1. Periodic Table of Elements

2. Dmitri Mendeleev Created first version of periodic table.
Predicted properties of elements yet to be discovered.
Ted Talk:
Rockin the shaggy beard…

3. Arranged elements according to atomic weights.
Today they are arranged by atomic number.
Development of the Table: 3:39

4. Periodic Law
“Properties of elements are periodic functions of their atomic numbers.”
In other words, properties tend to repeat as you start a new period.

5. Groups/Families (Columns 1-18)
Elements have:
Same number of valence electrons.
Similar chemical properties.
Form bonds in same way to get stable octet.

6. Periods (Rows 1-7) Elements have:
Same number of occupied energy levels.
Do not have similar properties.

7. Group 1: Alkali Metals 1 valence electron Form +1 Ions Very reactive
Found only in compounds.

8. http://youtu.be/uixxJtJPVXk Rubidium

9. Group 2: Alkaline Earth Metals
2 valence electrons
Form +2 ions
Very reactive
Found only in compounds

10. Some Alkaline Earth Metals
Group 2:
Some Alkaline Earth Metals

11. Group 17: Halogens 7 valence electrons Form -1 ions Very reactive
All nonmetals

12. Extremely reactive gas
Liquid
Solid
FLUORINE
Extremely reactive gas
IODINE
solid → gas
(sublimes)
3:00

13. Group 18: Noble Gases Inert Gases Have stable octet (except He)
Not reactive
Have stable octet
(except He)
Monoatomic gases

14. Transition Metals Metals in the “lower” columns. (d-block metals)
“Inner” transition metals are the two bottom rows
(f-block metals)

15. Transition Metals Form colored compounds and solutions.
Often have multiple “oxidation states” (charges)
Honors: May involve d-sublevel electrons in forming bonds

16. Lanthanide & Actinide Series
Two rows on the bottom of the table
“f” block
Start with lanthanum and actinium
Also called “inner Transition Metals”

17. Man Made Elements: (“Trans Uranium”)
Elements above Uranium (Atomic #92)
Not found naturally on earth
Must be created through nuclear bombardment using particle accelerators.
Radioactive Elements:
All atoms of elements higher than Bismuth (Atomic #83) are radioactive.

18. Do we know our groups? Elements Song Again!
Periodic Table Dating Game
Ted Talk: 4:24

19. Metals/Nonmetals/Metalloids

20. Properties of Metals Luster Malleable Ductile
Conduct heat and electricity
Lose valence electrons, form positive ions
All solids (except Hg)

21. Nonmetals No luster Brittle (if solid) Don’t conduct
Gain valence electrons, form negative ions
Can be solid, liquid, gas
Hydrogen is a nonmetal

22. Metalloids (Semimetals)
Most elements along the “staircase”
Properties of both metals and nonmetals.
B, Si, Ge, As, Sb, Te, At

23. Trends in the Periodic Table

24. Atomic Radius
Distance from nucleus to the outer edge of electron cloud.

25. Trends in Radius (Use Table S)Li Na K Rb Cs Fr
Down a Group
Ex: Group 1 What happens?
Across a Period
Ex: Period 2 What happens?
Li Be B C N O F Ne

26. Why does this trend happens?
Let’s Think:
Why does this trend happens?
How might it be related to electron shells and electron repulsion?
How might it be related to the pull of nuclear charge?

27. Down a Group: Size increases Add new energy levels
Greater shielding from core electrons
Outer electrons further from nucleus so less attractive force

28. Across a Period: Size decreases
Increasing nuclear charge pulls on same # of energy levels
No increase in shielding effect

29. Ionization Energy
Energy required to remove outermost electron

30. Trends in Ionization Energy (Use Table S)
Down a Group
Ex: Group 1 What happens?
Across a Period
Ex: Period 2 What happens? Li Na K Rb Cs Fr
Li Be B C N O F Ne

31. What is the trend? Down a Group IE __________________
Across a Period IE _________________
Therefore:
Larger Radius = Lower Ionization Energy

32. Why?
The further outermost
electron is from nuclear
pull, easier it is to remove.
More shells of kernel
electrons around nucleus
creates a greater
“shielding effect”.

33. Electronegativity
Attraction an atom has for electrons involved in bond formation.

34. Electronegativity
The higher the EN value the more the atom “pulls” on electrons involved in bond.
“Tug of war” for electrons in bond

35. Fluorine has the highest EN value = 4
EN scale was created by comparing other elements to Fluorine
Nonmetals generally have much higher EN values than metals

36. How does this Affect Bonds?
Polar Bond:
Unequal electron sharing
Atoms have different EN
Nonpolar Bond:
Equal electron sharing
Atoms have same EN

37. Trends in Electronegativity (Use Table S)
Down a Group
Ex: Group 1 What happens?
Across a Period
Ex: Period 2 What happens? Li Na K Rb Cs Fr
Li Be B C N O F Ne

38. What was the trend in electronegativity?
Down a group EN _________________
Across a period EN ________________
What is the relationship to atomic radius?
As size gets bigger EN gets ______________
As size gets smaller EN gets _____________
What element has the highest EN value?
What elements don’t have really have electronegativity values? Why is that?

39. Metallic/NonMetallic Character
More “Metallic”:
Large radius
Low IE
Low EN
More “Non Metallic”:
Small radius
High IE
High EN

40. Links and Songs (Honors) Intro to the Table
Dan Radcliffe Knows his elements!
Elements Song:
Periodic Table of Videos Crew:
A different Song
LIST OF COOL LINKS

41. Crash Course Video(13 minutes)
Interactive Table
Sortify Game
Go React Periodic Table