1. Organizing the PT Activity  1 textbook per group, 1 piece of printer paper per group  Each person needs their own piece of notebook paper  Turn to page 193, do the mini lab  Show me your table (I will sign your paper), draw your table, and answer questions 4 and 5 from the book.

2. The Periodic Table

3. The Mayan Periodic Table

4. The Telluric Helix or Screw-Shaped (1862)

5. Arranged by atomic weights Noticed that every eighth element had similar properties to the last. He called this the law of octaves and related it to the musical scale. Newlands’ Octaves (1864)

6. Mendeleev's Periodic Table (1871) Ordered by atomic mass and lined up according to properties.

7. Modern Periodic Table (extended)  Henry Moseley reordered the elements based on atomic number.

8. The Block at the Bottom The two rows at the bottom are actually removed from the middle of the periodic table to make the table more condensed.

9. Modern Periodic Table (compressed)

10. Periodic Table Lingo Groups –Also called families –The elements in vertical columns –Elements in a group have similar properties –Labeled 1A-8A or 1B-8B

12. Periods –Horizontal rows of elements –Numbered 1 - 7

14. Classification of Elements 1. Metals  Most elements are metals  Have luster (shininess)  Conduct heat and electricity  Most are solid at room temperature  Are malleable and ductile

15. 2. Nonmetals  Opposite of metals  No luster  Poor conductors of heat and electricity  Not malleable or ductile  Solid, Liquid or gases  Physical properties vary greatly

16. 3. Metalloids  Can have the properties of metals or nonmetals or a combination of both

17. Metals/Nonmetals/Metalloids

18. Special Group Names  Group 1A – Alkali Metals  Group 2A – Alkaline Earth Metals  Group 7A – Halogens  Group 8A – Noble Gases  B Groups –D block- Transition Metals –F block- Inner Transition Metals

20. REPRESENTATIVE ELEMENTS

21. Hydrogen  Has properties similar to the metals in Group 1A and the non-metals in group 7A  When Hydrogen acts like a non- metal, it gains an electron or shares electrons to have an electron configuration similar to He.  When Hydrogen bonds with a non- metal, it acts like a metal and is ionized to H +.

23. Group 1A: Alkali Metals  They are VERY reactive!  React with water to create Alkaline (basic) solutions.  Form 1+ Ions  Typically very soft in pure forms  Found in nature as part of compounds due to their high reactivity.  Good Conductors  Must be stored in oil to insure it doesn’t react with its environment Na with water

24. Group 2A: Alkaline Earth Metals  Called that by Medieval alchemists because they didn’t melt in their fires. –In fire they combine with O to form oxides which look ashy.  Typically are shiny solids.  Less reactive than Alkali metals, but still reactive  Form +2 ions

25. Group 3A: Boron Group  Most found as oxides in the earth’s crust.  Most ionize to a +3 charge (Ga and In can form a +1)

26. Group 4A: Carbon Group  Contains 1 non-metal, 2 metalloids, and 2 metals  No good general trends

27. Group 5A: Nitrogen Group  The Nitrogen group contains 2 non- metals, 2 metalloids, and 1 metal.  Physical properties vary.  Most ionize to a 3- charge or share electrons to achieve their octet.

28. Group 6A: Oxygen Group  Contains 3 nonmetals and 2 metalloids  Normally make 2- ions or share 2 electrons to achieve their octet.

29. Group 7A: The Halogens  Highly Reactive!  Combine with most metals forming salts –Halogen means “salt formers”  Tend to form 1- ions or share 1 electron to attain their octet.  They exist at room temperature in all 3 states of matter  Iodine and Astatine=solid  Bromine=liquid  Fluorine and Chlorine=gas

30. Group 8A: The Noble Gases  Nonreactive/Stable  Among the last naturally occurring elements to be discovered because they are colorless and unreactive –They have a full outer shell, preventing them from readily forming compounds –There are no known compounds of helium, neon, or argon

31. D AND F BLOCK ELEMENTS Transition and Inner Transition Metals

32. Family Characteristics  Transition Metals- 38 elements –Have “metals” characteristics –Some are magnetic  Inner Transition Metals (Rare Earth Elements) –30 elements –Most are man-made (synthetic)

33. Transition Metals  All metals  All about the same size, electronegativity, and ionization across a period  Physical properties determined by number of Unpaired electrons. –More unpaired electrons = harder with higher melting points

34. Formation of Ions  Most form 2+ ions, but can form up to 6+ ions –Happens when reacted with a highly electronegative ion like Fluorine  When ionization changes, color tends to change too. –Unpaired electrons can absorb specific wavelengths of light.  No good pattern as to what elements form what ions.

35. Magnetism  A moving electron creates a magnetic field. –Paired e- are not effected –Unpaired outer d electrons are.  Paramagnetism – substances act like temporary magnets  Ferromagnetism – Strong attraction –Ions align with magnetic field –Remain aligned when field is gone.  Ex iron, cobalt, nickel

36. Inner Transition  Tend to be all found mixed together.  Difficult to extract  Most synthetic