray intensifying screens.

5
Cerium
Lanthanum
6
Actinide Series - Radioactive
                                                
     
They are all radioactive and some are not found
in nature. Some of the elements with higher
atomic numbers have only been made in labs.
7
(No Transcript)
8
Arrangements (cont.)

• Groups or Families arranged according to the
  number of electrons in the outer energy level
• IA or 1 alkali metals
• IIA or 2 alkali earth metals
• VIIB or 17 halogens
• VIII or 18 noble gases inert gases

9
Alkali Metals
                                                
     .

• Very reactive
• One electron in the outer shell
• Shiny
• Light weight

10
Alkali Metals Properties

• Very reactive
• Explode when exposed to water
• Do not occur in nature
• One electron in outer shell
• Softer then most metals
• tarnish rapidly even in dry air
• good conductors of heat and electricity

11
Sodium
12
Alkaline Earth Metals
                                                
      So we just
                                                
     .

• Two electrons in the outer shell
• Fairly reactive (not as reactive as Alkali metals

13
Properties of Alkali Earth Metals

• Have an oxidation number of 2
• Very reactive
• Not as reactive as Alkali metals
• Not found in nature
• Two electrons in outer shell
• Soft metal
• Low-density

14
Magnesium - Mg
Magnesium tarnishes slightly in air, and finely
divided magnesium readily ignites upon heating in
air and burns with a dazzling white flame.
Normally magnesium is coated with a layer of
oxide, MgO, that protects magnesium from air and
water.
15
The Halogens
                                               
    
They have seven electrons in their outer shell.
They are all just one electron shy of having full
shells. Because they are so close to being
happy, they have the trait of combining with
many different elements. You will often find them
bonding with metals and elements from Group One
of the periodic table.
16
Halogens
The Halogens are a generally nasty bunch. Think
toxic choking fumes. But in compounds with the
similarly strong-willed alkali earths, they can
be delicious.
Fluorine
F
17
Halogen Properties

• Non-metallic
• halogen meaning salt-former
• Have 7 electrons in their outer shell
• Oxidation number of -1
• At room temperature, exist in a solid, liquid,
  and gas form

18
Inert Gases - Noble Gases
                                               
   
All of the inert gases have full outer shells
with eight electrons. Oh wait! That's not totally
correct. At the top of the inert gases is little
helium (He) with a shell that is full with two
electrons. The fact that their outer shells are
full means they are quite happy not reacting with
other elements.
19
Properties of the Noble Gases

• Oxidation number of 0
• Have maximum number of electrons in outer shell
• Stable
• unreactive

20
Metals vs Nonmetals
21
Metalloids