The Periodic Table

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The Periodic Table

• After this slide, everything in this power point
  must be in your notes you may abbreviate, as
  long as you will understand it as you prepare for
  tests etc.

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Organization of the Periodic Table
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1. Overview of organization

• a)      Groups/ Families
• i)        Go up and down
• ii)      Similar chemical and physical properties
• b)      Periods
• i)        Rows, go across
• ii)      These elements follow a repeating
  pattern as you go across.
• c)      Classes of elements
• i)        Metals-
• ii)      Nonmetals-
• Iii) Metalloids-

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2. Every element is unique!

• a)      Symbol
• i)        First letter must always be in
  capitols! (When there are 2 letters in the symbol
  the second is always in lower case!)
• b)      Atomic Number
• i)        Tells the number of protons in the
  nucleus
• ii)      This number is unique to every element!
• c) There are 92 (94) naturally occurring
  elements! Everything beyond that is created in a
  lab! (And not stable!...radioactive!)

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3. Electron configuration

• a)      Stable elements have full outer shell
  (only one group is stable) That would be 8
  electrons total in that outer shell
• b) Because, all but the noble gases do not have
  a full shell, most elements will gain or lose
  their valence electrons in reactions as they form
  compounds!
• c) Valence electrons are the electrons in the
  outer energy level.

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II) Grouping the Elements!
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1. Alkali Metals -Red

• a)      Group 1
• b)      Very reactive- will often burn or give
  off gas when touched with water!
• c)      One valence electron! Easily give away
  one electron. (This is why they are so reactive!)
• d) Low density- all will float in water!
• http//video.google.com/videoplay?docid-310361068
  7149839311

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2. Alkaline Earth Metals -Orange

• a)      Group 2
• b)      Very reactive, but less reactive than
  group 1
• c)      Two valence electrons (Will lose the 2
  valence electrons)
• d) More dense than group 1
• http//www.youtube.com/watch?vwqErrNvns4o

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3. Transition Metals Blue

• a)      Groups 3-12
• b)      Less reactive than group 2
• c)      1 or 2 valence electrons (will lose
  valence electrons)
• d)      Higher densities and melting points than
  groups 1 2
• e)      Lanthanides Actinides
• i)        These are part of periods 6 7
• ii) They are separated out in order to keep the
  periodic table from getting too wide!

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A look _at_ the PT w/o the La AC below!
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4. Boron Group Yellow

• a)      Group 13
• b)      3 valence electrons
• loses the outer 3 electrons
• Charge 3
• c) Reactive, because there is not a full outer
  shell they will bond with other elements, but
  they do not react violently!

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5. Carbon Group White

• a)      Group 14
• b)      4 valence electrons. They will either
  gain or lose 4 electrons.
• c)      Reactivity depends on the element.
• d) Carbon is the one element that all living
  things have in their atomic structure. We are
  able to date very old, once living things, by
  using radio carbon dating!

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Carbon in action
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6. Nitrogen Group Gray

• a)      Group 15
• b)      5 valence electrons
• gain 3 electrons
• Charge of -3
• c)      More reactive than Group 14
• d) Nitrogen makes up about 80 of the air that
  you breath!

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7. Oxygen Group Brown

• a)      Group 16
• b)      6 valence electrons
• gain 2 electrons
• a charge of -2
• c)      Reactive elements
• d)      All but oxygen are solid at room
  temperature.

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8. Halogens Green

• a)      Group 17
• b)      7 valence electrons
• gain 1 electron
• a charge of -1
• c)      Very reactive! Easily combine with metals
  to form compounds.

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9. Noble Gases Purple

• a)      Group 18
• b)      8 valence electrons
• except for He that has 2!
• c)      Not reactive at all!
• d)      Do not gain or lose electrons!
• e) Full outer shell.

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What is going on with the attraction?
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 Homework!

• Color code your white periodic table (as per the
  colors in the notes!) and put down important
  information
• Name of the group
• and a few facts
• reactivity the number of valance electrons!

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Other things to include

• How to determine the number of
• Protons
• Neutrons
• Electrons
• Simple definitions
• Ions
• Isotopes
• Leave room for more stuff we are nowhere near
  the end of Chemistry!

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