1. Periodic Table Trends Periodic Table Trends 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.

2. Chemistry 12.2 : Electron Configuration Chemistry 12.2 : Electron Configuration Infinite Campus Update: Nuclear Chemistry/Electron Configuration Study Guide- Gallery Walk Questions (17pts.) Nuclear Chemistry and Electron Configuration Exam(40pts.) Objectives: Review Nuclear Chemistry and Electron Configuration I can identify valence electrons using electron configurations. Homework: Review Worksheet for make-up exam- Due Wednesday.

3. Chemistry 12.2 : Electron Configuration Chemistry 12.2 : Electron Configuration Due: Nuclear Chemistry/Electron Configuration Study Guide- Gallery Walk Questions (17pts.) Infinite Campus Update: Nuclear Chemistry and Electron Configuration Exam(40pts.) Objectives: Review Nuclear Chemistry and Electron Configuration I can identify valence electrons using electron configurations. Homework: Review Worksheet for make-up exam- Due Wednesday.

4. Make-up Exam-Wednesday Make-up Exam-Wednesday Could earn ½ point back for missed questions on initial exam. Additional problems addressing electron configuration. (5pts.) Additional problems addressing radioactive decay graph and nuclear equations (alpha/beta). (5pts.) Review notes, quizzes, and study guide. Power Points (nuclear chemistry/electron configuration on my web-page). Study Guide Key on my web-page.

5. Periodic Table: Electron Configuration Periodic Table: Electron Configuration

6. Chemistry 12.3 : Electron Configuration Chemistry 12.3 : Electron Configuration Objectives: I can identify valence electrons using electron configurations. Homework: Electron Configuration Review sheet-due Wed. Study for make-up exam-Wed. Complete Short-Hand Configuration Worksheet

7. Chem I: Bell Ringer Chem I: Bell Ringer 1. Write the electron configuration for the neutral element, Nb (Niobium) using all four quantum numbers. 2. According to Hund’s Rule, how many unpaired electrons does Nb have? 3. According to the Pauli Exclusion Principle how many electrons can occupy a p-orbital at any time? a d-orbital at any time? 4. How many electrons are on the highest energy level for Nb? Bonus: What do chemist call electrons that occupy the highest energy level?

8. Periodic Table: Electron Configuration Periodic Table: Electron Configuration

9. Valence Electrons: Electrons on the highest energy level of an atom. Determines chemical stability of an atom.

10. Periodic Table: Short-Hand Configuration Periodic Table: Short-Hand Configuration Nb: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 3 Short-Hand Configuration:

11. Periodic Table: Short-Hand Configuration Periodic Table: Short-Hand Configuration Si: Cu:

12. Chemistry 12.3 : Electron Configuration Chemistry 12.3 : Electron Configuration Homework: Electron Configuration Review sheet-due Wed. Study for make-up exam-Wed. Complete Short-Hand Configuration Worksheet

13. Chemistry 12.4 : Electron Configuration Chemistry 12.4 : Electron Configuration Due: Electron Configuration Review sheet –place in tray Short-Hand Configuration Worksheet-keep Objectives: Make-up Exam(Nuclear/Electron Configuration) I can identify valence electrons using electron configurations. I can establish periodic table trends between valence electrons and chemical stability of an atom. Homework: Complete Short-Hand Configuration Worksheet

14. Chemistry 12.5 : Electron Configuration Chemistry 12.5 : Electron Configuration Due: Electron Configuration Review sheet –LATE Short-Hand Configuration Worksheet-analyze today Objectives: I can identify valence electrons using electron configurations. I can establish periodic table trends between valence electrons and chemical stability of an atom. Homework: Periodic Table Worksheet

15. Periodic Table: Organization of Elements Periodic Table: Organization of Elements Color code metals, non-metals, and metalloids. Groups: Represent columns on periodic table. Periods: Represent rows on the periodic table.

16. Periodic Table : Period vs. Group 1. a. What period and group is Aluminum on? b. What element is in period 4; group 2 ?

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

18. ICP 12.5 : Electron Configuration ICP 12.5 : Electron Configuration Due: Periodic Table Worksheet Objectives: I can identify valence electrons using electron configuration I can establish periodic table trends between valence electrons and chemical stability of an atom. Homework: Periodic Table Worksheet Periodic Table Quiz

19. Bell Ringer: Periodic Table 1. Classify each element as a metal, non-metal, or metalloid. a. As, b. Ar c. Mg 2. a. What element is on period 5, group 17? b. What period and group is Iodine on? 3. How many valence electrons does P have? 3. a. Which group has the most valence electrons? b. Do you predict that group is more stable or less stable than the other groups on the table?

20. Chemistry 12.9 : Periodic Table Trends Chemistry 12.9 : Periodic Table Trends Infinite Campus: Electron Configuration Review Sheet (12pts.) Make-up Exam (52pts.) Gallery Walk Study Guide(17pts.) 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 to reach stability. Homework: Periodic Table Worksheet Check Infinite Campus for missing assignments/assessments

21. Bell Ringer: Periodic Table 1. Classify each element as a metal, non-metal, or metalloid. a. As b. Ar c. Mg 2. a. What element is on period 4, group 12? b. What period and group is Iodine on? 3. Why do elements in the same group have similar chemical properties? 3. How many valence electrons does P have? 4. a. Which group has the most valence electrons? b. Do you predict that group is more stable or less stable than the other groups on the table? Explain.

22. Valence Electron Lab Valence Electron Lab Lab grps grp 1 ve- grp 2 ve- grp 3-12 ve- grp 13 ve- grp 14 ve- grp 15 ve- grp 16 ve- grp17 ve- grp18 ve- A122345678 B122345672 C122345678 D122345678 What can be concluded from the data table? Elements in the same group have the same number of valence electrons. (exception: He has 2 ve-) Transitional elements all have 2ve- As go across a period valence electrons increase by one. (exception: Transitional elements.)

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

24. Common Periodic Table Groups Common Periodic Table Groups Periodic GroupsGroup #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.

25. Chemistry 12.10 : Periodic Table Trends Chemistry 12.10 : Periodic Table Trends Due: Periodic Table Worksheet 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 to reach stability. Homework: Check Infinite Campus for missing assignments/assessments

26. Periodic Table Worksheet Check-up 1. Give an example of an element from the following groups: Noble Gases, Transitional, Alkali, Halogens, Alkaline 2. Circle the elements that are representative elements: Al, Fe, Br, Ag Explain how you know this. 3. Circle the elements below that have similar chemical properties: Explain how you know this. Carbon (C), Nitrogen, (N), Silicon (Si), Boron (B) 4. What is the name of the group of elements that are naturally stable?

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

28. Chemical Stability 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 bonding with other atoms. Formation of diverse compounds in nature.

29. Chemistry 12.11 : Periodic Table Trends Chemistry 12.11 : Periodic Table Trends Due: Metallic vs. Non-Metallic Properties Venn Diagram 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 to reach stability. I can distinguish between metallic and non-metallic properties. Homework: Check Infinite Campus for missing assignments/assessments

30. ICP 12.11 : Periodic Table Trends ICP 12.11 : Periodic Table Trends Objectives: I can distinguish between metallic and non-metallic properties. 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 to reach stability. Homework: Check Infinite Campus for missing assignments/assessments

31. Chemical Stability: Octet Rule Chemical Stability: Octet Rule 1. 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? www.teacherfurse.com http://www.green-planet-solar-energy.com/the-element-chlorine.html

32. Chemical Stability: Octet Rule 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) www.teacherfurse.com http://www.green-planet-solar-energy.com/the-element-chlorine.html

33. Chemical Stability 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 c. Argon d. Phosphorus e. Chromium

35. Chemical Stability-Key Chemical Stability-Key Determine what type of charge each element below would form to reach maximum stability. a. Sodium Na 1+ b. Oxygen O 2- c. Argon Ar d. Phosphorus p 3- e. Chromium Cr 2+

36. Metallic vs. Non-metallic Properties Metallic vs. Non-metallic Properties

39. Periodic Table: Bell Ringer Periodic Table: Bell Ringer 1. What element is on period 3 group 2 ? 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. 4. a. What is the name of the group that Nitrogen is in? b. What is the short-hand electron configuration of N? c. How many valence electrons does N have?

40. Chemistry 12.10 : Periodic Table Trends Chemistry 12.10 : Periodic Table Trends Due: Metallic vs. Non-Metallic Properties Venn Diagram 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 to reach stability. I can distinguish between metallic and non-metallic properties. I can understand how the periodic table was organized by Mendeleev and Moseley. Homework: Check Infinite Campus for missing assignments/assessments

41. 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?

42. 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) Currently accepted organization system for elements.

43. Bell Ringer: Atomic Stability Bell Ringer: Atomic Stability 1. What is stability for an atom? 2. Why do many atoms prefer to be ions? 3. Identify each of the following atoms as a neutral, anion, or cation. a. strontium has 36 electrons b. bromine has 36 electrons 4. Predict, if any, what type of ion each atom below would become to reach stability. a. Fe b. Rn c. I

44. Bell Ringer: Atomic Stability Bell Ringer: Atomic Stability 1. What is stability for an atom? 2. Why do many atoms prefer to be ions? 3. Identify each of the following atoms as a neutral, anion, or cation. a. strontium has 36 electrons b. bromine has 36 electrons 4. Predict, if any, what type of ion each atom below would become to reach stability. a. Fe b. Rn c. I

45. Periodic Table Trends 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 Trend Graph Analysis Periodic Trend Graph Analysis Analysis Procedures: 1. 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? 4. Repeat step three, but with elements in a different group. 5. Share your results with your partners.

47. Periodic Properties and Trends 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 during chemical bonding. - Determines the type of chemical bond between atoms.

48. Periodic Table Trends 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

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

50. Periodic Table : Atomic Radius

51. Periodic Trends: Ionization Energy Periodic Trends: Ionization Energy

52. Across a Period: Down a Group:

53. Periodic Trend Values 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

54. Periodic Trends: Atomic Radius

55. Periodic Trend Values 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

56. Periodic Trends: Ionization Energy Periodic Trends: Ionization Energy

57. Periodic Trend: Electronegativity mmsphyschem.com

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

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

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

63. Chemical Bonding 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.

64. Ionic Bonding Ionic Bonding

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

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

67. Ionic or Covalent Compounds Ionic or Covalent Compounds H 2 O BaCl 2 FeO C 6 H 12 O 6

69. Size of an Ion 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.

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

71. Size of a Cation 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.

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

73. Size of an Anion 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.

74. Size of an Anion Size of an Anion

75. Size of Ions Size of Ions 1. Circle the atom that is larger in size. a. Ca or Ca 2+ b. S or S 2- 2. Circle the atom that is smaller in size. a. Al or Al 3+ b. N or N 3-

76. Ionic Bonding 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

77. Ionic Bonding Ionic Bonding

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

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

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

81. Hydrogen Lab