1. ICP: Periodic Table Infinite Campus Update:
Nuclear Chemistry and Electron Arrangement Exam (33pts.)
Objectives:
I can classify elements as metals, non-metals, and metalloids.
I can classify elements based on the number of valence electrons.

2. Periodic Table: Locating Elements
Classify elements as metals, non-metals, and metalloids.

3. Periodic Table: Locating Elements
Periods:
Elements in the same row.
Groups:
Elements in the same column.
Have similar chemical properties.

4. Periodic Table : Bell Ringer
1. a. What period and group is Aluminum on?
b. What element is in period 4; group 2 ?
2. Circle the elements below that have similar chemical properties.
Carbon (C), Nitrogen, (N), Silicon (Si), Boron (B)
Classify the following as either a metal(M), non- metal (NM), or metalloid (MET)
a. H b. Si c. Al d. Sn e. Ar

5. ICP 12.2: Periodic Table Infinite Campus Update:
Nuclear Chemistry and Electron Arrangement Exam (33pts.)
Objectives:
I can classify elements as metals, non-metals, or metalloids.
I can classify elements based on the number of valence electrons.

6. Metallic vs. Non-metallic Properties

7. Periodic Table and Groups
Why do elements in the same group have similar chemical properties?

8. Periodic Table Lab: Group Patterns
grps
grp 1
ve-
grp 2
grp 13 ve-
grp 14
grp 15
grp 16
grp17
grp18 1. Li Be B C N O F Ne 2. Na Mg Al Si P S Cl Ar
Count the number of electrons on the highest
energy level and record in table above
Conclusion:

9. Periodic Table Lab: Group Patterns
grps
grp 1
ve-
grp 2
grp 13 ve-
grp 14
grp 15
grp 16
grp17
grp18 1. Li Be B C N O F Ne 2. Na Mg Al Si P S Cl Ar
Count the number of electrons on the highest
energy level and record in table above
Conclusion:

11. Periodic Table and Groups
Valence Electrons:
Electrons on the highest energy level.
Elements in the same group have the same number of valence electrons (why similar chemical properties).

12. ICP 12.9: Periodic Table Due: Periodic Table Worksheet
Infinite Campus Update:
Bohr’s model and valence electrons worksheet (10pts.)
Periodic Table: Bell Ringer (3pts.)
Periodic Table: Bell Ringer (7pts.)
Objectives:
I can classify elements as metals, non-metals, or metalloids.
I can predict chemical reactivity for an element based on its number of valence electrons and location on periodic table.
Homework:
Check infinite campus of missing assignments/exams

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

15. ICP 12.10: Periodic Table Objectives:
I can classify elements as metals, non-metals, or metalloids.
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 when it is stable.
Homework:
Check infinite campus of missing assignments/exams

16. Periodic Table Groups Check-up
1. Identify an element from each group below.
Noble Gases
Alkali Metals
Alkaline Earth Metals
Transitional Metals
Halogens
Representative Element
a. Which group from above is most stable?
b. Which metallic group above is most reactive?
c. Which non-metallic group above is most reactive?

17. Chemical Stability Octet Rule:
Atoms will gain or lose valence electrons to reach maximum stability.
Formation of ions.
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 bonding with other atoms.
Formation of diverse compounds in nature.

18. Chemical Stability Pattern
Metals tend to lose valence electrons to reach stability.
Non-metals tend to gain valence electrons to reach maximum stability?

19. Chemical Stability Pattern
Metals:
Will lose ve- to reach stability.
Form cations (+ charged atoms)
Non-metals:
Will gain ve- to reach stability.
Form anions (- charged atoms)

20. Chemical Stability
Determine what type of charge each element below would form to reach maximum stability.
a. Sodium
b. Oxygen
c. Argon
d. Phosphorus
Chromium

21. Chemical Stability: Charged Atoms
a. What do we call charged atoms? b. What do we call atoms with a positive charge? c. What do we call atoms with a negative charge?

22. Chemical Stability
Determine what type of ion each element below would form to reach maximum stability.
a. Sodium Na1+
b. Oxygen O2-
c. Argon Ar
d. Phosphorus P3-
Chromium Cr2+

23. Periodic Table: Homework
What element is on period 3 group 2 ?
Identify the elements below that are not representative elements:
Fe, S, Ca, Kr, Ag, U
3. Identify an element on the periodic table that has similar properties with oxygen.
a. What is the name of the group that Chlorine is in?
b. How many valence electrons does Cl have?
c. Will it gain or lose to reach maximum stability?
d. Identify the charge for Cl when it reaches maximum stability.
e. Is it classified as an anion or cation. Explain.

24. Periodic Table: Homework
What element is on period 3 group 2 ?
Identify the elements below that are not representative elements:
Fe, S, Ca, Kr, Ag, U
3. Identify an element on the periodic table that has similar properties with oxygen.
a. What is the name of the group that Chlorine is in?
b. How many valence electrons does Cl have?
c. Will it gain or lose to reach maximum stability?
d. Identify the charge for Cl when it reaches maximum stability.
e. Is it classified as an anion or cation. Explain.

25. Periodic Table: Homework
What element is on period 3 group 2 ?
Identify the elements below that are not representative elements:
Fe, S, Ca, Kr, Ag, U
3. Identify an element on the periodic table that has similar properties with oxygen.
a. What is the name of the group that Chlorine is in?
b. How many valence electrons does Cl have?
c. Will it gain or lose to reach maximum stability?
d. Identify the charge for Cl when it reaches maximum stability.
e. Is it classified as an anion or cation. Explain.

26. Periodic Table: Homework
What element is on period 3 group 2 ?
Identify the elements below that are not representative elements:
Fe, S, Ca, Kr, Ag, U
3. Identify an element on the periodic table that has similar properties with oxygen.
a. What is the name of the group that Chlorine is in?
b. How many valence electrons does Cl have?
c. Will it gain or lose to reach maximum stability?
d. Identify the charge for Cl when it reaches maximum stability.
e. Is it classified as an anion or cation. Explain.

27. Periodic Table: Valence Electrons
Lab
grps
grp 1
ve-
grp 2
grp 3-12
grp 13 ve-
grp 14
grp 15
grp 16
grp17
grp18 A 1 2 3 4 5 6 7 8 B C D
What can be concluded from the data table?

28. Common Periodic Table Groups
Periodic Groups
Group #
Valence Electrons
Chemical Reactivity
(Yes or No)
Alkali Metals 1
1ve-
Alkaline-Earth Metals 2
2ve-
Transitional
Metals
3-12
2 ve-
Halogens 17
7ve-
Noble Gases
(Inert Gases) 18
8ve-

29. 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)

30. 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.

31. Valence Electrons Post-Lab Qts.
Complete post-lab questions.

32. Metallic vs. Non-metallic Properties

33. Infinite Campus Update
Periodic Table Quiz (8pts.)
Periodic Table Worksheet (10pts.)
Due Today:
Valence Electron Lab (10pts)

34. Chemical Stability Pattern
Predict what type of ion, if any, each neutral element below would form to reach maximum stability. # of neutral/ion ve- max. stability a. Sodium b. Oxygen c. Argon d. Phosphorus e. Chromium

35. 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?

36. History of Periodic Table
Henry Moseley:
British Physicists
Observed that when elements were placed in groups by chemical properties, the periods consistently increased by atomic number. (1913)
Currently accepted organization system for elements.

37. Infinite Campus Update
Posted:
Valence Electron Lab (15pts)
Periodic Table Packet (10pts.)
*Reminder to complete ILPs by this Friday.

38. Bell Ringer: Atomic Stability
What is stability for an atom?
Why do many atoms prefer to be ions?
Identify each of the following atoms as a neutral, anion, or cation.
strontium has 36 electrons
bromine has 36 electrons
Predict, if any, what type of ion each atom below would become to reach stability.
a. Fe b. Rn c. I

39. Bell Ringer: Atomic Stability
What is stability for an atom?
Why do many atoms prefer to be ions?
Identify each of the following atoms as a neutral, anion, or cation.
strontium has 36 electrons
bromine has 36 electrons
Predict, if any, what type of ion each atom below would become to reach stability.
a. Fe b. Rn c. I

40. Periodic Table Trends 1. Define each term below related to an atom.
2. Graph data to determine the trend for each term below for an atom.
Atomic Radius
Ionization Energy
Electronegativity

41. Periodic Trend Graph Analysis
Analysis Procedures:
Locate elements in the same period.
Does the line graph increase or decrease with these elements in the same period.
2. Repeat step one, but with elements in a different period.
3. Locate elements in the same group.
Does the line graph increase or decrease with these elements in the same group?
Repeat step three, but with elements in a different group.
Share your results with your partners.

42. Periodic Properties and Trends
Atomic Radius:
-Size of an atom.
Distance from nucleus to highest energy level for that atom. (picometers, pm).
Ionization Energy:
Energy required to remove an electron from an atom.
Energy required to form a cation.
Electronegativity:
The attraction one atom has toward another atom’s valence electron.
Determines the type of chemical bond between atoms.

43. Periodic Table Trends 1. Define each term below related to an atom.
2. Graph data to determine the trend for each term below for an atom.
Atomic Radius
Ionization Energy
Electronegativity

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

47. Periodic Table : Atomic Radius

48. Periodic Trends: Ionization Energy

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

50. Periodic Trend Values
1. Use your atomic radius graph to rank the following elements in increasing atomic radius. Cl, Mg, Al, Na 2. Use your ionization energy graph to rank the following elements in decreasing ionization energy. Ba, Mg, Ca, Be

51. Periodic Trends: Atomic Radius

52. Periodic Trend Values
1. Use your atomic radius graph to rank the following elements in increasing atomic radius. Cl, Mg, Al, Na 2. Use your ionization energy graph to rank the following elements in decreasing ionization energy. Ba, Mg, Ca, Be

53. Periodic Trends: Ionization Energy

54. Periodic Trend: Electronegativity
mmsphyschem.com

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

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

58. Electronegativity and Chemical Bonding
Which compound has a greater electronegativity value difference? NaCl or CO

59. Chemical Bonding
Which compound has an ionic bond and which has a covalent bond? NaCl and CO
Ionic Bonding: NaCl
Between a cation(metal) and an anion (non-metal)
Electronegativity difference between atoms is large.
Transfer of valence electron(s).
Ionic Bond = Intramolecular Forces
Covalent Bonding: CO
Between two non-metals.
Electronegativity difference between atoms is small
Share valence electron(s)
Covalent Bond = Intramolecular Forces
Covalent compounds are also called molecules.

60. Ionic Bonding

61. Chemical Bonds: Intramolecular Forces
Physical Bonds: Intermolecular Forces .

62. Octet Rule Revised:
Atoms will gain, lose, or share valence electrons to reach stability.
The need for stability produces compounds (ionic and covalent)

63. Ionic or Covalent Compounds
H2O
BaCl2
FeO
C6H12O6

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

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

67. Size of a Cation A cation is smaller than its parent atom.
Why? Because metals will lose an energy level in the process
of becoming a cation.

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

69. Size of an Anion A anion is larger than its parent isotope.
Why? Repulsion force increases as more electrons are
added to the outer most energy level. Swells the energy level.

70. Size of an Anion

71. 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-

72. Ionic Bonding
Transfer of valence electrons from a metal atom to a non-metal atom.
Creates a metal ion and non-metal ion that are held together by electrostatic attractive forces (chemical bond)
Chemical bonds are intramolecular forces.
Formation of Ionic Compounds

73. Ionic Bonding

74. Intramolecular Forces
The chemical bonds within a single compound.

75. Ionic Bonding (Lewis Dot Transfer)
Metal
(Lewis Dot)
Non-metal
Ionic Bonding (Lewis Dot Transfer)
Chemical Formula Na Cl Al N Ca

76. Chemical Bonding
Lewis Dot Structures: Illustrates the number of valence electrons a neutral atom has prior to chemical bonding.

77. Hydrogen Lab