1. Standard: 1c Articles: 160 Mastering Concepts: 174 (41-53) Practice Problems: 162(7-9) Homework Cornell Notes: 6.2 Section Assessment: 162 (10-13) Labs: 170 1

2. Section 6-2 Section 6.2 Classification of the Elements Explain why elements in the same group have similar properties. valence electron: electron in an atom's outermost orbitals; determines the chemical properties of an atom Identify the four blocks of the periodic table based on their electron configuration. Elements are organized into different blocks in the periodic table according to their electron configurations.

3. Section 6-2 Organizing the Elements by Electron Configuration Recall electrons in the highest principal energy level are called valence electrons. All group 1 elements have one valence electron.

4. Section 6-2 Organizing the Elements by Electron Configuration (cont.) The energy level of an element’s valence electrons indicates the period on the periodic table in which it is found. The number of valence electrons for elements in groups 13-18 is ten less than their group number.

5. Section 6-2 Organizing the Elements by Electron Configuration (cont.)

6. Section 6-2 The s-, p-, d-, and f-Block Elements The shape of the periodic table becomes clear if it is divided into blocks representing the atom’s energy sublevel being filled with valence electrons.

7. Section 6-2 The s-, p-, d-, and f-Block Elements (cont.) s-block elements consist of group 1 and 2, and the element helium. Group 1 elements have a partially filled s orbital with one electron. Group 2 elements have a completely filled s orbital with two electrons.

8. Section 6-2 The s-, p-, d-, and f-Block Elements (cont.) After the s-orbital is filled, valence electrons occupy the p-orbital. Groups 13-18 contain elements with completely or partially filled p orbitals.

9. Section 6-2 The s-, p-, d-, and f-Block Elements (cont.) The d-block contains the transition metals and is the largest block. There are exceptions, but d-block elements usually have filled outermost s orbital, and filled or partially filled d orbital. The five d orbitals can hold 10 electrons, so the d-block spans ten groups on the periodic table.

10. Section 6-2 The s-, p-, d-, and f-Block Elements (cont.) The f-block contains the inner transition metals. f-block elements have filled or partially filled outermost s orbitals and filled or partially filled 4f and 5f orbitals. The 7 f orbitals hold 14 electrons, and the inner transition metals span 14 groups.

11. Standard: 1c Articles: 160 Mastering Concepts: 174 (41-50) Practice Problems: 162(7-9) Homework Cornell Notes: 6.2 Section Assessment: 162 (10-13) Labs: 170 11

12. Mastering Concepts: 174 (41-50) 41. Why do the elements chlorine and iodine have similar chemical properties? (6.2) They have the same valence electron configuration (s 2 p 5 ).

13. Mastering Concepts: 174 (41-50) 42. How are the numbers of valence electrons of the group A elements related to the group number? (6.2) The number of valence electrons equals the group number for group A elements.

14. 43. How is the energy level of an atom’s valence electrons related to the period it is in on the periodic table? (6.2) The energy level of an atom’s valence electrons equals its period number. Mastering Concepts: 174 (41-50)

15. 44. How many valence electrons do each of the noble gases have? (6.2) All noble gases have eight valence electrons, except for helium, which has two. Mastering Concepts: 174 (41-50)

16. 45. What are the four blocks of the periodic table? (6.2) s-, p-, d-, and f-block 46. In general, what electron configuration has the greatest stability? (6.2) ns 2 np 6, where n is the energy level Mastering Concepts: 174 (41-50)

17. 47. Determine the group, period, and block in which each of the following elements is located on the periodic table. (6.2) a.[Kr]5s 2 4d 1

18. 18 a.[Kr]5s 2 4d 1 [Kr] =36 s f d p Period Grou p 3B the group, period, and block

19. 47. a.Group:3B, period 5, d-block Mastering Concepts: 174 (41-53)

20. Mastering Concepts: 174 (41-50) 47. Determine the group, period, and block in which each of the following elements is located on the periodic table. (6.2) b. [Ar]4s 2 3d 10 4p 3

21. 21 [Ar]4s 2 3d 10 4p 3 [Ar] =18 s f d p Period Grou p 5A the group, period, and block [18+2+10+3=33

22. 47. b. Group-5A, period 4, p-block Mastering Concepts: 174 (41-50)

23. 47. Determine the group, period, and block in which each of the following elements is located on the periodic table. (6.2) c. [He]2s 2 2p 6

24. 24 [He]2s 2 2p 6 [He] =2 s f d p Period Grou p 8A the group, period, and block [2+2+6=1 0

25. 47. c. Group-8A, period 2, p-block Mastering Concepts: 174 (41-50)

26. 47. Determine the group, period, and block in which each of the following elements is located on the periodic table. (6.2) d. [Ne]3s 2 3p 1

27. 27 [Ne]3s 2 3p 1 [Ne] =10 s f d p Period Grou p 3A the group, period, and block [10+2+1=13

28. 47. d. Group-3A, period 3, p-block Mastering Concepts: 174 (41-50)

29. 48. Categorize each of the elements in problem 47 as a representative element or a transition metal. (6.2) Mastering Concepts: 174 (41-50)

30. 30 a.[Kr]5s 2 4d 1 [Kr] =36 Representative or transition [36+2+1=39 Representative or transition

31. 48. Categorize each of the as a representative element or a transition metal. (6.2) a.[Kr]5s 2 4d 1 transition element Mastering Concepts: 174 (41-50)

32. 32 [Ar]4s 2 3d 10 4p 3 [Ar] =18[18+2+10+3=33 Representative or transition

33. 48. b. [Ar]4s 2 3d 10 4p 3 representative element Mastering Concepts: 174 (41-50)

34. 34 [He]2s 2 2p 6 [He] =2 [2+2+6=1 0 Representative or transition

35. 48. c. [He]2s 2 2p 6 representative element Mastering Concepts: 174 (41-50)

36. 36 [Ne]3s 2 3p 1 [Ne] =10 [10+2+1=13 Representative or transition

37. 48. d. [Ne]3s 2 3p 1 representative element Mastering Concepts: 174 (41-50)

38. 49. Explain how an atom’s valence electron configuration determines its place on the periodic table. (6.2) Elements in a given column have the same number of valence electrons. The energy level of an atom’s valence electrons determines its period.

39. Mastering Concepts: 174 (41-50) 50. Write the electron configuration for the element fitting each of the following descriptions. (6.2)

40. 40 6s 5d 6p the metal in group 5A Noble gas=Xe 4f

41. Mastering Concepts: 174 (41-50) 50. a. the metal in group 5A Bi: [Xe]6s 2 4f 14 5d 10 6p 3

42. 42 3s 3p3p b. the halogen in period 3 Noble gas=Ne

43. Mastering Concepts: 174 (41-50) 50. b. the halogen in period 3 Cl: [Ne]3s 2 3p 5

44. 44 2s c. the alkali metal in period 2

45. Mastering Concepts: 174 (41-50) 50. c. the alkali metal in period 2 Li : [He]2s 1

46. 46 6s 5d transition metal that is a liquid at room temperature Noble gas=Xe 4f

47. Mastering Concepts: 174 (41-50) 50. d. the transition metal that is a liquid at room temperature Hg: [Xe]6s 2 4f 14 5d 10

48. Standard: 1c Articles: 160 Mastering Concepts: 174 (41-53) Cornell Notes: 6.2 Section Assessment: 162 (10-13) Labs: 170 Practice Problems: 162(7-9) 48

49. Practice Problems: 162(7-9) 7. Without using the periodic table, determine the group, period, and block of an atom with the following electron configurations. a.[Ne]3s 2 b. [He]2s 2 c. [Kr]5s 2 4d 10 5p 5

50. 7. Electron configuration Group Period Block a.[Ne]3s 2 2A 3s

51. 7. Electron configuration Group Period Block b. [He]2s 2 2A 2s

52. 7. Electron configuration Group Period Block c. [Kr]5s 2 4d 10 5p 5 7A 5 p

53. Practice Problems: 162(7-9) 8. Write the electron configuration of the element fitting each of the following descriptions. a.The group 2A element in the fourth period b. The noble gas in the fifth period c. The group 2B element in the fourth period d. The group 6A element in the second period

54. Practice Problems: 162(7-9) 8. Write the electron configuration of the element fitting each of the following descriptions. a.The group 2A element in the fourth period [Ar]4s 2

55. Practice Problems: 162(7-9) 8. Write the electron configuration of the element fitting each of the following descriptions. b. The noble gas in the fifth period [Xe]

56. Practice Problems: 162(7-9) 8. Write the electron configuration of the element fitting each of the following descriptions. c. The group 2B element in the fourth period [Ar]4s 2 3d 10

57. Practice Problems: 162(7-9) 8. Write the electron configuration of the element fitting each of the following descriptions. d. The group 6A element in the second period [He]2s 2 2p 4

58. Practice Problems: 162(7-9) 9. What are the symbols for the elements with the following valence electron configurations? a.s 2 d 1 Sc, Y, La, Ac b. s 2 p 3 b. N, P, As, Sb, Bi c. s 2 p 6 c. Ne, Ar, Kr, Xe, Rn