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O.A # 28

O.A # 28. Wavelength. O.A # 29. Calculate frequency if the wavelength is 200 nm (1nm= 10 -9 m) and c=3.00x 10 8 m/s. n= c / l. = 200 nm x 10 -9 m 1 nm. = 200x 10 -9 m =2x 10 -7 m. n = 3.00x 10 8 m/s 2x 10 -7 m. = 1.5 x 10 15. Hz, 1/sec, s -1.

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O.A # 28

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  1. O.A # 28 Wavelength

  2. O.A # 29 Calculate frequency if the wavelength is 200 nm (1nm=10-9 m) and c=3.00x108 m/s n= c / l • = 200 nm x 10-9 m 1 nm = 200x10-9 m =2x10-7 m n = 3.00x108 m/s 2x10-7 m = 1.5 x1015 Hz, 1/sec, s-1

  3. O.A # 30 Atomic Emission Spectrum

  4. O.A # 31 Electron Configuration

  5. 7s 7p 7d 7f 6s 6p 6d 6f 5s 5p 5d 5f 4s 4p 4d 4f 3s 3p 3d 2s 2p 1s O.A. # 32 Write the electron configuration for the following atoms a) Ti: 22 e- 1s22s22p63s23p64s23d2 b) Sr: 38 e- 1s22s22p63s23p64s2 3d104p65s2

  6. O.A # 33 Page 149 # 1-10 (skip #8) • D • A • C • D • A • B • A • C • B • D

  7. O.A # 34 What is the energy of violet light if the wavelength is 2.95x10-8 m? c = ln c=3.00x108 m/s E = hn h = 6.626 x 10 -34 J.s n = c/l n = 3.00 x 108 m/s 2.95x10-8m • n = 1.02 x 1016 1/s E = (6.6262 x 10 -34 J/s)(1.02 x 1016 1/s) E = 6.76 x 10 -18 J

  8. O.A # 33 Frequency

  9. O.A # Electromagnetic Radiation

  10. Chapter 5 – pg 116 Electrons in Atoms • What you’ll learn • Why It’s important?

  11. Light • Has properties of both particles and waves • Light is a kind of electromagnetic radiation. • All move at the same speed, called speed of light. C= 3.00 x 108 m/s

  12. Crest Wavelength l Amplitude Trough Parts of a wave Origin

  13. Frequency (n) • The number of waves that pass a given point per second. • How fast oscillates up and down • Units are: cycles/sec ,hertz(hz), 1/second ------------------------1 sec---------------------------- 2 hz or 1/sec • =

  14. Frequency and Wavelength • Are inversely related • As one goes up the other goes down. • Different frequencies of light is different colors of light. • The whole range is called a spectrum • speed of light = wavelength x frequency • c = l n

  15. Calculating speed of light l =? 1.What is the wavelength of blue light with a frequency of 8.3 x 1015 hz(1/sec)? =n speed of light = wavelength x frequency c = l.n 8 C = 3.00 x 10 m/s -8 L = c / n = 3.6 x 10 m

  16. n=? 2. What is the frequency of red light with a wavelength of 4.2 x 10 m ? -5 =l n= c / l c = l . n 12 n = 7.1 x 10 hz(1/sec) Page 147 # 65-68

  17. Objective • Explain the difference between continuous spectrum of white light and the atomic emission of an element.

  18. High energy Low energy Low Frequency High Frequency Classification of Electromagnetic Radiation X-Rays Radiowaves Microwaves Ultra-violet GammaRays Infrared . Long Wavelength Short Wavelength Visible Light R O Y G B I V

  19. Continuous Spectrum • White light is made up of all the colors of the visible spectrum. • Passing it through a prism separates it.

  20. If the light is not white • By heating a gas with electricity we can get it to give off colors.

  21. Atomic Spectrum How color tells us about atoms • Each element gives off its own characteristic colors. • Can be used to identify the atom. • How we know what stars are made of.

  22. These are called discontinuous spectrum • Or line spectrum • (finger print of elements) • unique to each element. • These are emission spectra

  23. Bohr’s Model of the Atom Nucleus Electron Orbit Energy Levels

  24. Bohr’s Model of the Atom • Why don’t the electrons fall into the nucleus? • Move like planets around the sun. • In circular orbits at different levels(7) • Amounts of energy separate one level from another.

  25. An explanation of hydrogen’s line spectrum

  26. Calculating Energy of a Photon • Light is energy • Energy is quantized • Light must be quantized • The smallest pieces of light are called photons. • Energy and frequency are directly related.

  27. Equation for Energy • E = h . n • E is the energy of the photon • n is the frequency • h is Planck’s constant • h = 6.626 x 10 -34 Joules . sec • joule is the metric unit of Energy

  28. Page 147 # 70-76

  29. Objective • Apply the Pauli exclusion principle, and Aufbau principle to write electron configurations

  30. Has energy levels for electrons. There are 7 energy levels. It can only tell us the probability of finding an electron at certain distance from the nucleus. The Quantum Mechanical Model of the Atom

  31. Quantum #’s • Principle Quantum Number (n) -- the energy level of the electron. • 2(n)2 = # of electrons per energy level (32 e- max.) • Sublevels (l)-- describes sublevels within an energy level. • s,p,d,f (names of sublevels)

  32. Orbitals (m)--Regions where there is a high probability of finding an electron. • Each orbital can hold 2 e-. • Spin (s)-- in each orbital there can be up to 2 electrons spinning in opposite directions.

  33. 1 s orbital for every energy level S orbitals 3s 2s 1s

  34. Start at the second energy level 3 different directions 3 different shapes P orbitals

  35. P Orbitals

  36. Start at the third energy level 5 different shapes D orbitals

  37. F orbitals • Start at the fourth energy level • Have seven different shapes

  38. Summary # of orbitals Max # e- Starts at energy level s 1 1 2 e- 3 6 e- p 2 5 10 e- 3 d 4 14 e- f 7

  39. Electron Configurations • Electron Configurations represents the way electrons are arranged in atoms. • Aufbau principle- electrons enter the lowest energy level first. Pauli Exclusion Principle: No two e- in an atom have the same set of quantum numbers

  40. 7s 7p 7d 7f 6s 6p 6d 6f 5s 5p 5d 5f 4s 4p 4d 4f 3s 3p 3d 2s 2p 1s Diagonal Rule

  41. 7s 7p 7d 7f 6s 6p 6d 6f 5s 5p 5d 5f 4s 4p 4d 4f 3s 3p 3d 2s 2p 1s Fill from the bottom up following the arrows

  42. 7s 7p 7d 7f 6s 6p 6d 6f 5s 5p 5d 5f 4s 4p 4d 4f 3s 3p 3d 2s 2p 1s Fill from the bottom up following the arrows

  43. 7s 7p 7d 7f 6s 6p 6d 6f 5s 5p 5d 5f 4s 4p 4d 4f 3s 3p 3d 2s 2p 1s Fill from the bottom up following the arrows

  44. 7s 7p 7d 7f 6s 6p 6d 6f 5s 5p 5d 5f 4s 4p 4d 4f 3s 3p 3d 2s 2p 1s Fill from the bottom up following the arrows

  45. 7s 7p 7d 7f 6s 6p 6d 6f 5s 5p 5d 5f 4s 4p 4d 4f 3s 3p 3d 2s 2p 1s Fill from the bottom up following the arrows

  46. 7s 7p 7d 7f 6s 6p 6d 6f 5s 5p 5d 5f 4s 4p 4d 4f 3s 3p 3d 2s 2p 1s Fill from the bottom up following the arrows

  47. 7s 7p 7d 7f 6s 6p 6d 6f 5s 5p 5d 5f 4s 4p 4d 4f 3s 3p 3d 2s 2p 1s Diagonal Rule

  48. Practice H 1s1 He 1s22s22p3 N Ca+2 1s22s22p6 3s23p6 F-1

  49. The Shorthand e- configuration • Write the symbol of the noble gas before the element. • Then the rest of the electrons.

  50. Noble gas e- configuration

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