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Periodic Table

Periodic Table. Chemistry is believed to have its origin with the Greeks and the Romans. Classification began early. Trends in the Periodic chart. Dobereiner—1817 Classified 3 related elements----Triad He used Ca Ba Sr. Newland---1863

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Periodic Table

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  1. Periodic Table

  2. Chemistry is believed to have its origin with the Greeks and the Romans. • Classification began early.

  3. Trends in the Periodic chart • Dobereiner—1817 • Classified 3 related elements----Triad • He used Ca Ba Sr

  4. Newland---1863 • Arranged elements by mass & realized that a pattern developed every 8th element: this is the Law Of Octaves

  5. Octet Rule: • elements with 8 e- in the outer energy level will be MOST stable and unreactive

  6. Parts of the Periodic Table • Rows/periods -7 • Groups/families ---18 • or • 1A, IIA, IIIA, IVA, VA, VIA, VIIA, VIIIA • IB, IIB, IIIB, IVB, VB, VIB, VIIB, VIIIB

  7. Periodic Table • Row(Period)—horizontal arrangement of elements on the chart • Group (Family)---vertical arrangement of elements on the chart—elements in the same family will have similar properties

  8. Families • Alkali metals----Group 1 • Alkaline earth metals---Group 2 • Chalcogens---oxygen family group 16 • Halogens---group 17 • Inert or Noble Gas----group 18 • Transition metals –3-12 • Rare earth metals –lanthanoid & actinoids

  9. Special PeriodsInner Transition Metals • Lanthanoid Series---58-71 • Actinoid Series---90-103

  10. Classes of Elements • Metals-- (left of zig/zag line) • Most are solid • Conduct electricity/heat well • Lose electrons to form + cations • Malleable ( can be bent into shapes) • Ductile ( can be pulled into a wire)

  11. Classes of elements • Non-metals--- to the right of zig/zag line • Liquids and gases • Gain electrons to form negative anions • Poor conductors • Brittle

  12. Classes of elements • Metalloids---lie exactly to left or right of the zig/zag line. Have properties of both metal and non-metals • Semi-conductors or insulators • Semi-metals

  13. Special metals • Transition metals— • Groups 3-12 • Multiple oxidation states • Hardest metals known • Elements with electrons in “d” orbitals

  14. Vocabulary • Valence electrons---electrons in the outer shell of an atom. • Group # #valence e- • 1 1 • 2 2 • 13 3 • 14 4 • 15 5 • 16 6 • 17 7 • 18 8 (except He)

  15. Representative Elements ( Main Group )----Groups 1,2, 13-18 • Oxidation state--- created by number of electrons lost or gained

  16. Vocabulary • Inert Gases or Noble Gas— • Have filled outer shells and are unreactive • “p” orbitals are full

  17. chart • Group oxidation number • 1 +1 • 2 +2 • 13 +3 • 14 + or – 4 • 15 -3 • 16 -2 • 17 -1 • 18 0

  18. As the Periodic Table began to take shape certain “trends” became apparent: • Size of atom (atomic radius) • Density • Metallic Character • Reactivity • Electronegativity • E-affinity • Ionization energy • Shielding effect

  19. Atomic radius: • Down a group----I (due to e- levels) • Rt to left on row----I (due to # of p+ ) • Ion size: • Anion(neg) > neutral • Cation(pos) < neutral

  20. Density • Down a group ----I • No trend for row

  21. Metallic Character • Down a group -----I • Rt to Left on row ----I

  22. Reactivity: • Down a group ---I ( metallic ) • Up a group -----I ( non-metallic) • The MOST reactive metal is Francium • The MOST reactive non-metal is Fluorine • No row trend

  23. Electronegativity---an attraction an atom for a “shared pair” of e- • Electronegativity --- • Down a group ---D (due to #e- levels) • Lt to rt on row----I (due to #p+ )

  24. Electron Affinity– attraction of atom for an electron • E- - affinity - • Down a group ---D • Lt to rt on row ---I

  25. Ionization energy ---energy needed to remove an e- from a neutral atom • Ionization energy— • Down a group ---D ( because of # e- levels) • Lt to rt on a row---I (due to # P+ )

  26. Shielding effect—decrease in the attraction between outer e- and the nucleus due to the presence of other e- between them • Shielding effect: • Down a group –I • Lt to right on row ---- same

  27. When using trend rules to answer a question, remember: • A) ask are these atoms in same row or same group • B) what is the trend for that property for a)a row or for a b) group

  28. Which is smallest from the following; • Si Pb Sn C

  29. Which is largest? • F B N Ne

  30. Which has the highest electronegativitiy? • Na Cl Ar Al

  31. Which has the lowest electronegativity? • Sb N As P

  32. Which has the highest ionization energy? • N C Li Ne

  33. Which has the lowest ionization energy? • Zn Hg Cd

  34. Which has the greatest shielding? • Ne Xe Ar He

  35. Which has the greatest amount of shielding? • S Al Ar Na

  36. Which atom has highest e-affinity? • K Li Fr Na

  37. Which atom has the smallest e-affinity? • Pb C Sn Si

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