1. Periodic Table: 4.23.14 Infinite Campus Update:
“Where do chemical elements come from” article (18pts.)
Periodic Table Worksheet (10pts.)
Periodic Table Basics Worksheet (15pts.)
Electron Configuration Exams (30pts.)
Homework:
Review electron properties and arrangement notes, review exam tomorrow.

2. Periodic Table Objectives
I can predict chemical reactivity for an element based on its number of valence electrons and location on periodic table.
I can distinguish between metallic and non-metallic properties.
I can graph and interpret periodic trends.
I can understand how the periodic table was organized by Mendeleev and Moseley.

3. Periodic Table and Valence Electrons
Due:
E- arrangement and Chemical Reactivity Wksht.
Objectives:
I can establish a relationship between the periodic table and valence electrons.
I can establish a relationship between the periodic table and chemical reactivity.

4. Periodic Table Objectives
I can predict chemical reactivity for an element based on its number of valence electrons and location on periodic table.
I can predict the charge for an element (ion) to reach maximum stability.
I can distinguish between metallic and non-metallic properties.
I can understand how the periodic table was organized by Mendeleev and Moseley.
I can graph and interpret periodic trends.
I can illustrate valence electrons using Lewis Dot structures.

5. Bell Ringer: Periodic Table
1. a. What period and group is sulfur on?
b. What element is in period 6; group 2 ?
2. Give an example of an element from the following groups:
Noble Gases, Transitional, Alkali, Halogens, Alkaline Earth
3. Circle the elements below that are representative: , Na, Cr, Ag, Kr, C, Sn
4. a. What are valence electrons?
b. Determine how many valence electrons each element below has:
a. H b. Se c. Sr d. Zn

6. Bell Ringer: Periodic Table
1. a. What period and group is sulfur on?
b. What element is in period 6; group 2 ?
2. Give an example of an element from the following groups:
Noble Gases, Transitional, Alkali, Halogens, Alkaline Earth
3. Circle the elements below that are representative: , Na, Cr, Ag, Kr, C, Sn
4. a. What are valence electrons?
b. Determine how many valence electrons each element below has:
a. H b. Se c. Sr d. Zn

7. Periodic Table: Organization of Elements
Groups: Represent columns on periodic table.
Periods: Represent rows on the periodic table.

8. Periodic Table and Groups
Transitional Groups:
Short groups.
Representative Groups:
Tall groups

9. Periodic Table and Valence Electrons
Objectives:
I can establish a relationship between the periodic table and valence electrons.
I can establish a relationship between the periodic table and chemical reactivity.

10. Valence Electron Worksheet

11. Lewis Dot Structures Illustrates valence electrons for an atom.
Place electrons (dots) around
the elements symbol using
cardinal direction.
Do NOT pair electrons
up until you have to.
Element
# of valence electrons
Lewis Dot Structure Na Mg S

12. Periodic Table: Arrangement
Valence Electrons:
Electrons on the highest energy level of an atom.
Determines chemical stability of an atom.

13. Common Periodic Table Groups
Periodic Groups
Group #
Valence Electrons
Chemical Reactivity
(Yes or No)
Alkali Metals
Alkaline-Earth Metals
Transitional
Metals
Halogens
Noble Gases
(Inert Gases)

14. ICP:
Objectives:
I can predict chemical reactivity for an element based on its location on the periodic table.
I can distinguish between metallic and non-metallic properties.

15. ICP:
Objectives:
I can predict chemical reactivity for an element based on its location on the periodic table.
I can distinguish between metallic and non-metallic properties.

16. Metallic vs. Non-metallic Properties
Brittle
Malleable
Conductors of heat and electricity
Insulators of heat and electricity
Transitional group
Noble gases
Halogens
Valence electrons
Alkali group
Groups have similar properties
Low luster
High luster
low density
High density
High melting point
Low melting point
Ductility
Primary gases at room temp.
Primary solids at room temp.
Alkaline earth group
stability

17. Metallic vs. Non-metallic Properties

18. Metallic vs. Non-metallic Properties

19. Common Periodic Table Groups
Periodic Groups
Group #
Valence Electrons
Chemical Reactivity
(Yes or No)
Alkali Metals
Alkaline-Earth Metals
Transitional
Metals
Halogens
Noble Gases
(Inert Gases)

20. Common Periodic Table Groups
Periodic Groups
Group #
Valence Electrons
Chemical Reactivity
(Yes or No)
Alkali Metals 1
1ve-
Yes, chemically reactive because they only has 1 ve-. Most reactive metallic group.
Alkaline-Earth Metals 2
2ve-
Yes , chemically reactive because they only have 2 ve-.
Transitional
Metals
3-12
2 ve-
Yes, chemically reactive because they only have 2 ve-.
Halogens 17
7ve-
Yes, chemically reactive because they only have 7ve-. Most reactive non-metallic group.
Noble Gases
(Inert Gases) 18
8ve-
No, not chemically reactive because they have the maximum number of ve-.
Most noble elements = 8 ve.
Exception: He = 2ve.
Most stable elements.

21. Chemical Stability Octet Rule:
Atoms will gain, lose, or share valence electrons to reach maximum stability.
What is maximum stability for most atoms?
8 valence electrons (ve-)
Exceptions: H and He max. stability = 2 ve-
How do atoms achieve stability ?
Atoms chemically bond with other atoms.
Formation of diverse compounds in nature.

22. Chemical Stability: Octet Rule
Will metals tend to gain or lose valence electrons to reach maximum stability?
Will non-metals tend to gain or lose valence electrons to reach maximum stability?

23. Chemical Stability: Octet Rule
Metals will lose ve- to reach stability.
Form a cation (+ charged)
Non-metals will gain ve- to reach stability.
Form an anion (- charged)

24. Chemical Stability Each of the elements below are neutral.
Determine if chemically stable by identifying what group it is in. (# of valence electrons)
If not stable, predict what charge it must have to reach stability.
a. Sodium
b. Oxygen
Argon
Phosphorus
e. Chromium

25. Chemical Stability-Key
Determine what type of charge each element below would form to reach maximum stability.
a. Sodium Na1+
b. Oxygen O2-
c. Argon Ar
d. Phosphorus p3-
Chromium Cr2+

26. Metallic vs. Non-metallic Properties
Brittle
Malleable
Conductors of heat and electricity
Insulators of heat and electricity
Transitional group
Noble gases
Halogens
Valence electrons
Alkali group
Groups have similar properties
Low luster
High luster
low density
High density
High melting point
Low melting point
Ductility
Primary gases at room temp.
Primary solids at room temp.
Alkaline earth group
stability

27. Metallic vs. Non-metallic Properties

28. Periodic Table: 11.5.14 Objectives:
I can predict chemical reactivity for an element based on its number of valence electrons and location on periodic table.
I can distinguish between metallic and non-metallic properties.
I can graph and interpret periodic trends.
I can understand how the periodic table was organized by Mendeleev and Moseley.

29. Chemical Stability: Octet Rule
Will metals tend to gain or lose valence electrons to reach maximum stability?
Will non-metals tend to gain or lose valence electrons to reach maximum stability?

30. Metals, Non-metals, Metalloids
Exhibits metallic and non-metallic properties
Depends upon what it is bonding with.
Most touch the staircase

31. Periodic Table: Exit Slip
Classify the following as either metallic (M) or non- metallic (NM)
insulator of heat high density ductility anion
Give an example of a metal, non-metal, and metalloid from the periodic table.
Determine if the following neutral elements need to become ions to reach maximum stability. If so, determine what charge they would have.
a. Al b. Br c. Ne d. Au

32. Periodic Table: 11.10.14 Objectives:
I can predict chemical reactivity for an element based on its number of valence electrons and location on periodic table.
I can distinguish between metallic and non-metallic properties.
I can predict what ion an element would become to reach stability.
I can graph and interpret electronegativity.

34. Periodic Trend: Electronegativity
Across a Period:
Down a Group:
mmsphyschem.com

35. Periodic Table: 11.11.14 Objectives:
Review electron arrangement and Periodic Table Trends
Set-up for Chemical Bonding Lab
Homework:
Review for exam-test tomorrow (Thursday)

36. Metallic vs. Non-metallic Properties
Brittle
Malleable
Conductors of heat and electricity
Insulators of heat and electricity
Transitional group
Noble gases
Halogens
Valence electrons
Alkali group
Groups have similar properties
Low luster
High luster
low density
High density
High melting point
Low melting point
Ductility
Primary gases at room temp.
Primary solids at room temp.
Alkaline earth group
stability

37. Electronegativity and Chemical Bonding
Do metals or non-metals have a greater electronegativity value?

38. Periodic Table: Exit Slip
Classify the following as either metallic (M) or non- metallic (NM)
insulator of heat high density ductility anion
Give an example of a metal, non-metal, and metalloid from the periodic table.
Determine if the following neutral elements need to become ions to reach maximum stability. If so, determine what charge they would have.
a. Al b. Br c. Ne d. Au

39. Gallery Walk Review content for exam.
Validate participation by recording answers on worksheet.

40. Review

42. Metals, Non-metals, Metalloids
Exhibits metallic and non-metallic properties
Depends upon what it is bonding with.
Most touch the staircase

43. Size of an Ion
Use the diagrams below to determine what happens to the size of a neutral atom(parent atom) when it becomes an ion.

44. Size of a Cation
Why is the cation smaller than its parent atom (neutral)?

45. Size of an Anion
Why is an anion larger than its parent atom?

46. Size of Ions Circle the atom that is larger in size. Ca or Ca2+
S or S2-
Circle the atom that is smaller in size.
a. Al or Al3+
b. N or N 3-

47. Periodic Table: 4.28.14 Objectives:
I can predict chemical reactivity for an element based on its number of valence electrons and location on periodic table.
I can distinguish between metallic and non-metallic properties.
I can graph and interpret periodic trends.
I can understand how the periodic table was organized by Mendeleev and Moseley.
I can illustrate Lewis Dot Structures using valence electrons.
Homework:
Review for exam: Wednesday

48. Periodic Trends: Atomic Radius
Across a Period
Down a Group

49. Periodic Table : Atomic Radius

50. Periodic Trends: Ionization Energy
Across a Period:
Down a Group:

51. Periodic Trend: Electronegativity
Across a Period:
Down a Group:
mmsphyschem.com

52. Electronegativity and Chemical Bonding
Do metals or non-metals have a greater electronegativity value?

53. Periodic Table: 4.29.14 Infinite Campus Update:
Valence Electron Lab (15pts.)
Periodic Trends Graph (14pts.)
Electron Configuration Exams (posted tonight)

54. Periodic Table: 4.29.14 Objectives:
I can predict chemical reactivity for an element based on its number of valence electrons and location on periodic table.
I can distinguish between metallic and non-metallic properties.
I can graph and interpret periodic trends.
I can understand how the periodic table was organized by Mendeleev and Moseley.
I can illustrate Lewis Dot Structures using valence electrons.
Homework:
Periodic Table Exam-tomorrow

55. History of the Periodic Table
Dmitri Mendeleev:
Russian chemist and teacher
When organized elements into groups by similar chemical properties,
he observed the periods increasing in atomic mass. (1869)
His organization system was successful at predicting undiscovered elements.
Do you observe any inconsistencies with his organization system?

56. History of Periodic Table
Henry Moseley:
British Physicists
Tweaked Mendeleev’s periodic table.
When elements were placed in groups by chemical properties, the periods consistently increased by atomic number. (1913)
Current organization of elements on the periodic table.

57. Periodic Table: 4.30.14 Objectives: Periodic Table Exam
I can predict chemical reactivity for an element based on its number of valence electrons and location on periodic table.
I can distinguish between metallic and non-metallic properties.
I can graph and interpret periodic trends.
I can understand how the periodic table was organized by Mendeleev and Moseley.
I can illustrate chemical bonding using Lewis Dot Structures.

58. Lewis Dot Structures Illustrates valence electrons for an atom.
Place electrons (dots) around
the elements symbol using
cardinal directions.
Do NOT pair electrons
up until you have to.
Element
# of valence electrons
Lewis Dot Structure Na Mg Si S He

59. Explain how this picture illustrates ionic bonding?

60. Ionic Bonding (Lewis Dot Transfer)
Metal
(Lewis Dot)
Non-metal
Ionic Bonding (Lewis Dot Transfer)
Chemical Formula