1. Ch 7 Ions Part A A. Representative Ions

2. Valence e- # Valence e- for representative elements – use group A group numbers Group # 1A2A3A4A5A6A7A8A # Ve-12345678

3. Lewis Dot Structure – Model to show Valence e- Do first round at 12,3,6,9 o’clock, then double up Example: Magnesium ___ Ve Mg Example: Fluorine ____ Ve F

4. Practice Lewis Dot Si N Fr Ar

5. Valence e- and stability The most stable Valence e- configuration is a full octet: noble gas configuration All other elements are unstable and use different strategies to get a full octet

6. Strategy A: Stealing e- Groups 5A, 6A, 7A will steal e- Then they are not neutral anymore protons ≠ electrons Example: Chlorine has ___ Ve- Needs to steal ____e- for full octet Net charge is now _____ Rewrite as Cl - top right corner is for ionic charges Called Anion (a negative ion)

7. Practice Anions Write the charge of the following anions Br O S P As

8. Strategy B: Losing Ve- Sometimes its easier to lose Ve- and expose the full octet underneath Example: Sodium has ____ Ve- It’s unlikely to steal somewhere 7 e-… Sodium loses ____ Ve- Net charge is ____ Rewrite as Na + Called a Cation (t is like a +)

9. Practice Cations Write the following elements as cations Be Al Ba K Li

10. Identify and write the ion symbols below 8p+ and 10e- ion: _______ 11p+ and 10 e- ion: _______ 3p+ and 2 e- ion: _______ 16p+ and 18e- ion: ______ 13+ and 10e- ion: ______

11. Warm-up 1. Name the ions for Phosphorus, Magnesium, Chlorine, Aluminum 2. Identify ionic charge and element: a)8p+ and 10e- ion: _______ b)11p+ and 10 e- ion: _______ c)16p+ and 18e- ion: ______ d)13p+ and 10e- ion: ______

12. Finding/naming cations Metals always form cations Naming: metal name followed by ion Ca 2+ : Calcium Ion

13. Ion Names Non-metals always form Anions Naming: drop ending (-ygen, -ogen, - ine, -ur, -orus, -ium, -ic) and replace with -ide ion Cl - (Chlor –ine) Chloride Ion

14. Write the name of the anions for____ Nitrogen Nitride ion Oxygen Oxide Ion Fluorine Fluoride Ion Phosphorus Phosphide Ion Sulfur Sulfide Ion

15. Chlorine Chloride Ion Arsenic Arsenide Ion Selenium Selenide Ion Bromine Bromide Ion Tellurium Telluride Ion Iodine Iodide Ion

16. Write the following elements as ions Be O N Li H

17. The rest of the PT Group 4A Non-Metals don’t ionize: too many to loose or too many to steal!!!! Noble Gases never ionize: have full octet Metalloids: some can form cations as well as anions…if asked, treat according to group number! Transition Metals: can form multiple ions, addtl info needed

18. Crash course chemistry isotopes and ions

19. Notes 7.B -Ionization Exceptions How many Valence e- does Carbon have? Will it steal or lose e-? Group 4A Non-Metals don’t ionize: too many to lose or too many to steal!!!! Noble Gases never ionize: have full octet Metalloids: some can form cations as well as anions…if asked, treat according to group number! Transition Metals: can form multiple ions, addtl info needed

20. Size of Ions Cations are smaller than their elements (lose a ring) Anions are larger than their element ( less charge effect: too many e- not enough protons)

21. Cations and Aufbau Diagram Magnesium 1s2, 2s2, 2p6, 3s2 Magnesium Ion 1s2, 2s2, 2p6

22. Anions and Aufbau Diagram Fluorine 1s2, 2s2, 2p5 Fluoride Ion 1s2, 2s2, 2p6

23. Corresponding Noble gases When elements ionize, they acquire Noble gas configuration Type of Ion Element Class Gain/loss of e- Correspo nding Noble Gas Example CationMetalsLose e-Noble gas from previous period Na → Ne AnionNon- Metals Gain e-Noble gas from end of same period O → Ne

24. Lewis Dot of Ions Draw the Lewis Dot of Cl Cl - Draw the Lewis Dot of Mg Mg 2+

25. Ionization Energy Def: Energy needed to remove a Valence e- Easy in elements with lots of shields Hard in elements with high charge effect Ionization energy increases

26. Highest/Lowest Ionization Energy Element with highest IE? Helium (yes you can remove an e- from He, it’s hard!) Element with lowest IE? Francium Which of the pairs below has a higher IE? Si or CNa or Cs F or Ga

27. Identify the element groups m