1. 1. Have the rest of the homework packet on periodic table trends out to be stamped 2. Take 5 minutes to prepare for the quiz by answering the questions on the board. **Lab Thurs/Fri – have comp. book **Test next Thursday/Friday

2. Part 1: 1. Elements on the left side of the periodic table have a larger radius because there are LESS protons so they pull on the outer shells LESS making the atom bigger 2. Elements on the bottom of the periodic table have more shells so their radius is larger 3. A. Lithium – less protons, less pull B. Barium – more shells

3. Part 2: 1. Elements on the right side of the periodic table have a higher ionization energy because they have MORE valence electrons meaning it is HARDER to pull them away. They are closer to a full shell or stability 2. Elements on the top of the periodic table have a higher ionization energy because they have less shells so electrons are closer to the nucleus and HARDER to pull away 3. A. Chlorine – more valence e-, harder to take away B. Beryllium – less shells, e- closer to nucleus, harder to take away

4. Part 3: 1. Elements on the right side of the periodic table have a higher electronegativity because they have more valence electrons and their desire for more is high 2. Elements on the top of the periodic table have a higher electronegativity because they have less shells making the outer electrons MORE attracted to the nucleus 3. A. Fluorine – less shells, e- more attracted to nucleus B. Bromine – more valence e-, wants more

5. Atomic Radius – size of atom 1. Find the elements on the periodic table 2. If Left – Right  look at # of protons a. More protons = more pull = smaller radius b. Less protons = less pull = larger radius 3. If Up – Down  look at # of shells a. More shells = larger radius b. Less shells = smaller radius

6. Ionization Energy – energy needed to remove e- 1. Find the elements on the periodic table 2. If Left – Right  look at # of valence electrons a. More valence electrons = harder to pull away = higher ionization energy b. Less valence electrons = easier to pull away = lower ionization energy 3. If Up – Down  look at # of shells a. More shells = lower ionization energy because electrons farther from nucleus (easier to remove) b. Less shells = higher ionization energy because electrons closer to nucleus (harder to remove)

7. Electronegativity – desire for or attraction to electrons 1. Find the elements on the periodic table 2. If Left – Right  look at # of valence electrons a. More valence electrons = more attracted to electrons = higher electronegativity b. Less valence electrons = less attracted to electrons = lower electronegativity 3. If Up – Down  look at # of shells a. More shells = lower electronegativity because electrons farther from nucleus (not as attracted) b. Less shells = higher electronegativity because electrons closer to nucleus (more attracted)

8. Friday 4-5pm

10. Test next Thurs/Fri will cover: Scientists (4) – who did what and discovered what Atomic structure – p+, n 0, e

11. 1. Grab a pair of headphones IF YOU DON’T HAVE ANY 2. What was the hardest thing about the quiz on Wednesday? 3. What was the easiest thing? 4. What will you do to prepare better next time, if need be? **Pass back quizzes **Test next Thurs/Fri

12. 1. Bellwork from last two weeks 2. Periodic table groups note taker (stamped) 3. Homework: periodic table groups.

13. Station 1 – Small group instruction I will be calling a few students aside to work on problems with me Station 2 – Independent You will be working on an EduCanon video silently by yourself with headphones (see instructions on the board)

15. Fill us in: 1. What were the three groups discussed in the video? 2. What are the major differences between metals and nonmetals as discussed in the video? 3. Those of you who did not see the video, what would you predict the properties of metalloids (or semi-metals) to be?

16. You will be testing three different samples for the characteristics described in the video. Objective: You will be able to identify a substance as a metal or a nonmetal given specific properties of that substance.

17. CharacteristicsSample 1: Battery Sample 2: PencilSample 3: Copper Wire Is it malleable? Is it ductile? Is it brittle? Does it conduct electricity? Does it conduct heat? It is a metal or nonmetal? ***Use the information on the board in green box when using the multi-meters***

18. Characteristics to think about: 1. Malleable – can it be hammered or pressed permanently out of shape without cracking? 2. Ductile – can it deform under stress without cracking? 3. Brittle – does it crack easily? 4. Conductivity – does it conduct electricity or heat? Use voltage meter to test this 5. Shiny – does it reflect light?

19. They have intermediate properties of metals and nonmetals Blue zig-zag section on the periodic table Those of you who did not see the video, label each section of the periodic table as metal, nonmetal or metalloids

21. Check your neighbor’s periodic table and make sure each section is appropriately labeled. Thumbs up if the property is metal, thumbs down if nonmetal: 1. Conducts electricity 2. Lustrous – shiny 3. Poor conductor of heat 4. Brittle and breaks easily 5. Malleable – bends easily 6. Dull in appearance