1. OUTLINE OF TOPICS 1. A Light Wave – What is light? 2. History of the Periodic Table 3. Electron Configuration 4. Quantum Number – Atom’s Address 5. Quantum Power – What is energy? 6. Atom is Bohr-ed – The story of Atom Part II

2. 1. A Light Wave What is light? What is color? What does the word “frequency” mean?

3. 1. A Light Wave OBJECTIVE: To understand what light and colors are

4. 1. A Light Wave Light is a WAVE This wave has electrical properties AND This wave has magnetic properties So we call light an electro-magnetic wave

5. 1. A Light Wave Spectrum = a range This picture is a range of waves from long to short

6. 1. A Light Wave

7. 1. A light wave WavelengthFrequency What is it Symbol: Unit: 2 quantitative properties of a wave

8. 1. A Light Wave Wavelength: distance between two waves “crest to crest” or “trough to trough”

9. 1. A Light Wave What does it mean to do something frequently?

10. 1. Quantum Model Frequency: how many waves in 1 second

11. 1. Quantum Model 2 properties of waves Wavelength: distance between two waves either crests or troughs Symbol: l Units = meters, m

12. 1. Quantum Model 2 properties of waves Frequency: How many waves in 1 second Symbol: v Units = Hz, or sec -1

13. 1. Quantum Model

14. Which has a longer wavelength: radio or ultraviolet?

15. 1. Quantum Model Which has a higher frequency: radio or ultraviolet?

16. 1. A Light Wave Heat energy in the form of Infrared waves

17. 1. A Light Wave X-RaySunburn from UV rays

18. 1. Quantum Model 2 properties of waves Wavelength: is… Symbol: ? Units = ? Frequency: is… Symbol: ? Units = ? What does it mean for wavelength and frequency to have an inverse relationship?

19. 1. Quantum Model 2 properties of waves l = Wavelength v = Frequency C = Speed of light = 3.0 x 10 8 meters/seconds <- this number never changes l v = c l

20. 1. Quantum Model Calculations using l v = c Your favorite radio station broadcasts the signal at 99.5 MHz. This is equal to 9.96 x 10 7 Hz. Calculate the wavelength in meters. 1. Write the equation: l v = c 2. Plug in values. C = 3.0 x 10 8 m/s ALWAYS 3. Rearrange equation to solve for unknown. 4. Solve Answer = 3.01 meters

21. 1. Quantum Model Calculations using l v = c Photosynthesis uses light waves with a wavelength of 660 nm to convert CO 2 and H 2 O into glucose and O 2. 660 nm = 6.6 x 10 - 7 m. Calculate the frequency. 1. Write the equation: l v = c 2. Plug in values. C = 3.0 x 10 8 m/s ALWAYS 3. Rearrange equation to solve for unknown. 4. Solve Answer = 4.5 x 10 14 Hz or 4.5 x 10 14 sec -1

22. 1. A Light Wave Answer on Warmup Paper. Label it as “WAVES” Your favorite FM radio station broadcasts at a frequency of 101.1 MHz. This is equal to 1.011 x 10 8 Hz. What is the wavelength of this station in meters? A police officer is using a radar gun for speeding citations. The gun uses waves with a wavelength of 8.45 nanometers. This is equal to 8.45 x 10 -9 meters. What is the frequency in Hz?

23. 1.Make sure that l is in METERS, or that v is in Hz 2.If not, then convert to METERS or Hz using the conversion factors given to you. 3.Solve: Step-by-step instructions on how to solve should be in your notes 4.Does your final answer have the units that is asked for in the problem?

24. 1. A Light Wave 1. What is light? 2. What are the symbols and units for the two quantitative properties of a wave? 3. What is the relationship between the two quantitative properties? 4. Explain why we have different colors using the two quantitative properties 5. What does a high frequency mean in terms of energy? Summary & Review

25. 2. Quantum Power What is energy? What are some examples of energy? What is energy made out of? What do you think the word “quantum” means? How is walking up stairs different from walking up a hill?

26. 2. Quantum Power OBJECTIVE: To understand what energy is

27. 2. Quantum Power Energy as massless waves

28. 2. Quantum Power Relationship between ENERGY and WAVELENGTH

29. 1. Quantum Model

30. 2. Quantum Power What does it mean for energy to be quantized? What does it mean for light to be quantized? What is a quantum?What is a photon?

31. 2. Quantum Power Max Plank Discovered that Energy is QUANTIZED Quantized? Means WHOLE NUMBERS Energy is quantized = energy is gained or lost in WHOLE NUMBERS

32. 2. Quantum Power Max Plank Energy is quantized = energy is gained or lost in WHOLE NUMBERS Similar Examples: 1. Musical instruments are “quantized” in that they can only produce certain notes, like C or F #. 2. US Dollars is “quantized” in whole number of pennies.

33. 2. Quantum Power

34. What does it mean for energy to be quantized? Whole numbers of what? Whole numbers of quantum What is a quantum? The smallest UNIT of energy. A penny is similar to a quantum because…

35. 2. Quantum Power Einstein and the Photoelectric Effect Photoelectric Effect: when metals lose electrons when it is hit with light

36. 2. Quantum Power Einstein and the Photoelectric Effect Why does nothing happen when red light makes contact with the metal? Why does only violet light release an electron?

37. 2. Quantum Power Einstein and the Photoelectric Effect It was thought that color should not matter, only intensity But experiment showed that color does matter.

38. 2. Quantum Power Einstein and the Photoelectric Effect Einstein applied Plank’s idea, and said Light is also quantized Light is made up of particles called PHOTONS PHOTON: a particle of light

39. 2. Quantum Power What does it mean for energy to be quantized? What does it mean for light to be quantized? What is a quantum?What is a photon?

40. 2. Quantum Power Why Plank and Einstein are important Plank’s and Einstein's postulate that energy is quantized is in many ways similar to Dalton’s description of atoms. Both theories are based on the existence of simple building blocks, atoms in one case, and quanta in the other. The work of Plank and Einstein thus suggested a connection between the quantized nature of energy and the properties of individual atoms. In fact, Einstein's Nobel Prize was awarded for his work in the photoelectric effect and demonstrating its fundamental important, not for his famous E=mc 2 equation.

41. 2. Quantum Power Why Plank and Einstein are important Plank’s and Einstein's postulate that energy is quantized is in many ways similar to Dalton’s description of atoms. Both theories are based on the existence of simple building blocks, atoms in one case, and quanta in the other. The work of Plank and Einstein thus suggested a connection between the quantized nature of energy and the properties of individual atoms. In fact, Einstein's Nobel Prize was awarded for his work in the photoelectric effect and demonstrating its fundamental important, not for his famous E=mc 2 equation.

42. 2. Quantum Power Why Plank and Einstein are important 1. Light is as BOTH waves and particles. simulation

43. 2. Quantum Power What does it mean for energy to be quantized? What does it mean for light to be quantized? What is a quantum?What is a photon? How is a penny or steps on a stair like a quantum of energy/a photon of light?

44. 2. Quantum Power Summary & Review What is a quantum? A package of energy, the smallest unit of energy How is a photon like a quantum? A photon is like a quantum because a photon is the basic unit of light Explain what it means for energy to be quantized by using one of the examples used in class: stairs, hills, penny, music notes

45. 1. Quantum Model What does it mean for energy to be quantized? It means that energy is transferred in whole numbers. Example: Stairs vs a hill, music, US Dollars What does it mean for light to be quantized? It means that light is also transferred in whole numbers because light is made up of particles What is a quantum? Smallest unit of energy What is a photon? A particle of light How is a penny like a quantum of energy? Just like the penny is the smallest unit, a quantum is the smallest unit of energy.

46. 1. Quantum Model Max Plank E = hv h = Plank’s Constant h = 6.626 x 10 -34 Jsec (J = Joule, the unit for measuring energy)

47. 1. Quantum Model Plank + Einstein = Calculating the Energy of one Photon E = (hc)/ l h = Plank’s Constant h = 6.626 x 10 -34 Jsec This number NEVER changes (J = Joule, the unit for measuring energy)

48. 1. Quantum Model Plank + Einstein = Calculating the Energy of a Photon E = (hc)/ l The blue color in fireworks results when copper is heated to about 1200°C. The blue light has a wavelength of 450 nm. What is the unit of energy emitted? 1. Write equation 2. Plug in values. h = 6.626 x 10 -34 Jsec ALWAYS 3. Solve ANSWER = 4.42 x 10 -19 J

49. 1. Quantum Model Plank + Einstein = Calculating the Energy of a Photon E = (hc)/ l A ruby laser emits a red light at a wavelength of 694.3 nm. What is the energy in J? 1. Write equation 2. Make sure l is in METERS. Plug in values. h = 6.626 x 10 -34 Jsec ALWAYS 3. Plug in values. h = 6.626 x 10 -34 Jsec ALWAYS 4. Solve ANSWER = 2.861 x 10 -19 J

50. 1. Quantum Model Plank + Einstein = Calculating the Energy of a Photon E = (hc)/ l An x-ray generator, such as those used in hospitals, emits radiation with a wavelength of 1.544 angstrom. What is the energy of a single proton? 1. Write equation 2. Make sure l is in METERS. Plug in values. h = 6.626 x 10 -34 Jsec ALWAYS 3. Plug in values. h = 6.626 x 10 -34 Jsec ALWAYS 4. Solve ANSWER = 1.287 x 10- 15 J

51. 1. Quantum Model Plank + Einstein = Calculating the Energy of a Photon E = (hc)/ l 1. Write equation 2. Make sure l is in METERS. If not, then convert it to METERS using sideways T 3. Plug in values h = 6.626 x 10 -34 Jsec ALWAYS Plug in values. c = 3.0 x 10 8 m/sec ALWAYS 4.Solve

52. 3. History, Period. What is atomic number? Where is the atomic number found on the Periodic Table? What is atomic mass? Where is the atomic mass found on the Periodic Table?

53. 3. History, Period. OBJECTIVE: History of the Periodic Table

54. 3. History, Period. Brief History of the Table Just like class activity many different versions 1860 - John Newlands & Octaves 1869 – Dimitri Mendeleev Compare Mendeleev’s table with the modern one. List two similarities and two differences

55. 3. History, Period. 1869 – Dimitri Mendeleev

56. 3. History, Period. 1869 – Dimitri Mendeleev put elements into ROWS by ATOMIC MASS. made columns by PROPERTY Left blank spaces Blanks = elements not yet discovered Predicted properties of undiscovered elements AND PREDICTIONS WERE CORRECT!

57. 3. History, Period. Brief History of the Table Just like class activity, different versions 1860 - John Newlands & Octaves 1869 – Dimitri Mendeleev So how did we get from Mendeleev’s table to today’s table?

58. 3. History, Period.

59. Modern (YOUR) Periodic Table Arranged by ROWS By ATOMIC NUMBER

60. 3. History, Period. Modern (YOUR) Periodic Table Arranged by COLUMNS By SIMILAR PROPERTIES

61. 3. History, Period. Brief History of the Table Just like class activity, different versions 1860 - John Newlands & Octaves 1869 – Dimitri Mendeleev 1913 – J. Moseley & Protons & Atomic # Nickel vs Cobalt Classwork: Textbook pg 122, #2,5,6,7,8

62. 3. History, Period. Summary & Review 1.In what two ways is today’s periodic table organized? 2.List 2 ways Mendeleev and your table are different. List 2 ways how they are similar 3.Why is Nickel and Cobalt placed in a different order in your PT than it was in Mendeleev’s? 4.In 2013, a new element was created, element 115. Use your periodic table to predict 1.Its possible mass 2.Its period and group 3.Elements with similar property

63. 4. Atom is Bohr-ed Draw our solar system on your warmup paper Draw a hydrogen atom It was one proton and one electron Draw a helium atom It has two protons, two neutrons and two electrons Draw a lithium atom It has three protons, three neutrons, three electrons

64. 4. Atom is Bohr-ed OBJECTIVE: Another model of the Atom

65. 4. Atom is Bohr-ed Bohr said that electrons ORBIT the nucleus Okay…how is this different from Rutherford’s model?

66. 4. Atom is Bohr-ed Bohr’s Model Bohr said that electrons ORBIT the nucleus, ORBITS are QUANTIZED What does this mean???

67. 4. Atom is Bohr-ed You MUST be ON a step You CANNOT be BETWEEN steps

68. 4. Atom is Bohr-ed Orbits are “quantized” means… electrons MUST be ON an orbit Electrons CANNOT be BETWEEN orbits You MUST be ON a step You CANNOT be BETWEEN steps

69. 4. Atom is Bohr-ed Orbits are “quantized” means… The orbits are like steps! Notice the “steps”/orbits are not all the same distance?

70. 4. Atom is Bohr-ed Orbits are “quantized” means… electrons MUST be ON an orbit Electrons CANNOT be BETWEEN orbits You MUST be ON a step You CANNOT be BETWEEN steps

71. 4. Atom is Bohr-ed Why did Bohr say atoms have quantized orbits? Evidence? LINE SPECTRUMS was Neil Bohr’s evidence that atoms have quantized orbits

72. 4. Atom is Bohr-ed What is a line spectrum? Red Orange Yellow Green Blue + Purple/Violet White Light

73. 4. Atom is Bohr-ed What is a line spectra?

74. 4. Atom is Bohr-ed Energy, Photons and Line Spectrum What is a line spectra?

79. 4. Atom is Bohr-ed Why do we get line spectrums?

80. 4. Atom is Bohr-ed

81. Bohr’s Model

82. 4. Atom is Bohr-ed Bohr’s Model

83. 4. Atom is Bohr-ed Orbits represent ENERGY LEVELS Closer to nucleus = lower energy level Farther from nucleus = higher EL Period = Energy Level Period 1 = Lowest Period 7 = Highest

84. 4. Atom is Bohr-ed Orbits represent ENERGY LEVELS Closer to nucleus = lower energy level Farther from nucleus = higher EL Period = Energy Level Period 1 = Lowest Period 7 = Highest

85. 4. Atom is Bohr-ed IMPORTANT Bohr’s idea of orbit is correct …kind of After more discovery, we call it an orbital, and yes, there is a BIG difference BUT, for us, we will treat it similarly

86. 4. Atom is Bohr-ed There are 4 types of orbits/orbitals S orbital P orbital

87. 4. Atom is Bohr-ed There are 4 types of orbits/orbitals D orbital

88. 4. Atom is Bohr-ed There are 4 types of orbits/orbitals F orbital

89. 4. Atom is Bohr-ed There are 4 types of orbits/orbitals We are only going to use the s p d orbitals

90. 4. Atom is Bohr-ed

91. W hat is the difference between 1s orbital and 2s orbital?? size (draw)

92. 4. Atom is Bohr-ed 1. What do the orbits/orbitals represent? 2. What does it mean for orbits to be quantized? 3. What are the three orbitals we will use? 4. What is the different between a 1s orbital and a 2s orbital? 5. What is the difference between a 2p and a 3p orbital? 6. What do the number and the letter represent in “1s” and “2p”?

93. 5. Electron Configuration So what do we do with the orbitals and the energy levels?

94. 5. Electron Configuration OBJECTIVE: Learn how electrons are organized inside an atom

95. 5. Electron Configuration Each orbital can have 2 electrons MAX 1s orbital and 2s orbital

96. 5. Electron Configuration Each orbital can have 2 electrons S orbital 2 electrons

97. 5. Electron Configuration p orbital 2 2 2 6 electrons

98. 5. Electron Configuration d orbital 2 + 2 + 2 + 2 + 2 = 10 electrons

99. 5. Electron Configuration f orbital

100. 5. Electron Configuration How to write Electron Configurations 1. Find element on PT 2. Write symbol of element 3. Write number of electrons 4. Start counting from Hydrogen. 5. you MUST start at Hydrogen, ALWAYS 6. Count from left to right, in this direction  7. Use H.O. to help remember the different blocks. 8. Check your work

101. 5. Electron Configuration Write electron configurations for the following elements HHeBeCONe MgAlSiScVCo

102. 5. Electron Configuration What are valence electrons? electrons in its outermost orbital are called the valence electrons

103. 5. Electron Configuration How do we know which are the valence electrons? electrons in the HIGHEST ENERGY LEVEL are valence electrons

104. 5. Electron Configuration Write electron configuration for Silicon, Si Si = 1s 2 2s 2 2p 6 3s 2 3p 2

105. 5. Electron Configuration Write electron configuration for Gallium, Ga Ga = 1s 2 2s 2 2p 6 3s 2 3p 2 4s 2 3d 10 4p 1 Ge has 3 valence electrons

106. 5. Electron Configuration 1.Write electron configurations 2.Underline valence electrons Do you notice a pattern? LithiumMgBoronSulfurFluorineNeon SodiumCaAluminumSelleniumChlorineKrypton

107. 5. Electron Configuration 1.Write electron configurations for the following 2.Underline the valence electrons Barium [Xe]6s 2 Carbon [He]2s 2 2p 2 Nitrogen [He]2s 2 2p 3 Oxygen [He]2s 2 2p 4 Fluorine [He]2s 2 2p 5 Neon [He]2s 2 2p 6 AluminumTinPhosphorusTelluriumChlorineKrypton

108. 5. Electron Configuration How many valence electrons do you predict the last row will have? Do you notice a pattern? BariumCarbonNitrogenOxygenFluorineNeon AluminumTinPhosphorusTelluriumChlorineKrypton IndiumSiliconArsenicSeleniumBromineArgon

109. 2. Electron Configuration EXAMPLE: Sodium 1s 2 2s 2 2p 6 3s 1 = [Ne]3s 1 Lithium 1s 2 2s 1 = [He]2s 1 This pattern is seen in columns 1-2 and 13-18 of the PT What other patterns might exist within the PT? Maybe there is a reason why the PT has that weird shape!

110. 5. Electron Configuration Summary & Review 1. How many electrons can the s, p, and d orbitals hold? 2. What are valence electrons 3. How do you know which electrons are the valence electrons? 4. Write the EC for Calcium and Titanium 5. How many valence electrons do calcium and titanium have? What is their energy levels?

111. Periodic Table Important GROUPS 1. Alkali Metals 2. Alkali Earth Metals 3. Halogens 4. Noble Gases 5. Transition Metals 6. Lanthanides 7. Actinides 8. Metalloids

112. Periodic Table 1. Alkali Metals metals very reactive 2. Alkali Earth Metals metal does NOT dissolve quickly in water high melting point

113. Periodic Table 3. Halogens non-metal very reactive 4. Noble Gases gases stable not reactive – why?

114. Periodic Table 5. Metals conducts heat and electricity malleable – like Playdoh ductile

115. Periodic Table 6. Lanthanides extremely rare 7. Actinides also rare radioactive

116. Periodic Table 8. Metalloids solid, but not metal has properties of metals