1 / 19

Quiz: Nov. 24

Quiz: Nov. 24. When you see a color in the flame test, what is happening? Describe the behavior of an electron according to the Bohr/Rutherford model? Which is more energetic, Yellow or Green light? List the colors of the rainbow in order. If n = 1, what energy level is the electron in?

ailish
Download Presentation

Quiz: Nov. 24

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Quiz: Nov. 24 • When you see a color in the flame test, what is happening? • Describe the behavior of an electron according to the Bohr/Rutherford model? • Which is more energetic, Yellow or Green light? • List the colors of the rainbow in order. • If n = 1, what energy level is the electron in? • Write the electron configuration for lithium Due Dates: Notebook: M 8th Period T 5th period W 11th period R 10th period F 4th period Essay: TODAY

  2. When you see a color in the flame test, what is happening? Describe the behavior of an electron according to the Bohr/Rutherford model? Which is more energetic, Yellow or Green light? List the colors of the rainbow in order. If n = 1, what energy level is the electron in? Write the electron configuration for lithium (3 electrons) The electron is dropping to a lower energy level. The electrons revolve around the nucleus. Green light is more energetic. ROY G BIV Red, Orange, Yellow Green, Blue, Indigo, Violet. n= 1, energy level = 1 1s22s1 Answers

  3. n=3 Electron Configuration n=2 n=5 n=4 n =1 • The electron configuration is used to quickly summarize the quantum numbers of electrons in the atom.. This quantum number is the shape of the electron cloud. Principal Quantum Number = Energy Level Number of Electrons in this orbital What are the s’s for? What are the superscript 2 and 1? What are these? Li = 1 s 2 2 s 1

  4. Electron Configurations 14 electrons 2 electrons 6 electrons 10 electrons #8 Start here #1 Hydrogen Helium = 1s2 1s1

  5. Electron Configurations 14 electrons 2 electrons 6 electrons 10 electrons #8 # 2 Start here #1 Lithium Beryllium = 1s2 2s1 2

  6. Electron Configurations 14 electrons 2 electrons 6 electrons 10 electrons #8 # 3 # 2 Start here #1 Nitrogen (7)= Carbon (6) = 2 3 Boron (5) = 1s2 2s2 2p

  7. Electron Configurations 14 electrons 2 electrons 6 electrons 10 electrons #8 # 3 # 2 Start here #1 Fluorine (9) = Oxygen (8) = Boron (5) = 1s2 2s2 2p 4 5

  8. Electron Configurations 14 electrons 2 electrons 2 s2 6 electrons 10 electrons 2 p2 #8 1s2 2 p2 2 p2 # 3 # 2 2 + 2 + 6 = 10 electrons TOTAL 2 e- 2 e- 6 e- Start here #1 Neon (10) = 1s2 2s2 2p6

  9. Write the electron configurations for Na (11), Mg (12), Al (13) 1s22s22p63s1 = Na 1s22s22p63s2 = Mg 1s22s22p63s23p1 = Al

  10. Electron Configurations 14 electrons 2 electrons 6 electrons 10 electrons #8 #4 # 3 # 2 Start here #1 1s2 3p3 Phosphorous 2s2 2p6 3s2

  11. Electron Configurations 14 electrons 2 electrons 6 electrons 10 electrons #8 #7 #6 #5 #4 # 3 # 2 Start here #1 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p6…..

  12. Write the electron Configuration for silver (47) and gold (79). • 1s22s22p63s23p64s23d104p65s24d9 • 1s22s22p63s23p64s23d104p65s24d105p66s24f145d9 Write the electron Configuration for iron and zinc. Fe ends in 3d6, Zn ends in 3d10

  13. orbital Hund’s Rule electron electrons • One in each before two in any. orbitals 2s 1s 2p Be = 4 N = 7 Ne = 10 H = 1 O = 8 He = 2 B = 5 Li = 3 C = 6 F = 9

  14. 6. e- =? n = 2 n = 3 n = 5 n = 7 7. sublevels =? n = 1 n = 3 n = 4 e- = 2(2)2 = 8 e- e- = 2(3)2 = 18 e- e- = 2(5)2 = 50 e- e- = 2(7)2 = 98 e- 7. n = 1, 1 sublevel n = 3, 3 sublevels n = 4, 4 sublevels Homework 16: 6  13 p 118…Honors: 32  34 p 133

  15. 8. orbitals/sublevel? s p d f 9. Define orbitals, list how many orbitals are in an f sublevel? 10. State Pauli’s exclusion principle. 8. s = 1 s orbital per sublevel p = 3 p orbitals per sublevel d = 5 d orbitals per sublevel f = 7 f orbitals per sublevel. 9. The space occupied by one pair of electrons is called an orbital. There are 7 f orbitals in a sublevel. 10.No two electrons in an atom can have the same set of 4 quantum numbers. Homework 16: 6  13 p 118…Honors: 32  34 p 133

  16. 11. List and explain each of the four quantum numbers. 12. If two orbitals are degenerate, what do they have in common? 13. How many sublevels will be found in level x? 11. n = the principal quantum number. It is equal to the energy level and describes the relative electron cloud size. l = shape quantum number, it describes the shape: s, p, d or f. m = the orientation in space of the electron cloud: x,y, z,… s = spin quantum number: + ½ or – ½ (clockwise or counter-clockwise) 12. Degenerate orbitals have the same amount of energy. 13. There will be x sublevels. Homework 16: 6  13 p 118…Honors: 32  34 p 133

  17. Homework 16: 6  13 p 118…Honors: 32  34 p 133 Level 1 # sublevels Letter(s) 32. Complete the chart. 33. What is an orbital, how many orbitals are possible at each sublevel. 34. Explain the factors that determine the size of an electron charge cloud. 1 1 s 2 2 s, p 3 3 s,p,d 4 4 s,p,d,f An orbital is the space that can be occupied by a maximum of two electrons; s = 1, p = 3, d = 5, f = 7e- = 2(2)2 = 8 e- The size of the electron cloud is determined by the principal quantum number, n, repulsion of other electrons and attraction to the nucleus.

  18. The electrons revolve around the nucleus like planets around the sun. Each electron has discrete quanta of energy. The amount of energy in one photon of energy equals one quantum E = h Where h = Plank’s constant = 6.6x10-34 Joules/Hz (1Hz = 1 cycle per second) Energy is given off in quanta, not continuously. The electrons surrounding the nucleus have defined orbits. In the Bohr-Rutherford Atom This relates to Lab 10

More Related