1. Chapter 4 The Modern Model of the Atom

2. The Puzzle of the Atom  Protons and electrons are attracted to each other because of opposite charges  Electrically charged particles moving in a curved path give off energy  Despite these facts, atoms don’t collapse  HMMMMM  The answer is in the light

3. c = c = speed of light, a constant (3.00 x 10 8 m/s) = frequency, in units of hertz (Hz, sec -1 ) = wavelength, in meters Electromagnetic radiation propagates through space as a wave moving at the speed of light.

4. Long wavelength, low frequency Short wavelength, high frequency

5. Types of electromagnetic radiation:

6. …produces all of the colors in a continuous spectrum Spectroscopic analysis of the visible spectrum…

7. Example Calculate the frequency of yellow light that has a wavelength of 559 nm (nanometers)

8. E = h E = Energy, in units of Joules (kg·m 2 /s 2 ) h = Planck’s constant (6.626 x 10 -34 J·s) = frequency, in units of hertz (hz, sec -1 ) = frequency, in units of hertz (hz, sec -1 ) The energy (E ) of electromagnetic radiation is directly proportional to the frequency ( ) of the radiation.

9. Alternate Equation E = hc/ E = Energy, in units of Joules (kg·m 2 /s 2 ) h = Planck’s constant (6.626 x 10 -34 J·s) c = Speed of Light (3.00x10 8 m/s) = Wavelength (meters) = Wavelength (meters)

10. Example What is the energy associated with yellow light at 559nm? Orange light at 633nm?

11. Long Wavelength = Low Frequency = Low ENERGY Short Wavelength = High Frequency = High ENERGY Wavelength Table

12. Problems o p. 154 #'s 30,31,38,40 include frequency

13. …produces all of the colors in a continuous spectrum Spectroscopic analysis of the visible spectrum…

14. …produces a “bright line” spectrum Spectroscopic analysis of the hydrogen spectrum…

15. But What Does It Mean? Well, it means there are only certain energies available in an atom. Of course! Energy is “quantized” –Only certain energies are allowed –Ex Cars can only travel at certain speeds

16. Bohr’s Model of the Atom Electrons can circle the nucleus only in allowed paths or shells The energy of the electron is greater when it is in a shell further from the nucleus (excited state) The atom achieves the ground state when electrons occupy the closest possible positions around the nucleus Electromagnetic radiation (light) is emitted when electrons move closer to the nucleus

17. Bohr’s Model cont. Each shell can hold a specific number of electrons –2n 2 where n is the shell number 1,2,3. 1 st shell = 2 electrons 2 nd shell = 8 electrons 3 rd shell = 18 electrons 4 th shell = 32 electrons –Elements in the same group on the periodic table must have the same number of electrons in the outer shell

19. Time to Draw! Draw a Bohr atom for Lithium-7 and Sodium-23 –Is there anything similar/different about the atoms?

20. The Bohr Model of the Atom Neils Bohr Electrons can jump from a lower shell to a higher shell by gaining a specific amount of energy. Electrons give off a specific frequency of light when they return to a lower shell

21. Another Example Bohr’s Model Applet http://www.colorado.edu/physics/2000/qua ntumzone/bohr.htmlhttp://www.colorado.edu/physics/2000/qua ntumzone/bohr.html

22. This produces bands of light with definite wavelengths. Electron transitions involve jumps of definite amounts of energy.

23. Energy Values for Shells Shell 1 = 1.0 eV Shell 2 = 11.2 eV Shell 3 = 13.1 eV Shell 4 = 13.8 eV Shell 5 = 14.1 eV Shell 6 = 14.2 eV –1 eV = 1.602x10 -19 J Why such a small change in outer shells?

24. Homework P. 155 #’s 41,45,48,52,55,56

25. A) Calculate the wavelength of light (nm) associated with an electron transition from the n=5 shell to n=2 shell. B) What color of light is this? C) How would this transition compare to n=5 to n=1?

26. Types of electromagnetic radiation:

27. So this is the model of the atom? No. There are a couple problems. 1.Bohr’s mathematics only predicts hydrogen’s spectrum (and 1 electron systems) 2.Try drawing a Bohr atom for Potassium –Yep, wrong number of electrons in outer shell. Should be 1 not 9

28. So why waste our time with this? Good question –Well there are a few reasons 1.Easy to predict outer number of electrons 2.Gave evidence for the structure of atoms

29. Homework o 155 #'s 60,62,65,66 include frequency

30. So, what’s the fix? Quantum Mechanics my friends! –Placing electrons in subshells and orbitals –Treating the electron as a standing wave.

31. Subshells The spectra (colors) emitted from excited atoms did not match what Bohr predicted. Scientists proposed the idea of subshells within the shells –Subshell – place of specific energy where electrons have a high probability of being found. –Each subshell has a specific number of orbitals

32. Subshells cont. Subshells are designated as – s, p, d, f s has 1 orbital and holds 2 electrons. p has 3 orbitals and holds 6 electrons. d has 5 orbitals and holds 10 electrons. f has 7 orbitals and holds 14 electrons. each subshell is higher in energy for a specific shell only!!!!!!

33. The s orbital has a spherical shape centered around the origin of the three axes in space. s orbital shape

34. p orbital shape

35. Shape of d orbitals

36. Shape of f orbitals

37. Relationship to an Atom Draw the Bohr atom for nitrogen. What subshells are necessary? –How many orbitals are present?

38. Electron Configurations Address for electrons Tells specific shell, subshell type, and # of electrons in that subshell Electrons always occupy the lowest energy subshell first. –Aufbau principle 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 What’s up with that 4s-3d-4p thing?

39. Lets Try a Couple Write the electron configuration for the following elements Li, Br, Fe, K Li = 1s 2 2s 1 Br = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 5 Fe = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 K = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 Anything interesting about Li and K?

40. Valence Electrons Total number of s and p electrons in last shell These are the electrons involved in reactions How many valence electrons are there –Li, Br, Fe, K –Li = 1 –Br = 7 –Fe = 2 –K = 1

41. Noble Gases How many valence electrons will noble gases have? 8 (or 2 if you are helium) 8 is a stable number of electrons –Octet rule (or duet if you are He) Use this knowledge to write electron configurations 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6

42. Noble Gas Configuration Shortened way of writing configurations Since we always know configurations of noble gases we use them as a starting point. Electron configuration of P is P = 1s 2 2s 2 2p 6 3s 2 3p 3 With noble gas configuration choose noble gas that come before which is Ne P = [Ne] 3s 2 3p 3

43. You Try It Write noble gas configuration for Li, Br, Fe, K Li = [He] 2s 1 Br = [Ar] 4s 2 3d 10 4p 5 Fe = [Ar] 4s 2 3d 6 K = [Ar] 4s 1

44. Homework Write electron configurations for elements 1,5,10,15,20, 25,30,35,40 Write noble gas configurations for elements 1,5,10,15,20, 25,30,35,40

45. 1 = 1s 1 5 = 1s 2 2s 2 2p 1 10 = 1s 2 2s 2 2p 6 15 = 1s 2 2s 2 2p 6 3s 2 3p 3 20 = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 25 = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 5 30 = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 35 = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 5 40 = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 2

46. 1 = 1s 1 5 = [He] 2s 2 2p 1 10 = [He] 2s 2 2p 6 15 = [Ne] 3s 2 3p 3 20 = [Ar] 4s 2 25 = [Ar]4s 2 3d 5 30 = [Ar] 4s 2 3d 10 35 = [Ar] 4s 2 3d 10 4p 5 40 = [Kr] 5s 2 4d 2

47. Orbital filling table

48. Electron configuration of the elements of the first three series

49. Assignment Use the periodic table to write noble gas configurations for elements 1,5,10,15,20,25,30,35,40

50. 1 = 1s 1 5 = [He] 2s 2 2p 1 10 = [He] 2s 2 2p 6 15 = [Ne] 3s 2 3p 3 20 = [Ar] 4s 2 25 = [Ar]4s 2 3d 5 30 = [Ar] 4s 2 3d 10 35 = [Ar] 4s 2 3d 10 4p 5 40 = [Kr] 5s 2 4d 2

51. Quantum Numbers Numbers that define an electrons probable position is space Very similar to electron configurations 1 extra number Spin –An electron can only spin in one direction –+1/2 or -1/2

52. Principle, angular momentum, and magnetic quantum numbers: n, l, and m l

53. Pauli Exclusion Principle No two electrons can have the same 4 quantum number This means when there are two electrons in an orbital they have to be spinning in different directions

54. Hunds Rule Every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals spin in the same direction

55. Orbital Diagrams A representation of the location and spin of electrons within an atom Process –Write the electron configuration –Place bars above configuration to represent the number of orbitals s = 1 p=3 d=5 –Place arrows on the bars to represent the spin

56. Example Draw the orbital diagram for Be Nitrogen Cobalt

57. Ionization Energy Revisited The trend for ionization energy has some exceptions Use orbital diagrams to explain the trend

59. Unpaired Electrons Electrons that are by themselves in an orbital How many unpaired electrons are there in a oxygen atom? Unpaired electrons make an atom magnetic –Paramagnetic

60. Problems P. 156 #’s 81,84 and orbital diagram

61. B = Sc = Co = Se = Ru =

63. Problems P. 157 #’s 122,124,126, 129,131,134,139 P. 114 #’s 95,96,99,100,103,110

64. Problems P. 114 #’s 95,96,99,100,103,110