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Let’s go over PAGE 77-78

Let’s go over PAGE 77-78. #1. Name 2 elements in which the last electron(s) to be added are placed into s subshells . You could have named any elements in group 1A or group 2A. #2. How many electrons can be placed into the 2s subshell ?. 2.

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Let’s go over PAGE 77-78

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  1. Let’s go over PAGE 77-78

  2. #1. Name 2 elements in which the last electron(s) to be added are placed into s subshells. You could have named any elements in group 1A or group 2A

  3. #2. How many electrons can be placed into the 2s subshell? 2

  4. #3. Name 2 elements for which the last electron(s) to be added are placed into p subshells. You could have named any elements in group 3A, 4A, 5A, 6A, 7A or 8A

  5. #4. List all the elements with 6 electrons in the outermost p subshell. 8A: Neon, Argon, Krypton, Xenon, Radon

  6. #5. Name 2 elements for which the last electron(s) to be added are placed into the 3d subshell. Period 4, Groups 3-12

  7. #6. How many electrons can be placed into the 3d subshell? 10

  8. #7. Shade in the s-block, p-block, d-block and f-block with different colors of pen or pencil on the periodic table on the previous page. p s d f

  9. #8. A total of eighteen electrons can be placed in the 3rd shell. Explain why. 3s  2e- 3p  6 e- 3d  10 e- ________ 18 e-

  10. #9. How many subshells are in the 4th shell? 4: 4s, 4p, 4d, 4f

  11. #10. An electron configuration is a list of all the subshells that have electrons for a given element. Determine which element is associated with each electron configuration in the following table.

  12. #11. Refer to the following electron configuration and answer the questions below: 1s22s22p63s23p64s23d5 a) How many total electrons does this element have? 25 b) What element is this? Manganese (Mn) c) How many shells are represented? 4 d) How many subshells are represented? 7

  13. #13. Consider the noble gas shorthand notation in the table below: a) What do you think [He] and [Ar] stand for? The electron configuration up to that point.

  14. b) Use this shorthand notation to write the electron configurations for the elements in Group IIA, the alkaline earth metals). • Beryllium: [He] 2s2 • Magnesium: [Ne] 3s2 • Calcium: [Ar] 4s2 • Strontium: [Kr] 5s2 • Barium: [Xe] 6s2

  15. c) Explain why the elements in Group IIA have similar properties. They all have 2 electrons in their outer shell.

  16. d) Use this shorthand notation to write electron configurations on your handout for the elements in the third row from sodium to silicon. Na: [Ne] 3s1 Mg: [Ne] 3s2 Al: [Ne] 3s23p1 Si: [Ne] 3s23p2

  17. e) Explain why the properties of the elements change as you move across the row. They have different #s of valence electron.

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