Ch 5 Electrons

1. Ch 5 Electrons • Use various atomic models to explain atomic behavior. • Use the periodic table for atomic information.

2. Quiz on beyond question • Mr. Burkholder, being the great guy that he is, will skip this quiz.

4. Rutherford’s atomic model did not explain complex properties of atoms

5. Bohr – e- could move to another energy level if it absorbed a quantum of energy

6. The modern atom Schrödinger, shape is based on probability of finding the electron. Pictures of the orbital shapes are on Page 131.

7. Lower energy orbitals fill up first.Look at pg 135, textbook.In what order will the orbits fill?

8. Energy order you need to memorize RED! (quiz?) (Slide 15 shows how to memorize) (1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s,4d,5p)s = 1 orbital p = 3 orbitals d = 5 orbitalsf = 7 orbitalsorbital = region of 90% high probability of finding an e-

9. Also look at page 131 of text book.

10. Electron configurations: the way e- are arranged in orbit around the nucleus of an atom The period table was arranged before they knew about e-. P.T. is arranged by physical properties.

11. Text Book Pg 131-2 shows orbital Pictures This website shows different combinations of orbitals: http://www.orbitals.com/orb/orbtable.htm Look at: s orbital: 1 shape p orbital: 3 same shape but different directions d orbital: 5 orbitals

12. 3 Rules for assigning electrons(w/o the exceptions)

13. 1. Aufbau principle: electrons enter orbitals of lowest energy firstRemember the quiz!!! (1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s,4d,5p)

14. Draw Orbitals of each principle energy level as a class. 7s…. 6s 6p 6d 6f 6g… 5s 5p 5d 5f 5g… 4s 4p 4d 4f 3s 3p 3d2s 2p 1s

15. (answers)Orbitals in each principle energy level. (Draw lines up and to the left to show lowest energy levels in order.)6s 6p 6d 6f 6g… 5s 5p 5d 5f 5g… 4s 4p 4d 4f 3s 3p 3d2s 2p 1s

16. (answers)Orbitals in each principle energy level. (Draw lines up and to the left to show lowest energy levels in order.)6s 6p 6d 6f 6g… 5s 5p 5d 5f 5g… 4s 4p 4d 4f 3s 3p 3d2s 2p 1s

17. (answers)Orbitals in each principle energy level. (Draw lines up and to the left to show lowest energy levels in order.)6s 6p 6d 6f 6g… 5s 5p 5d 5f 5g… 4s 4p 4d 4f 3s 3p 3d2s 2p 1s

18. (answers)Orbitals in each principle energy level. (Draw lines up and to the left to show lowest energy levels in order.)6s 6p 6d 6f 6g… 5s 5p 5d 5f 5g… 4s 4p 4d 4f 3s 3p 3d2s 2p 1s

19. (answers)Orbitals in each principle energy level. (Draw lines up and to the left to show lowest energy levels in order.)6s 6p 6d 6f 6g… 5s 5p 5d 5f 5g… 4s 4p 4d 4f 3s 3p 3d2s 2p 1s

20. (answers)Orbitals in each principle energy level. (Draw lines up and to the left to show lowest energy levels in order.)6s 6p 6d 6f 6g… 5s 5p 5d 5f 5g… 4s 4p 4d 4f 3s 3p 3d2s 2p 1s

21. (answers)Orbitals in each principle energy level. (Draw lines up and to the left to show lowest energy levels in order.)6s 6p 6d 6f 6g… 5s 5p 5d 5f 5g… 4s 4p 4d 4f 3s 3p 3d ETC. with 2s 2p the lines 1s Draw this in PP Notes

22. Pauli exclusions principle: an orbital may hold at most two electrons1s = 2e- max(1 orbital)2s = 2e- max 2p = 6e- max(2 x 3 orbitals) 3s = 2e- max 3p = 6e- max(2 x 3 orbitals) 4s = 2e- max 3d = 10e- max(2 x 5 orbitals)

23. Electron configurationsPut a little number (looks like an exponent) to show number of electrons in the orbital.Start by listing all orbitals. Fill in numbers until you hit number of e-.1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 1e- H 1s12e- He 1s210e- Ne 1s2 2s2 2p6 18e-Ar 1s2 2s2 2p6 3s2 3p6

24. Electron configurationsH 1s1He 1s2Ne 1s2 2s2 2p6Ar 1s2 2s2 2p6 3s2 3p6Question: F9e- F 1s2 2s2 2p52p5 =second principle energy level, p-orbitals, with 5 electronsWhat element ends with 3d7 = ?

25. Remember: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 Electron configurations 1s2 2s2 2p6 3s2 3p6 4s2 3d7 = 27e-Co Review:2p5 =second electron level, p shaped orbitals, with 5 electrons out of 6

26. Electron configurations: the way e- are arranged in orbit around the nucleus of an atom

27. 3. Hund’s rule: when e- occupy orbitals of equal energy, one e- enters each orbital until all the orbitals contain 1e- then they pair up. Make all the singles you can before pairing.

28. 3. Hund’s rule- when e- occupy orbitals of equal energy, one e- enters each orbital until all the orbitals contain 1e- then they pair up

29. 3. Hund’s rule- when e- occupy orbitals of equal energy, one e- enters each orbital until all the orbitals contain 1e- then they pair up

30. 3. Hund’s rule- when e- occupy orbitals of equal energy, one e- enters each orbital until all the orbitals contain 1e- then they pair up

31. 3. Hund’s rule- when e- occupy orbitals of equal energy, one e- enters each orbital until all the orbitals contain 1e- then they pair up

32. 3. Hund’s rule- when e- occupy orbitals of equal energy, one e- enters each orbital until all the orbitals contain 1e- then they pair up

33. 3. Hund’s rule- Please look at page 135.

34. 3 Rules for WOD:1. Aufbau principle : Fill lowest energy orbital first.1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s,4d,5p2. Pauli exclusions principle:2 max e- per energy orbiral level. (Each orbital has 0, 1, 2 e-)3. Hund’s rule: Make all the singles you can before making pairs.

35. Examples Do these in your Powerpoint notes. 1. How many unpaired electrons does sulfur have?2. What is the e- configuration of B?3. What is the e- configuration of Br? How many are unpaired?

36. Electron configurations1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 Sulfur has16e-1s2 2s2 2p6 3s2 3p4 So unpaired is 2 because p isBoron has 5e- 1s2 2s2 2p1Bromine has 35e- 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 1 unpaired

37. Electromagnetic Radiation

38. Electromagnetic Radiation:Electrons can change levels. When they drop, they produce electromagnetic radiation.See page 145 Bottom.Explained more in a few slides.

39. electromagnetic radiation– all light waves. microwaves, visible light, infrared and ultraviolet light…

40. Thermal imaging

42. Demo prism with OLD overhead projector light or mirror and sunlightor Computer Projector on this slide made best rainbow.Then have students look through diffraction gradient slides.

43. Wave

44. Wavelength, λ: distance between crests Frequency, f: number of wave cycles to pass a given point per unit of time(waves per second.)Hertz, Hz: Waves per Second (frequency)Amplitude: height of wave above zero or the middle.Crest: Top of waveTrough: Bottom of wave

45. to calculate frequency, c= speed of light 3.0x10 8 m/s f = c λ Frequency is speed of light divided by the wavelength

46. Calculate the frequency of a blue light emitted by a UV lamp. (λ= 9.76 × 10-8 m)f = c/ λ

47. Calculate the frequency of a blue light emitted by a UV lamp. (λ= 9.76 × 10-8 m) f = c/ λ f = 3.0 × 108 m/s / 9.76 × 10-8 m f = 3.07 × 1015 Hz

48. Show EM Brain Pop.Stop it 1min and have students copy EM spectrum.Stop again at Visible Light 2:10? and have students copy ROYGBIV.

49. Atomic Emission Spectrum:

50. Atomic emission spectrum: passing the light emitted by an element through a prism Each line is a specific energy of light. Each is unique to that element