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PERIODIC TABLE

PERIODIC TABLE. Where it all is. History. John Newlands determined a repeating pattern of every 8 elements. He called it the law of octaves. Developed in the 1860’s Dmitri Mendeleev arranged the first on based on Atomic Masses.

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PERIODIC TABLE

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  1. PERIODIC TABLE Where it all is

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

  3. 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

  4. 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.

  5. Group 1 – Alkali Metals • Highly reactive • Replace Hydrogen in Water • All have 1 valence electron • All are s1 • Forms +1 ions

  6. Group 2 – Alkaline Metals • Very reactive • Don’t 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

  7. 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

  8. 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

  9. 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)

  10. More on Group 14 • Carbon always forms 4 bonds • All known life based on Carbon • Computers function based on Silicon and Germanium’s unique properties • They conduct electricity but not heat • Lead and Tin are common metals • Used to be used a lot in food storage

  11. 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

  12. 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

  13. 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

  14. 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

  15. 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

  16. 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

  17. 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

  18. 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

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