1. Do Now 1/7/10 Explain IN COMPLETE SENTENCES why atoms are neutral in charge. HINT: think about the charges and numbers of the subatomic particles Reminder: Bring your book tomorrow!

2. No scores recorded! Must be made up by Mon after school! MissingPer. 5Per. 7Per. 8Per. 9 EG Quiz (12/14) May have not been scored yet! MichaelNoneAdrian Francisco Ramiro Jose Salgado Luis Salgado Eduardo Ch. 5/6 Exam (12/16) NoneAlvaro Desirae Osvaldo Ribelino Franco Waldemar Khadijah Louis Quiz yesterday Anyone absent yesterday

3. Do Now Discussion Atoms are neutral because they have equal numbers of protons and electrons. Protons are positively charged and electrons are negatively charged When equal in number, the charges cancel each other out.

4. Review: What is an ion? A single atom or groups of atoms with either a positive or negative charge. Cation: positively charged ion Remember: Cats purrrrr. Anion: negatively charged ion Think: If you are “anti” something, you are against it, or have a negative opinion of it.

5. How do Ions form? Ions form when atoms lose or gain valence electrons. Lose electrons = Make a CATION Gain electrons = Make an ANION NaNa +

6. Atoms want 8 e- in their valence shell so it is full.  This will give them the configuration of a noble gas Atoms lose, gain, or share e- in order to get 8 e- in their valence shell NaCl+Na + Cl+  - Cation, Like Ne Anion, Like Ar Octet Rule “octo” means 8

7. Trends in Ion Formation Groups 1, 2, 13 & sometimes 14 give their valence electrons away (lose) 1 2 1314 LiLi +  MgMg 2+  B  B 3+

8. Trends in Ion Formation Groups 15, 16, 17 take electrons (gain) 151617 P  P 3- O  O 2- F  F -

9. Trends in Ion Formation Group 18 doesn’t form ions (noble gases) They already have the lucky 8 electrons! 18

10. Example 1 What would be the ion for Calcium (Ca)? Group Gain/Lose electrons Charge 2 Lose 2+ Ion Ca 2+

11. Example 2 What would be the ion for Boron (B)? Group Gain/Lose electrons Charge 13 Lose 3+ Ion B 3+

12. Example 3 What would be the ion for Phosphorus (P)? Group Gain/Lose electrons Charge 15 Gain 3- Ion P 3-

13. Do Now for 1/8 (15 min) 1. Read the article that you should have grabbed from the table up front. 2. Answer questions 1-4 on your “Do Now” sheet.  Dictionaries are on the book cart. 3. When you are done, order all of your “Do Now” sheets from 11/17/09 until today, STAPLE them NEATLY, and put them in the HW bin.  If you do not have them with you today, turn all of them in (including today’s) on Monday. 4. Return the article NEATLY to the stack on the table.

14. Review from yesterday What would be the ion for Sulfur (S)? Group Gain/Lose electrons Charge 16 Gain 2- Ion S 2-

15. One more What would be the ion for Beryllium (Be)? Group Gain/Lose electrons Charge 2 Lose 2+ Ion Be 2+

16. Practice What group is Sodium in? What is the atomic #? How many:  Protons = ______  Electrons = ______ What is the e- configuration for Na? How many valence e- does Na have? Group 1 1 from the 3s block = 1 valence e- 1s22s22p63s11s22s22p63s1 11 Na 11 protons 11 neutrons Na needs to loose 1 e- to have a full outer shell! Cation

17. Practice What group is Fluorine in? What is the atomic #? How many:  Protons = ______  Electrons = ______ What is the e- configuration for F? How many valence e- does F have? Group 17 2 from the 2s block + 5 from the 2p block = 7 valence e- 1s22s22p51s22s22p5 9 9 9 F 9 protons 9 neutrons F needs 1 more e- to fill it’s outer shell! Anion

18. So what happens? F 9 protons 9 neutrons Na 11 protons 11 neutrons Na looses its single e- in the 3 rd energy level, donating it to F Na+ no longer has e- in the 3 rd energy level, but does have a full 2 nd energy level w/ 8 e- Has become a Na+ ion. F now has a full 2 nd energy level with a full 8 e-, and has become the F- ion. 1. What do you notice about the e- shell diagrams after the e- has been given to F? 2. What element has this e- configuration normally? + - Exit Slip – Respond on your “Do Now” sheet from today. Then turn all of your “Do Nows” in.

19. “Do Now” 1/11/10 Respond using complete sentences!! 1. Identify the number of protons in K and then identify the number of electrons in K.  The number of protons in K is 19.  The number of electrons in K is 19. 2. Identify the number of protons in K + and the number of electrons in K +.  The number of protons in K + is 19.  The number of electrons in K + is 18. 3. Is K + an anion or cation?

20. Periodic Trends (Ch. 6) Trends are:  Predictable ways in which something changes  Things that are commonly seen (think fashion trends) Atomic Radius  Trend in the size of an atom Ionic Radius  Trend in the size of ions of an atom when they have formed Ionization Energy  Trends in the amount of energy needed to remove a single e- from an atom Get ready for Cornell notes!!!

21. Atomic Radius An atom’s size is determined by the space occupied by its e- cloud  Remember: The e- cloud is the area around the nucleus where the orbitals containing the e- are. Size is measured by determining the size of the radius. Turn to p. 187, look at graphic Radius of:  Metals = ½ the distance between nucleus of 2 atoms next to each other in crystal form  Nonmetals = Distance between nuclei of 2 bonded atoms of the same element.

22. Turn to p.188 – Atomic Radius Generally decreases Generally increases When drawing arrows to show trends, always start from the upper right corner! Period 1, Group 1

23. What trend(s) do you notice as you move from left to right across the periods? Do you have more or less e- as you move from left to right? The size _________ because: Trends in periods The atomic radius gets smaller as you move from left to right Elements in the same period have the same highest (principal) energy level. e- AND protons are added (atomic # increases) Nucleus has more power to pull e- in principal energy level closer to nucleus (= smaller radius) decreases Less e-

24. Trends in groups What trend(s) do you notice as you move from top to bottom? Do you have more or less e- as you move from top to bottom? The atomic radius gets _________ because: The atomic radius gets larger as you move from top to bottom More larger Each atom has the same # of e- in their valence shell, but the highest (principal) energy level has increased by 1 each time you move down. (You would need to draw an additional shell around the nucleus.)

25. Examples Using only your notes and a periodic table, which would have a bigger radius? He / Ar K / Ar Fe / Br Ar K Fe Mg / SMg

26. Ionic Radius Size of radius of an atom after it has gained or lost e- to become stable  Remember: Stability is achieved by having a full valence shell. Size is measured by determining the size of the radius, same as for atomic radius. Turn to p. 190, look at graphic The ionic radius becomes:  Smaller = When e- are lost  Larger = When e- are gained e- gainede- lost

27. Ionic Radius, p. 190 Write down your thoughts in your notes: 1. What is happening between Groups 14 and 15 that accounts for the sudden increase in the size of the ionic radius?

28. Ionic Radius, p. 190 According to the image, Group 14 elements donate their 4 valence e-  Loosing e- = smaller radius Group 15 is gaining e- (only needs 3 to fill shell)  Gaining e- = larger radius

29. Ionization Energy Energy required to remove an e- from an atom  Only looking at energy required to remove valence e-, so those in the outermost shell or highest (principal) energy level. Think about how ions are formed (which groups give up e- and which ones take e-) and write down your thoughts to the following ?’s: 1. As you move from left to right, would you expect it to be easier or harder to remove valence e-? Why?? 2. As you move down a group, would you expect it to be easier or harder to remove valence e-? Why??

30. Graph showing Ionization Energy Look at the elements that are represented by the circles – Why do you think the amount of energy needed may have decreased for these? Think about what happens to the e- configuration … New energy sub- level (from s block to p block, etc.)

31. Ionization Energy cont. From left to right = Increase in the amount of energy (more needed)  As # of valence e- increases, more energy is needed  More protons to pull e- towards nucleus From top to bottom = Slight decrease in the amount of energy needed (less needed)  As atomic radius increases due to additional energy levels (more shells), e- are farther from the nucleus and it is harder for protons to hold on to them.

32. Trend in Ionization Energy