1. The Periodic Table
Chapter 5

2. Alchemy & Diderot's Alchemical Chart of Affinities (1778):

3. Dalton's elements and symbols (1808):

6. The Bayley Pyramid Periodic Table

7. Mohammed Abubakr's circular periodic table is one alternative to the standard periodic table of the elements.

9. A Spiral Periodic Table by Prof. Thoedor Benfey

11. Spiral Periodic Table

13. The Dufour Periodictree

14. AtomFlowers
A periodic table that gives a representation of the electron orbitals that look like flowers

15. Chinese periodic table

16. Chapter 5 section 1 pg

17. Organizing the Elements
What was going on in history during this time?
Why is this organization limited?
1750 = 17 elements known
Mostly common metals
After 1750, more chemists begin to study elements many more elements discovered faster
Needed a way to organize elements
1789 Antoine Lavoisier grouped elements based on type
Metals, nonmetals, gases & earths
1860 Mendeleev

18. Mendeleev’s Periodic Table
Draw an example of ordering strategy
Organized elements like a deck of cards
1st  order by mass
2nd  property patterns
esp. rxns with O & H

19. A 2 4 5 6 7 8 9 10 J Q K

20. A 2 3 4 5 6 7 8 9 10 J Q K

21. Mendeleev’s Periodic Table
Draw an example of ordering strategy
Draw a small periodic table to illustrate rows and columns
Organized elements like a deck of cards
1st  order by mass
2nd  property patterns
esp. rxns with O & H
Rows (called periods)
Mass increases from left to right
Columns (called groups)
Mass increases from top to bottom
Similar properties
groups
periods

22. groups
periods

23. Mendeleev’s Periodic Table
Left blanks for elements not discovered yet
Why remember Mendeleev if he wasn’t the first to come up with a P.T.?
Best organization strategy
Used to make accurate predictions about what elements were yet to be discovered

24. Mendeleev’s Periodic Table
EX: Gallium
Predicted similar properties to aluminum
Soft metal
Low melting point
Density ~ 5.9 g/cm3
Truth about gallium:
Melting pt 29.7˚C
Density 5.91 g/cm3
Further proof his PT was good:
Discovery of scandium and germanium
Would gallium be a solid, liquid or gas at room temperature (20-22˚C)?

25. Check your understanding
Pg 126 reading strategy
Pg 127 figure 3
Pg 129 figure 4 (already done )
Pg 129 assessment, #1-8

26. REMINDER!!!
Open note reading quiz
WARNING

27. Chapter 5 section 2 pg

28. 5.2 More on Mendeleev (note: 1860) Did not know about protons
Did not know that all atoms in an element have the same # of protons
His PT arranged by mass, ours by atomic #

29. 5.2 Periods Groups Rows (side-to-side)
# of periods = # of electron energy levels
Groups
Columns (up-and-down)
Similar properties
Similar electron configuration
Determines chemical properties

30. 5.2 Atomic mass Weighted avg.s AMU
# given on PT is an average of the element’s isotope masses
Weighted avg.s
Atomic mass = avg. mass of isotopes compared to how common they are
AMU
Atomic Mass Unit
Unit of mass for atoms (like grams but much smaller!)

31. 5.2 Classes of Elements Solid, liquid, gas  dependant on temp.
Occur naturally vs. those that do not (man-made)
Metals, nonmetals, metalloids

32. 5.2 Metals Most elements are metals (+75%!) Physical properties
Good conductors
Solids at room temp. (except for Hg)
Malleable
ductile
Chemical properties
Some are reactive, others are not (to rust or not to rust?)

33. 5.2 Special Metals Transition metals Chemical properties
Form compounds with distinctive colors
Lanthanide & actinide series

34. 5.2 Nonmetals Physical properties Chemical properties Poor conductors
Brittle
Most are gasses at room temp. (low bp)
Chemical properties
Vary  some very reactive, others not at all
Most reactive = group 17
Least reactive = group 18

35. 5.2 Metalloids Physical properties Conductivity varies with temp.
Semi-conductors  computer chips  “Silicon Valley”

36. Chapter 5 section 3 pg 139-149 Part I: pg 139 & ions
Part II: pg
Part III: pg

37. 5.3 Part I Valence electrons Electrons in the outermost energy level
Chemical properties depend on the number of valence electrons
What does this mean after learning about the organization of the PT?
Groups have similar properties so they must also have similar #s of valence electrons

38. 5.3 Part I Octet magic # in chemistry =
Valence orbitals can hold no more than 8 e-
All atoms want a full valence (8 e-) or none (all or nothing)
Exceptions: H & He
Why?

39. 5.3 Part I
Ions
Atoms that gain or loose e- to fill or empty the valence orbital
1p+ +1

40. 5.3 Part I
Ions
Atoms that gain or loose e- to fill or empty the valence orbital
2p+ Ø

41. 5.3 Part I
Ions
Atoms that gain or loose e- to fill or empty the valence orbital
3p+ +1

42. 5.3 Part I
Ions
Atoms that gain or loose e- to fill or empty the valence orbital
4p+ +2

43. 5.3 Part I
Ions
Atoms that gain or loose e- to fill or empty the valence orbital
5p+ +3

44. 5.3 Part I
Ions
Atoms that gain or loose e- to fill or empty the valence orbital
6p+ +4 `

45. 5.3 Part I
Ions
Atoms that gain or loose e- to fill or empty the valence orbital
6p+ -4 `

46. 5.3 Part I
Ions
Atoms that gain or loose e- to fill or empty the valence orbital
7p+ -3 `

47. 5.3 Part I
Ions
Atoms that gain or loose e- to fill or empty the valence orbital
8p+ -2 `

48. 5.3 Part I
Ions
Atoms that gain or loose e- to fill or empty the valence orbital
9p+ -1 `

49. 5.3 Part I
Ions
Atoms that gain or loose e- to fill or empty the valence orbital
10p+ Ø `

50. 5.3 Part I
Ions
Atoms that gain or loose e- to fill or empty the valence orbital
11p+ +1 `

51. 5.3 Part II Groups Group # Alkali Metals Alkaline Earth Metals
Transition Metals
Boron Family
Carbon Family
Nitrogen Family
Oxygen Family
Halogens
Noble Gases
Group # 1 2
3-12 13 14 15 16 17 18

52. 5.3 Part II For each group: List the elements in that group
How many valence electrons do they have?
What kind of ions do they form?
Are they reactive?
What are some of their physical and chemical properties?
Where are they found?
What are they used for?

53. 5.3 Part III
Elemental Friends & Foes
Add to your group list

54. Transition Metals
Groups 3-12

55. Transition Metals 1st elements discovered Make colorful compounds
Often used to tint/color glass
Metals
Good conductors
Malleable
Ductile
Solids at room temp. (exception Hg)

56. Transition Metals All ions are positively charged
Valence electron #s vary  Type of ion formed varies
Example: Iron – Fe2+ and Fe3+

57. Transition Metals
Most mined
Many uses:
Wires
Construction
Decoration