PERIODIC TABLE

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PERIODIC TABLE

• Where it all is

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History

• John Newlands determined a repeating pattern of
  every 8 elements. He called it the law of
  octaves.
• Developed in the 1860s
• Dmitri Mendeleev arranged the first on based on
  Atomic Masses.
• Henry Moseley Arranged the Modern Periodic Table
  based on Atomic Number.

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How is it Arranged

• Based on increasing atomic number and on electron
  configurations
• Results in repeating chemical and physical
  properties.
• Groups or Families
• Columns that go up and down.
• There are 18 Groups
• Periods
• Rows that go across
• There are 7 Periods

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Classification of Elements

• Metals
• On the left side
• Make up ¾ of all elements
• Malleable, Ductile, Conduct electricity, form
  positive ions.
• NonMetals
• On the Right side
• Dull, Brittle, Insulators, form negative ions
• Metalloids (Semimetals)
• Found along the staircase between metals and
  nonmetals, have properties of both.

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Group 1 Alkali Metals

• Highly reactive
• Replace Hydrogen in Water
• All have 1 valence electron
• All are s1
• Forms 1 ions

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Group 2 Alkaline Metals

• Very reactive
• Dont replace Hydrogen in Water
• Readily burn in O2 when exposed to heat
• Calcium makes up your bones.
• Batteries get their name from this group
• Have 2 Valence electrons
• All are s2 forms 2 ions

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Transitional MetalsGroups 3 to 12

• These are the common metals
• All have d orbitals filling
• Less reactive then other metals
• Copper, Silver, and Gold least reactive
• Forms various positive ions

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Boron Family Group 13

• Have 3 Valence electrons
• All are s2 p1
• All form 3 ions except
• Boron which forms a 3 ion
• One is a metalloid (Boron)
• The rest are all metals

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Carbon Family Group 14

• Carbon family has 4 valence electrons
• All are s2 p2
• Composed of
• one non-metal (Carbon)
• Two metaloids (Silicon and Germanium
• Two metals (Tin and Lead)

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More on Group 14

• Carbon always forms 4 bonds
• All known life based on Carbon
• Computers function based on Silicon and
  Germaniums unique properties
• They conduct electricity but not heat
• Lead and Tin are common metals
• Used to be used a lot in food storage

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Group 15 Nitrogen Family

• All have 5 valence electrons
• All are s2 p3
• Composed of
• two nonmetals - Nitrogen and Phosphorous
• Two metalloids Arsenic and Antimony
• One metal - Bismuth

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Some facts on 15

• Nitrogen
• makes up most of the atmosphere
• Critical to plant and animal life
• Forms strong bonds that are used in explosives
• Phosphorous
• Critical to plant and animal life

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Group 16 Oxygen Family

• All have 6 valence electrons
• All are s2 p4
• Usually form 2 bonds
• Form 2 ions (except Polonium 2, 4 ions)
• Composed of
• 3 nonmetals Oxygen, Sulfur, Selenium
• 1 metalloid Tellerium
• 1 metal - Polonium

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Group 17 - Halogens

• All have 7 valence electrons
• All are s2 p5
• Forms 1 bond
• Forms 1 ions
• All are nonmetals
• Highly reactive
• Never found in nature as single atoms
• When pure will form F2, Cl2, Br2, I2

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Group 18 Noble Gases

• All have 8 valence electrons
• All are s2 p6
• Rarely form bonds
• Never form ions
• Helium, Neon, Argon have never been found in a
  compound
• Krypton, Xenon, Radium can sometimes be forced to
  form compounds but these are very unstable

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Actiticides and Lanthicides

• Called Rare Earths
• They are rare on earth - Most are manmade
• All are radioactive
• All elements greater then Uranium (92) are
  manmade
• Some are used in medical research

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TRENDS

• Atomic Radius The size of the atom.
• Hard to measure due to cloud not being distinct
• Smaller Up and Right
• Negative Ions Larger
• Positive Ions Smaller
• Ionization Energy The energy required to remove
  one electron, the more electrons removed, the
  more energy required.
• Greater Up and Right
• Fluorine the highest
• Francium the lowest

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More on Trends

• Electronegativity The ability of atoms to
  attract electrons during bonding
• Greater Up and Right
• Fluorine the Greatest Electronegivity
• Francium the Lowest
• Octet Rule Atoms Tend to gain, lose or share
  electrons to have a full (s2, p6) valence shell.
• Shielding Effect The ability of inner electrons
  to shield valence electrons from the nucleus.
  Increase Down, Across Same