1. Day 4 3-6 1.Which of the following are larger? F OR S -2 2. Give all 3 reasons why (BE SPECIFIC!).

2. How is the periodic table arranged?

3. 1.Which of the following are larger? Ca OR Sr Cs OR Cs +1 Rb OR Ca +2

4. Partner Review 1. What element is in Group 17, Period 3? 2. What family of elements is the element above in? 3. How many valence electrons does it have? 4. Which is more reactive Ne or F?

6. Day 5 3-9 1.Why are Na and K both in group 1? 2.Why are Na and Mg both in period 3?

7. How is the periodic table arranged?

8. Electronegativity – ability to attract electrons in a bond Na—Cl … In the compound above electrons shift toward Cl because it is more electronegative! Notes page 6

9. What is electronegativity? How does it increase on the p. t. ? Electronegativity – ability to attract electrons in a bond

10. How does it increase on the p. t. ? In this bond: Mg—O, which way do elecs. Shift? WHY? O, > electroneg.

11. Metals Halogens Octet rule Ion Alkali metals Noble gases electronegativity Alkaline metals Atomic size Period 2

12. As of today, you should already have the following: Families colored in (page 168) Valence electrons marked +1, +2, -1,-2, and -3 ions marked Reactivity trend (front / back) Atomic size (front / back)

13. Added today: Electronegativity (front / back) Day 5 3-9

14. Valence electrons = 2 1 3 4 5 6 7 8 Ions = +1 +2-3 -2 -1 Atom size decreases Atom size increases Reactivity increases away from the middle Electronegativity increases from Fr to F

15. Read Section 6.3 and complete #s 18-25 on page 182