1. Self and Group Evaluations
Criteria
Unacceptable 1
Marginal 2
Very good 3
Outstanding 4
Quality of work
Work was not usable, or regularly needed major rework
Work often had flaws and omissions that needed fixing
Generally high quality of work, only occasional fixes needed
Amazingly good output, well beyond expectations
Quantity of work
Did hardly any work.
Contributed OK, somewhat less than their share.
Worked hard, carried their share of the load.
Considerable extra work, more than their share.
Dependability and meeting commitments
Could not be counted on at all.
Usually met commitments. Needed some reminders or follow-up.
Conscientious about commitments. Very dependable.
Went out of the way to pick up slack for others who miss commitments.
Interaction, supporting other team members, sharing information
Was a major problem to interact and work with.
Some interaction problems, unhelpfulness, or failure to communicate.
Interacted well with others, helpful, flexible, pleasure to work with.
Went out of the way to help teammates and enable them to contribute.
Team meetings: participation, use of team time
Little participation in discussions and activities, wasted the class team time.
Participation spotty: not always participative, did not always use class team time effectively
Participated fully in all team activities, used the class team time wisely
Drew out others and ensured that everyone participated, used and encouraged the team to use the class meeting time efficiently
Overall Contributions Rating
Often failed to complete assigned work, was difficult to work with and made no real contributions to the team.
Sometimes failed to complete assigned work, was often unprepared, but made some contributions
Consistently good contributions, valuable member of the team, and usually prepared
Did everything well and added some outstanding contributions

2. Today’s Do Now 9/9/2014 Number of protons in the nucleus
1. What is the definition of atomic number?
2. What is the definition of atomic mass?
Number of protons in the nucleus
Neutrons + Protons; mass of an atom

3. Today’s Catalyst 9/9/2014
D, E, Q 1 3

4. By the end of the class period today, I will be able to….
compare and contrast Mendeleev and Moseley’s periodic tables.
explain the benefits and drawbacks of the Bohr model of the atom, and describe the currently accepted theory of the locations of electrons around an atom.

5. History of the Periodic Table
By 1860, more than 60 elements had been discovered
(How should we organize all of these elements!?)

6. History of the Periodic Table
Mendeleev is credited with developing the periodic table (father of the PT!)
Created his table in 1869

7. History of the Periodic Table
Mendeleev arranged the elements in order of increasing atomic mass and noticed that certain similarities in element’s properties appeared at regular intervals

8. Mendeleev’s Table Arranged in order of increasing atomic mass
Rows and columns switched

9. Henry Moseley
In 1911, Henry Moseley created a periodic table that was arranged by increasing atomic number.
How is the PT organized today?

10. Write-Pair-Share
What is the main difference between Mendeleev and Moseley’s periodic table? What are some similarities between the two tables?

11. Rows (periods): elements are put in rows by increasing atomic number Columns (groups): elements are put into columns (groups) based on how they react (chemical properties)

12. Take out your Periodic Table!

13. Natural States of the Elements
(solid/liquid/gas)

14. Next objective!
explain the benefits and drawbacks of the Bohr model of the atom, and describe the currently accepted theory of the locations of electrons around an atom.

15. What’s wrong with this picture??

16. By the end of class today I will be able to…
describe the organization of the electron cloud into energy levels and sublevels
list the amount of electrons that can fill each energy level

17. Electrons must occupy specific energy levels.
What Bohr Did Right…
Electrons must occupy specific energy levels.

18. What Bohr Did Right…
Electrons of increasing energy occupy orbits farther and farther from the nucleus
Electrons exist in quantized orbits (specific energy levels).
Electrons can’t exist between energy levels

19. Electrons Exist in Quantized Energy Levels

20. Electrons exist in Quantized Energy Levels… just like steps on a staircase
Electrons can’t exist between energy levels, just like people can’t stand between stair steps

21. Group Practice
With the partner who is sitting next to you, create an analogy about quantized energy

22. Partner Work Expectations
Both partners need to contribute to the final product
Conversation should be on task
2 minute time limit!!

23. Draw your analogy/something brilliant below:
Electrons exist in Quantized Energy Levels… just like “something brilliant.”
Draw your analogy/something brilliant below:

24. Electrons exist in Quantized Energy Levels… just like
Draw your analogy/something brilliant below:

25. Where Bohr Went Wrong…
Electrons do not travel in neat, planet-like orbits

26. Atoms actually look something like this:
This will blow your mind!

27. Bringing it all together:+

28. Energy levels contain orbitals
Energy level= stair 1. 2. 3. 4.
Stairs contain shapes
Shapes contain orbitals

29. What is an orbital??
Orbital: a three-dimensional region around the nucleus
Each orbital contains 2 electrons; where the electrons spend 90% of their time

30. Total number of electrons
Guided Notes
Orbital
(Subshell)
Shape
Number of Orbitals
Total number of electrons S
Sphere 1 2 P D F

31. S orbital

32. Total number of electrons
Guided Notes
Orbital
(Subshell)
Shape
Number of Orbitals
Total number of electrons S
Sphere 1 2 P
Peanut 3 6 D F

33. P orbital

34. Total number of electrons
Guided Notes
Orbital (Subshell)
Shape
Number of Orbitals
Total number of electrons S
Sphere 1 2 P
Peanut 3 6 D
Clover 5 10 F

35. d orbital

36. Total number of electrons
Guided Notes
Orbital Shape
Shape
Number of Orbitals
Total number of electrons S
Sphere 1 2 P
Peanut 3 6 D
Clover 5 10 F
Flower? 7 14

37. f orbital

38. Practice, practice, practice
Whiteboard directions/expectations

39. Practice, practice, practice
How many electrons can an orbital hold?

40. Practice, practice, practice
How many electrons can an orbital hold? 2

41. Practice, practice, practice
True or false? Each energy level contains shapes.

42. Practice, practice, practice
True or false? Each energy level contains shapes. Answer: TRUE

43. Practice, practice, practice
How many electrons can the S orbital shape hold?

44. Practice, practice, practice
How many electrons can the S orbital shape hold?
Answer: 2

45. Practice, practice, practice
What is the shape of d orbitals? 

46. Practice, practice, practice
What is the shape of d orbitals? Answer: Clover

47. Practice, practice, practice
Name that orbital: This orbital shape can hold 6 electrons and is shaped like a peanut/dumbbell.

48. Practice, practice, practice
Name that orbital: This orbital can hold 6 electrons and is shaped like a peanut/dumbbell. Answer: p orbital

49. Practice, practice, practice
Put your notes away!

50. Practice, practice, practice
How many orbitals does the f orbital shape contain?

51. Practice, practice, practice
How many orbitals does the f orbital shape contain? Answer: 7

52. Practice, practice, practice
How many electrons does the f orbital shape contain?

53. Practice, practice, practice
How many electrons does the f orbital shape contain? Answer: 14

54. Practice, practice, practice
What is the number of orbitals in the p-shape? What is the number of electrons total in the p-shape?

55. Practice, practice, practice
What is the number of orbitals in the p-shape? What is the number of electrons total in the p-shape? Answer: 3 orbitals; 6 electrons

56. Practice, practice, practice
Why was Bohr’s model wrong?

57. Practice, practice, practice
Why was Bohr’s model wrong? Electrons do not orbit the nucleus on singular paths (like planets around the sun)

58. Practice, practice, practice
Where do electrons have more energy? Closer or farther from the nucleus?

59. Practice, practice, practice
Where do electrons have more energy? Closer or farther from the nucleus?

60. Which electron has more energy?#1 #2