1. Unit 5: The Periodic Table
Chemistry

2. Agenda 11/3/14 Today’s Objectives: - Hand back spectra labs
- Introduction to the Periodic Table
- Periodic Table Activity
HW: Finish the questions from the table structure activity
Now: Quietly read the unit 5 learning targets,
Highlighting words you may not be familiar with

3. Structure of the Table
Using a blank Periodic Table create your own table following the guidelines in the activity directions.
Be sure to pay attention to what each section is called.
Do not answer the questions for this lab yet, we will have time at the end of the class period to work on the questions.

4. Crystal Lake Central Nobel Prize Contest

5. We have discovered new elements!!
It is your job to take the data you are given and arrange it in a way that organizes all of the data. You will slowly get more information as scientists discover it. You will have to present your table to the other scientists in the class upon your final draft, be sure to have a reason for your setup!!

6. The first set of Data
**The elements are named after the famous scientists who discovered them at The University of Iowa

7. Element
Symbol
Mass # (Top Right)
Meekeron Em
30.97
Bernardine Bp
19.00
Sonntagium Js
14.01
Baldinic Mb
79.90
Ballentite Kb
32.07
Kreiterite Ck
20.18
Leonardium Ln
35.45
Olsonium Om
16.00
Schmiederon Sh
74.92
Soderlous Sd
28.09

8. Element
Symbol
Mass # (Top Right)
Energy Levels (Bottom Right)
Meekeron Em
30.97 3
Bernardine Bp
19.00 2
Sonntagium Js
14.01
Baldinic Mb
79.90 4
Ballentite Kb
32.07
Kreiterite Ck
20.18
Leonardium Ln
35.45
Olsonium Om
16.00
Schmiederon Sh
74.92
Soderlous Sd
28.09

9. Element
Symbol
Mass # (Top Right)
Energy Levels (Bottom Right)
# protons (Top Left)
Meekeron Em
30.97 3 15
Bernardine Bp
19.00 2 9
Sonntagium Js
14.01 7
Baldinic Mb
79.90 4 35
Ballentite Kb
32.07 16
Kreiterite Ck
20.18 10
Leonardium Ln
35.45 17
Olsonium Om
16.00 8
Schmiederon Sh
74.92 33
Soderlous Sd
28.09 14

10. Element
Symbol
Mass # (Top Right)
Energy Levels (Bottom Right)
# protons (Top Left)
Valence electrons (Bottom Left)
Meekeron Em
30.97 3 15 5
Bernardine Bp
19.00 2 9 7
Sonntagium Js
14.01
Baldinic Mb
79.90 4 35
Ballentite Kb
32.07 16 6
Kreiterite Ck
20.18 10 8
Leonardium Ln
35.45 17
Olsonium Om
16.00
Schmiederon Sh
74.92 33
Soderlous Sd
28.09 14

11. Our Periodic Table
Is organized so that the properties of elements repeat themselves in each row. Mendeleev was able to predict properties of elements before they were discovered!! Can you predict the properties of an element that would fit in the hole in your periodic table??

12. Fake Element
Real Element
Meekeron (Em)
Phosphorus
Bernardine (Bp)
Fluorine
Sonntagium (Js)
Nitrogen
Baldinic (Mb)
Bromine
Ballentite (Kb)
Sulfur
Kreiterite (Ck)
Neon
Leonardium (Ln)
Chlorine
Olsonium (Om)
Oxygen
Schmiederon (Sh)
Arsenic
Soderlous (Sd)
Silicon

13. Element
Fake Symbol
Mass #
Orbital
Shells
# protons
Valence electrons
Phosphorus Em
30.97 3 15 5
Fluorine Bp
19.00 2 9 7
Nitrogen Js
14.01
Bromine Mb
79.90 4 35
Sulfur Kb
32.07 16 6
Neon Ck
20.18 10 8
Chlorine Ln
35.45 17
Oxygen Om
16.00
Arsenic Sh
74.92 33
Silicon Sd
28.09 14

14. Agenda 11/4/14 Happy Election Day
Today’s Objectives:
- Recap Yesterday
- What are metals and non-metals?
- Begin analyzing the Periodic Table
Now: Take out your homework from last night

15. Our Roadmap to the Chemical World
Where are the transition metals located?
Where are the metalloids located?
Where are the Non-metals located?
Where are the Metals located?

16. Important Properties of…
Metals:
Non-Metals:

17. Structure and Regions Metals Largest region – left of staircase
Solids (except Hg)
Conduct heat/electricity
Luster
Ductile (stretchable)
Malleable (able to be flattened)

18. Structure and Regions Right of staircase Solids, liquids, gases
Non-metals
Right of staircase
Solids, liquids, gases
Low conductivity (heat and electricity)
Low luster
Brittle solids

19. Structure and Regions On staircase
Metalloids/Semi-Metals
On staircase
Share properties of metals and nonmetals
Semi-conductors

20. Some Vocab you need to know
Family/Group
Period

21. Blast from the past!!! Write the electron configuration for: Li Na K
Do you notice a trend?
As you go down a family/group, each element gains an energy level.

22. Agenda 11/5/14 Today’s Objectives: - Review P.T. Basics
- Learn the Trends of the Periodic Table
HW: Complete note review of periodic trends
Now: Discuss with your neighbors about the answer to yesterday’s homework question!

23. The Shielding Effect
The ability/tendency of lower energy level electrons to “shield” outer electrons from the pull/attraction of protons in the nucleus.

24. Which would show a greater “Shielding Effect”?

25. Greater Shielding
Having a greater shielding effect means that the outer electrons are not as attracted to the nucleus. Remember our holding hand demo…

26. Atomic Size/Radii

27. Atoms increase in size as you go from top to bottom within a family/group because . . .
“Bottom” elements have electrons in higher principal energy levels ---> greater distance from the nucleus ---> more levels means larger atom!
Plus, each successive element in a group exhibits a greater shielding effect!! Outer electrons feel only a weak pull from the nucleus!

28. Atoms decrease in size as you go from left to right across a period because . . .
From left to right, successive elements have more protons & electrons. However, the “extra” electrons do not occupy higher energy levels, so there is no additional shielding effect. With the “extra” protons, all electrons are pulled closer to the nucleus!

29. Smallest Atomic Radius! (Helium)
Greatest Atomic Radius! (Francium)

30. Let’s Recap
What are some properties of Metals? What are some properties of Non-Metals? What causes the changes in atomic size within a FAMILY? What causes the changes in atomic size in a PERIOD?

31. Agenda 11/6/14 Today’s Objectives: - Review P.T. Basics - Discuss Ions
- Ionization Energy
HW: Forming Ions Homework
Now: Find a partner for an activity

32. Let’s Recap
What are some properties of Metals? What are some properties of Non-Metals? What causes the changes in atomic size within a FAMILY? What causes the changes in atomic size in a PERIOD?

33. P.T. Review
2. Vertical columns of elements are called groups/families. Horizontal rows are called __________.
3. True or False: Elements in the same row tend to have very similar chemical properties.
4. What is the chemical symbol for the halogen in Period 4?
5. An element’s outermost electrons are found in the 5th energy level. The Lewis dot structure for the element shows four dots. Give the chemical symbol for this element.
6. Of the elements that have 2 valence electrons, which has the lowest atomic mass? What family is this element a part of?

34. P.T. Review
2. Vertical columns of elements are called groups/families. Horizontal rows are called periods.
3. True or False: Elements in the same row tend to have very similar chemical properties. False! Elements in the same column have very similar chemical properties!
4. What is the chemical symbol for the halogen in Period 4? Br
5. An element’s outermost electrons are found in the 5th energy level. The Lewis structure for the element shows four dots. Give the chemical symbol for this element. Sn
6. Of the elements that typically form ions with a +2 charge, which has the lowest atomic mass? What family is this element a part of? Be; part of Alkali Earth metals

35. Reactivity

36. Metal Reactivity Metals react by losing electrons.
Would it be easier to lose an electron from a smaller or larger atom??
Think about the shielding effect.

37. Reactivity increases as you go down a group of metals. Why?
Shielding effect! Lower elements have electrons further from the nucleus which are less firmly held and therefore more easily lost.

38. Reactivity decreases as you go left to right in a row of metals. Why?
Successive elements have more protons, but no “new” energy levels for electrons. “Extra” protons hold the electrons more tightly (helps that there’s no added shielding effect!).

39. Trend #2: Reactivity The most reactive metals tend to be located in the lower left hand corner of the periodic table. Why?
Metals react by losing electrons. The easier it is to lose electrons, the more reactive the metal.

40. Reactivity of Metals
Most Reactive Metal!! (Francium)

41. The most Reactive Metals

42. Agenda 11/6/14 Today’s Objectives: - Review P.T. Basics - Discuss Ions
- Ionization Energy
HW: Forming Ions Homework
Now: Find a partner for an activity

43. One answers, one explains…
Which has the smaller atomic radius?
Na or S ??

44. One answers, one explains…
Which exhibits the greater shielding effect?
F or I ??

45. One answers, one explains…
Which is the larger particle:
N or As ???

46. One answers, one explains…
Which is the most reactive:
Rb or Sr ???

47. One answers, one explains…
Which has 2 valence Electrons:
HE or Ca ???

48. Ionization Energy
The ability for an atom to gain or lose an electron. The ability for an atom to become an ion.

49. Metals v. Non-Metals Metals Lose electrons in order to become an ion
Gain electrons in order to become an ion
Would a smaller atom or a larger atom be able to attract an electron better?
Would a smaller atom or a larger atom be able to release an atom easier?

50. Shielding increases so the electrons are attracted less strongly!
Generally, ionization energy decreases from top to bottom within a family because….
Shielding increases so the electrons are attracted less strongly!

51. Extra protons in nucleus attract the Valence electrons more strongly!
Generally, ionization energy increases from left to right across a period because….
Extra protons in nucleus attract the Valence electrons more strongly!

52. Ionization Energy
Highest
I.E.
(Helium)

53. Agenda 11/7/14 Today’s Objectives: - Electronegativity Trend
- Review all other trends
- Reactivity Demo
COLLECT FORMING IONS
HW: Trends Packet
Now:Take out your Forming Ions Homework

54. Electronegativity
The ability for an atom to attract an electron. Can a smaller or larger atom attract an electron better? Think about shielding effect.

55. Generally, electronegativity tends to decrease from top to bottom in a group because….
As the size of the atom increases, the pull of the nucleus is less strong

56. Generally, electronegativity tends to increase from left to right in a row because….
The are more protons in the nucleus but the same number of energy levels.

57. Electronegativity Highest Electronegativity (Fluorine)
Note: Noble gases will not attract extra electrons!!

58. Agenda 11/10/14 Today’s Objectives: - Review the periodic trends
- White board review activity
- Periodic Table History Web Quest
HW: Unit 5 Review Packet due Wednesday
Now: Take out your homework from this weekend

59. Become the expert
You and your table will select a trend to become the expert on.
It is your job to study this trend from your notes and prepare a 2-3 minute presentation on your trend to the class.
You may use a whiteboard to organize your presentation.
Your presentation should include:
Definition of the trend
How the trend changes on the PT
How does the shielding effect or atomic size relate to your trend.
What is an example question that could be asked on a test about your trend?

60. The trends are… Reactivity of Metals Ionization Energy
Electronegativity
Atomic Radius
Shielding Effect

61. DURING PRESENTATIONS…
Add to your notes from in class.
Think about questions you might have about this trend for the group.
Work out the problems on a separate sheet of paper to turn in for credit.

62. History of the Periodic Table
Work in groups to answer the questions about each scientist.
This document will serve as your notes for this portion of the unit.
You are accountable to your classmates!

63. Acc Chem 3/13/14 Today’s Objectives: - Study for test tomorrow
H.W. Study for test tomorrow