Introduction To The Periodic Table Of The Elements by xiaohuicaicai

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									                    October 26, 2009




Introduction To The Periodic
   Table Of The Elements
    Who Came Up With The Periodic
           Table Anyway?
   Dmitri Mendeleev
          Came up with cards for each element
          Put them on a wall in order of increasing
           atomic mass
          It was like a game of cards, where
           Mendeleev tried arranging the elements in
           vertical columns and horizontal rows
              The Periodic Table




What three pieces of information does each square give?
       Organizing The Elements
   Every element has a group and a period:
   Group – A group is a vertical column of
    elements on the periodic table of the elements
   Period – A period is a horizontal row of
    elements on the periodic table of the elements
               Common Groups

   Alkali Metals
   Alkaline Earth Metals
   Halogens
   Noble Gases
                Alkali Metals

   Group 1
   React rapidly when exposed to air and water
   Ex:
           Alkaline Earth Metals

   Group 2
   Less reactive than alkali metals
   If heated, they will burn in air
   Ex:
                  Halogens

   Group 17
   The most reactive non-metals
   Corrosive
   Ex:
                 Noble Gases

   Group 18
   Inert
   Odourless, colourless gases at room
    temperature
   Ex:
       Periodic Table Organizers

   Atomic Number – The atomic number is used
    to organize he elements within the periodic
    table of the elements
   Atomic Mass – The atomic mass is the average
    mass of an elements' atom
   Where will these concepts be important?
              Atomic Notation

    Atomic notation allows for the atomic
     mass and atomic number of an element to
     be visible.

Atomic Mass
                      4
Atomic Number         2
       Subatomic Particle Details

   Atomic number = number of protons = number
    of electrons (atoms have no overall electrical
    charge)


   Atomic mass - atomic number = number of
    neutrons
      Subatomic Particle Example

   Ex:

								
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