1. Unit : Periodic Table Elements and their Properties

2. Bell Work Review comments from objective questions and make corrections as needed.

3. Periodic- regular repeating pattern

4. A. Dmitri Mendeleev – late 1800 devised the periodic table Based on elements atomic mass At the time, only about 63 known elements Left blanks/ spaces in table for unknown elements There were some flaws with his table.

5. C. Modern Table – by increasing atomic number Vertical Columns  “groups or families” – 18 groups – Have similar properties – Elements have the same number of electrons in outer energy level Called “valence electrons” Horizontal Rows  “periods or rows” – 7 periods – DO NOT HAVE similar properties – All elements in the same period have the same number of electron energy levels

6. II. Electron Energy Levels and Orbitals A. Each of the 7 energy levels can hold a maximum number of electrons – Each energy level is a different distance from the nucleus – Atoms only use the number of energy levels that are needed for its electrons – Levels closest to the nucleus have a lower energy

7. B. Within energy levels are orbitals, each holding a certain number of electrons OrbitalShapeTotal # e- holds “s”spherical 2 “p”dumbbell 6 “d”clover10 “f”flower14 i. Each orbital has a certain number of sub-shells that can each hold up to two electrons (that spin opposite each other)

10. I. Metals Found on left side of table Majority of elements on table

11. Properties of Metals solid at room temp – (except Hg)

12. Properties of Metals: Conduct heat and electricity

13. Luster  reflect light well (shiny)

14. Properties of Metals: Malleable – can be hammered or rolled into sheets; Capable of being shaped or formed

15. Properties of Metals: Ductile – can be drawn into wires Tend to lose or give up outer electrons  form positive ions

16. Alkali Metals - Group #1 1 valence electron softer and more reactive than other metals  especially with oxygen and water

17. Alkali Metals: Don’t occur naturally in elemental form – usually in compound form Flame test: Li  crimson Na  Yellow Orange K  Violet

18. Alkaline Earth Metals  Group 2 Moderately reactive not found naturally in elemental form

19. Alkaline Earth Metals Form bases when react with water 2 valence electrons Flame test: – Calcium  dull red – Mg  Bright white flash Strontium –-> bright red – Barium –-> dull yellowish green

20. Transition Metals  Groups 3-12 Often occur in nature as uncombined elements

21. Transition Metals: Typically form colored compounds – Cr found in rubies and emeralds

22. Transition Metals Iron triad – iron, cobalt, nickel – Only elements known to create magnetic field

23. Iron – most widely used of all metals – main ingredient in steel – found in hemoglobin

24. Coinage metals Cu, Ag and Au – Coinage metals since once were commonly used in coins Cu – electrical wiring

25. Transition Metals Nobel Metals – – Highly resistant to corrosion – Ag, Au, Hg, Pt, Pd, Ir, Rh, Ru, Os

26. Inner Transition Metals located at bottom of table ** Called “Rare Earth Elements”

27. Rare Earth Elements Lanthanide Series – includes Lanthanum (La) Actinide Series – includes Actinum (Ac) – All are radioactive, and unstable – Uranium and Plutonium are best known  Nuclear power

28. Transuranic Chemical Elements # 93  until the end all synthetic (manmade) usually disintegrate quickly

29. Other Metals Includes Al, Ga, In, Sn, Tl, Pb, Bi Lead – toxic, no longer in paint and fuel

30. II. Nonmetals Right upper hand corner of table

31. Properties of nonmetals Usually gases or brittle solids at RT Usually Dull Appearance

32. Properties of Nonmetals Not Malleable or ductile Usually Poor Conductors Tend to gain or share electrons when forming bonds  form negative ions

33. Hydrogen Most abundant element in universe Diatomic molecule – two atoms of the same element bonded together Highly reactive element found mostly on Earth as part of water compound Hindenburg

34. Halogens Group 17 (have 7 valence electrons) A salt forms when a halogen forms bond with a metal Fluorine – in toothpaste

35. Chlorine Cl – disinfectant and bleach – (most abundant Halogen)

36. Noble Gases (or Inert gases ) Group 18 exist as isolated, stable atoms, normally unreactive - are found in Elemental form

37. Noble Gases Helium – used in blimps and balloons Neon, Argon and Krypton – used in lights

38. III. Metalloids On either side of zig- zag line Have some metallic and nonmetallic properties Partial Conduction gives them semiconductor characteristics

39. What is an Allotrope? Carbon – found in coal, oil, natural gas and foods All organic compounds contain carbon, but not all compounds are organic Has 3 allotropes  Same element with different molecular structures: 1. Graphite 2. Diamond 3. Buckminsterfullerene (“Bucky Balls”)

40. 1. Graphite

41. 2. Diamond

42. 3.Buckminsterfullerene (“Bucky Balls”) Carbon 60 molecule

43. Atomic Size- How large atom is IV. Periodic Properties of Elements

44. Bell Work Eat breakfast quickly, will be dismissed for assembly at 8:15

45. Atomic Size- How large atom is “atomic radii” Decrease left to right across a period More electrons on energy level stronger attraction between nucleus and the electrons Smaller left to right on table Increases down a family because add an energy level as move down

47. Metallic Nature elements less metallic as go left to right across table increases as go down a family

48. IV. Periodic Properties of Elements Electron Affinity – – elements ablilty to attract an electron to it, increases left to right on table

49. Ionization Energy (IE) The amount of energy required to remove an electron from an atom Easy to remove electron from metals  Low IE, Very hard to remove electron from nonmetal  High IE IE increases as move left to right on table