1. Periodic Table Trends

2. Remember these groups of the periodic table?

3. Organization by atomic # = repeating patterns in chem and physical behavior

4. He 2 Ne 10 Ar 18 Kr 36 Xe 54 Rn 86 1s21s2 1s 2 2s 2 2p 6 1s 2 2s 2 2p 6 3s 2 3p 6 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 6p 6 How the configurations of the noble gases similar? The outer energy level is completely full!

5. 1s11s1 1s 2 2s 1 1s 2 2s 2 2p 6 3s 1 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 1 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 1 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 6p 6 7s 1 H 1 Li 3 Na 11 K 19 Rb 37 Cs 55 Fr 87 How are the configurations of the alkali metals similar? They all end in s 1

8. patterns in e - config = patterns in properties= Periodic Trends.

10. Rings/orbits/ shells: “how far out the e - cloud spans” More E levels= valence e - further away from nucleus

12. 1. Ca or Ge 2. Al or Ba 3. Fr or Cl

13. How strong is the nucleus? More p + = greater charge= e - pulled closer

15. 1. Na or Rb 2. Ca or Se 3. S or Mg 4. Li or O

16. + Nuclear charge Inner e - BLOCKS Valence e- from the nuclear charge( p+) b/c  E Level

18. 1. Na or Rb 2. Sn or C 3. Br or F

20. + E level Top of a group No  in E level  nuclear charge =  p + = stronger nucleus = valence e - are pulled closer

21. Atomic Radius ( under flap)

22. Atomic Radius

23. 1. Li or Cs 2. Ga or B 3. O or C 4. Be or Ba 5. Si or S

25. Gain, lose, or share e - to be STABLE like Noble gases s 2 p 6 **Exception energy level 1

26. Cation (+) loses e - = more p + than e - GroupmustCharge 1loses 1 e - 1+ 2Loses 2 e - 2+ 13Loses 3e - 3+ Anion (-) gains e - = more e - than p + Groupmustcharge 15Add 3 e - 3 - 16Add 2 e - 2 - 17Add 1e - 1 - Add or Lose e - based on what's EASIER

27. 1. becomes Smaller 2. Lose valence e -, lose E level 3. More nuclear charge

28. Atom Ion Losing e - Lost E level

29. 1. becomes Bigger 2. Gain valence e - 3. Less nuclear charge, weaker nucleus

30. Atom Ion add e - Same #p + BUT more e -

31. NonMetalMetal

32. 1. Al 3+ or P 3- 2. K + or Cs + 3. O 2- or Te 2-

33. Energy needed to remove ONE e -

34. Top of a group Bigger = valence e - farther away= less E (easier) to remove e - lower IE Closer to being noble gas = more E (harder) to remove e - higher IE Ionization Energy

37. 1. Na or S 2. Mg or Ba 3. Ga or Br 4. P or Bi

38. Electronegativity: BONDEDWANT likelihood BONDED atom WANT to take e - from another atom Like tug of war

39. Electronegativity

40. More E level & more e - = less likely to want more e - closer to being a noble gas = wants an e - Top of a group higher electroneg Lower electroneg

42. 1. Na or Mg 2. K or Br 3. F or Br 4. Ca or Ga 5. Li or S 6. Br or As

43. Shielding is constant Atomic Radius decreases Ionization energy increases Electronegativity increases Nuclear charge increases Shielding increasesAtomic radius increasesIonization energy decreasesElectronegativity decreases

44. SAMPLE PROBLEM Ranking Elements by Atomic Size PLAN: SOLUTION: PROBLEM: Using only the periodic table (not Figure 8.15), rank each set of main group elements in order of decreasing atomic size: (a) Ca, Mg, Sr(b) K, Ga, Ca(c) Br, Rb, Kr(d) Sr, Ca, Rb Elements in the same group increase in size and you go down; elements decrease in size as you go across a period. (a) Sr > Ca > Mg These elements are in Group 2A(2). (b) K > Ca > Ga These elements are in Period 4. (c) Rb > Br > Kr Rb has a higher energy level and is far to the left. Br is to the left of Kr. (d) Rb > Sr > Ca Ca is one energy level smaller than Rb and Sr. Rb is to the left of Sr.

45. SAMPLE PROBLEMRanking Elements by First Ionization Energy PLAN: SOLUTION: PROBLEM:Using the periodic table only, rank the elements in each of the following sets in order of decreasing IE 1 : (a) Kr, He, Ar(b) Sb, Te, Sn(c) K, Ca, Rb(d) I, Xe, Cs IE decreases as you proceed down in a group; IE increases as you go across a period. (a) He > Ar > Kr (b) Te > Sb > Sn (c) Ca > K > Rb (d) Xe > I > Cs Group 8A(18) - IE decreases down a group. Period 5 elements - IE increases across a period. Ca is to the right of K; Rb is below K. I is to the left of Xe; Cs is further to the left and down one period.