1. YOU WILL USE THE 4 SMALL TABLES TO LABEL Solids/Liquids/Gases Metal/Nonmetal/Metalloid # of Valence Electrons Group Names Ion Charges

2. LABEL YOUR PERIODIC TABLE: Energy Level

3. LABEL YOUR PERIODIC TABLE: # of Valence Electrons

4. LABEL YOUR PERIODIC TABLE: Metalsblue Non-metalsyellow Metalloidspink

5. LABEL ON YOUR PERIODIC TABLE Liquid blue Gasyellow Solid green

6. LABEL YOUR PERIODIC TABLE: Group Names 1 2 3-12 17 18

7. ATOMIC RADII PAGE 170

8. DEFINITION  The distance from the center of the nucleus to the furthest orbital in a neutral atom. Found using half the distance between two identical atoms bound together in a compound.

9. EXPLANATION  AR becomes smaller going right in a period because the nucleus has more positive pull holding the electrons closer.  AR becomes larger going down a group because there are more E levels.

10. TRENDS GROUP TREND  AR increases going down the group PERIOD TREND  AR decreases going right in a period

11. ATOMIC RADII

12. EXAMPLES Put the following elements in order of largest to smallest atomic radii: Mg, Cl, Na, P Order of AR:

13. EXAMPLES Put the following elements in order of largest to smallest atomic radii: Mg, Cl, Na, P Order of AR: Na>Mg>P>Cl

14. IONIC RADII PAGE 176

15. DEFINITION  The distance from the center of the nucleus to the furthest orbital in a charged atom.

16. EXPLANATION Recall that...  Positive ions are formed by the loss of electrons and are called cations. Cations are smaller than the original atom.  Negative ions are formed by the gain of electrons and are called anions. Anions are larger than the original atom.

17. TRENDS GROUP TREND  There is a gradual increase of ionic radii going down a group. PERIOD TREND The metals on the left of a period tend to form cations and the non metals tend to form anions.  Cationic radii decrease going right in a period.  Anionic radii also decrease going right across a period.

18. IONIC RADII

19. EXAMPLES  Put the following ions in order from largest to smallest radii  P 3- Cl - S -2  Sc 3+ K + Ca 2+

20. EXAMPLES  Put the following ions in order from largest to smallest radii  P 3- >S -2 >Cl -  K + >Ca 2+ >Sc 3+

21. Notes Atomic Radii Ionic Radii Periodic Table Vocabulary Complete Individual Periodic Table Trends Parts A & B of Scavenger Hunt practice problems

22. Notes Electronegativity Ionization Energy Periodic Table Vocabulary Complete Individual Periodic Table Trends Complete Parts A of Scavenger Hunt practice problems

24. IONIZATION ENERGY “STINGY ELEMENTS” PAGE 173

25. DEFINITION  Ionization energy is the amount of energy required to remove an electron from an element.

26. EXPLANATION  An electron can be removed from any atom using the appropriate amount of energy. Since most atoms want to look like a noble gas, it is easier for the metals to lose e and for the nonmetals to gain e. IE decreases down the group because the e in the last orbitals are further from the draw of the nucleus and thus easier to remove.

27. TRENDS GROUP TREND  Ionization energies decrease down the group PERIOD TREND  G 1 elements have the lowest IE in each period indicating that they lose e very easily.  G18 have the highest IE because they are stable and do not want to loose any e.  IE increases going right in a period.

28. IONIZATION ENERGY

29. EXAMPLE Put the following elements in order of largest to smallest ionization energy: Li, Ne, O Order of ionization energy:

30. EXAMPLE Put the following elements in order of largest to smallest ionization energy: Li, Ne, O Order of ionization energy:  Ne>O>Li

31. ELECTRONEGATIVITY “ATTRACTIVE ELEMENTS” PAGE 177

32. DEFINITION  Electronegativity is a measure of the ability of an atom in a chemical compound to attract electrons.

33. EXPLANATION  Atoms seek to have a full outer electron shell.  Elements close to having 8 electrons in their outer shell will be highly attractive to new electrons.  Elements far from having 8 electrons in their outer shell will be very unattractive to new electrons.

34. TRENDS GROUP TREND  Electronegativity tends to decrease going down most groups or remain about the same in other groups. PERIOD TREND  Electronegativity tends to increase going right in a period.

35. ELECTRONEGATIVITY

36. EXAMPLES  Put these elements in order from largest to smallest electronegativity: Na, P, Cl, Al

37. EXAMPLES  Put these elements in order from largest to smallest electronegativity: Na, P, Cl, Al Cl>P>Al>Na

38. ADDITIONAL INFORMATION  Noble Gases, Alkali metals, and Alkaline Earth Metals have extremely low electronegativities.  N, O, and the halogens are the most electronegative elements.

39. BLOCK PARTY !!! Complete Part A of Scavenger Hunt practice problems

40. BLOCK PARTY !!! Group Members should complete the previously agreed upon separate tasks Groups must begin assembling posters Make a list of tasks each member must complete over the weekend. Monday is the last workday.

41. Notes Electronegativity Ionization Energy Periodic Table Vocabulary Complete Individual Periodic Table Trends Turn in Parts A B & C of Scavenger Hunt practice problems