1. Catalyst (Reg/Honors) Catalyst Questions ① Draw the Bohr Diagram for Lithium ②What charge would lithium form to become stable? ③Is the answer to #2 a cation or anion or none? ④ What is the name of the group that Lithium is found in. ① Draw the Bohr Diagram for Lithium ②What charge would lithium form to become stable? ③Is the answer to #2 a cation or anion or none? ④ What is the name of the group that Lithium is found in. To Do & Homework  Update your Table of Contents Homework: Study Guide Q’s 5-10; 14-16  Update your Table of Contents Homework: Study Guide Q’s 5-10; 14-16 T of C Unit 2: Atomic Theory and Periodic Table 98 Questions/Simulation Notes: Atomic Structure (Part 1) 10Flame Test LabNotes: Atomic Structure (Part 2) 11Atomic AccountantNotes: Period Table (Part 3) 12PT CardsNotes: Octet and Charges 13Secret Agent PuzzleNotes: Atomic Radius and Ionization Energy

2. Elements are classified by 1) metals, nonmetals, and semimetals. 2) Groups or families. (Group 1A, 2A, 3A) 3) Increasing atomic # or # of protons (NOT MASS!) Or Semimetals Color Code: Exception Hydrogen is a nonmetal

3. Metals are 1) Good conductors of heat and electricity. (Conductors- transfer matter) 2) Found on the left side of the periodic table Exception: Hydrogen (it’s a nonmetal)

4. Nonmetals are 1) poor conductors (insulators – don’t transfer matter). 2) Found on the right side of the PT

5. Semimetals are 1) In between metals and nonmetals on the PT, and have properties of both metals and nonmetals. 2) Touching the staircase with the exception of Al and Po. There are 7 of them: B, Si, Ge, As, Sb, Te, At. Si Ge Te Color code semimetals on PT found in 13R

6. Review Families of the Periodic Table

7. Alkali Metals Found in column 1A of the periodic table. They form 1+ ions by losing their one valence electron to satisfy the octet rule They react rapidly with water (H 2 O) Remember the explosions video clip? 2Na + 2H 2 O  H 2 + 2NaOH

8. Alkaline Earth Metals Are found in 2A family/column form 2+ ions in their compounds to satisfy the octet rule. They may lose their two valence electrons. Ca + 2H 2 O  H 2 + Ca(OH) 2

9. Halogens These elements always form -1 ions. They each have 7 valence electrons so they tend to gain one electron to satisfy the octet rule.

10. The Noble Gases Fully stable, satisfy the octet rule, and are typically unreactive. Xe He

11. More on Halogens Halogens that exist with a twin of itself are called diatomic elements. Cl 2 F 2 Mr. Brinclhof Br 2 I 2 N 2 Cl 2 H 2 O 2 F 2

12. Trends in the Periodic Table Trends in size, ionization energy, and electronegativity..

13. Memorize! Increasing Atomic Size or Atomic Radius Increasing Ionization Energy, and Electronegativity

14. Size The size (radius) of an atom shrinks as you go to the right of the periods/rows. But more protons are added, why is it shrinking then? But why? Think-pair-share Remember: Periods are horizontal rows. Groups or families are vertical columns.

15. Trends in Size The size of an atom is due to the size of the electron cloud. Know that there are attractions between the electrons and protons in the nucleus. (Opposite charges attract.)

16. Trends in Size Across: Atoms get smaller because there are more protons pulling the electrons toward itself making the size of the atom smaller. Down: The atoms get larger because there are more layers of electrons; more orbits. Each layer is further from the nucleus so there is less attraction between the nucleus and the valence electrons.  More protons  More layers

17. Sizes of Ions Each time an e- is removed, the ion becomes smaller because the nucleus can now further pull electrons toward itself making the ion smaller. Atoms that gain electrons become larger because the more electrons, the harder it is for the protons in the nucleus to attract those extra electrons. Electron Shielding Effect – Valence electrons become shielded from the positively charged nucleus as you add more electron orbits. This effect allows the atomic radius to increase moving down the periodic table. HONORS ONLY

18. Ionization Energy This is the amount energy needed to remove an electron. It is easier to remove an electron from a larger atom because the electron is farther from the nucleus and feels less attraction. If it’s easy to remove an e, would there be a high or low IE?

20. Try on own, share with partner after.  Order the elements from smallest to largest IE: potassium, cesium, lithium.

21. Try again on your own, then talk:  Order the elements from largest to smallest IE: Fluorine, Carbon, Oxygen.

22. Secret Agent Puzzle  Cut up the squares, throw trash in trash.  Organize the “periodic people” just like the PT is set up using PATTERNS.  Things to consider  Energy Levels  Electrons in each shell  Valence Electrons  Atomic Mass  Stability Homework: 5-10; 14-16 You should have at least 5-10 done in class today Further Instructions: 1)Order them like a PT 2)Assign an element to each person 3)Paste people on back of instructions paper sideways 4)TAPE entire sheet on page 13L

23. 1. Order the following elements from smallest atomic radius to largest atomic radius: Arsenic, Gallium, Germanium. 2. Which element has a larger ionization energy, fluorine or selenium? 3. Why does germanium have a higher ionization energy than lead? EXIT TICKET

24. Catalyst (Reg/Honors) Catalyst Questions ① What are transitional metals? ②Define ionization energy ① What are transitional metals? ②Define ionization energy To Do & Homework  Update your Table of Contents  Pass up your study guides. Homework:  Update your Table of Contents  Pass up your study guides. Homework: T of C Unit 2: Atomic Theory and Periodic Table 12PT CardsNotes: Octet and Charges 13Secret Agent PuzzleNotes: Atomic Radius and Ionization Energy 144 Square Graphic OrganizerElectronegativity

25. Podcast 4 Square (14L) Distinguish between metals and nonmetals. Atomic Radius (WHAT, TREND, WHY) Ionization Energy (WHAT, TREND, WHY)Electronegativity (WHAT, TREND, WHY)

26. Electronegativity

28.  Electronegativity is the measure of the ability of an atom to attract electrons.

29. Electronegativity Trends  As you go up a group, the electronegativity of an element increases.  As you go across a period towards the right, the electronegativity of an element increases.

31. Why Electronegativity Decreases Down a Group  As you go down a group more orbits are added.  Electron Shielding – Valence electrons become shielded from the positively charged nucleus as you add more orbits.  Electroneg. decreases because there is a decreased ability of the nucleus to attract electrons because of larger distance.

32. Why Electronegativity Increases Across a Period  As you move to the right, you add more protons.  The more protons, the attracted the electrons to the nucleus so it’s harder for electrons to be removed so elements must have a high electronegativity as you move to the right.

33. By yourself, then partner talk:  Order the elements from smallest to largest electronegativity: oxygen, beryllium, lithium,

34. Try again  Order the elements from largest to smallest electronegativity: chlorine, bromine, fluorine

35. Memorize! Increasing Atomic Size or Atomic Radius Increasing Ionization Energy, and Electronegativity

36. Based on your notes for 13R and today’s notes on 14R  Create 1 high level question based on notes from 13R  Create 1 high level question based on 14R notes  Write the question and the answer on your flashcard. Doesn’t matter where. Sentence Starters:  Compare and contrast  Predict what would happen if…  Why does the following occur as….  What allows…..

37. Quiz, Quiz, Trade  Step 1: Form an outer and inner circle.  Step 2: People on the outside will rotate to the left upon sound of a bell.  Step 3: Ask Question, if time permits, other person asks question.  Step 4: Quiz, rotate, quiz, rotate, trade  Don’t just give out the answer.  Ask probing questions; give hints.  Use the periodic table/illustrations

38. Letter to Mr. Narez Mr. Narez fell down the stairs, hit his head on the wall and experienced memory loss. He forgot what he knew about periodic trends such as atomic radius (size), ionization energy and electronegativity. You are to teach Mr. Narez all of this in detail so we can finish the unit. The requirements of the letter are found on the right side: Letter to Mr. Narez Mr. Narez fell down the stairs, hit his head on the wall and experienced memory loss. He forgot what he knew about periodic trends such as atomic radius (size), ionization energy and electronegativity. You are to teach Mr. Narez all of this in detail so we can finish the unit. The requirements of the letter are found on the right side: Criteria for Success:  What is atomic radius?  What is EN and IE?  Why does size decrease moving to the right of the PT?  Why does size increase going down?  Why does EN and IE increase going up?  If EN goes up, why must IE increase too?  Include illustrations If you have a what, make sure you elaborate with a WHY. Refer to pictures to help Mr. Narez. Done early? Start Practice Questions Criteria for Success:  What is atomic radius?  What is EN and IE?  Why does size decrease moving to the right of the PT?  Why does size increase going down?  Why does EN and IE increase going up?  If EN goes up, why must IE increase too?  Include illustrations If you have a what, make sure you elaborate with a WHY. Refer to pictures to help Mr. Narez. Done early? Start Practice Questions Plagiarism by copying straight from a website or your teacher’s notes will result in an NP

39. Exit Ticket 1. Define ionization energy. 2. Define electronegativity. 3. Order from largest to smallest electronegativity: Ca, Se, Ni 4. Order from smallest to largest atomic radius: O, Po, S 5. If electronegativity is high, do you think ionization energy would be high or low? Justify with evidence and scientific language.