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Making Light

Making Light. How do we make light?. Making Light. How do we make light? Heat and Light : Incandescent Lighting (5-10% efficient) Atoms and Light : Fluorescent Lighting & LED’s (20-40% efficient)

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Making Light

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  1. Making Light How do we make light?

  2. Making Light How do we make light? • Heat and Light: Incandescent Lighting (5-10% efficient) • Atoms and Light: Fluorescent Lighting & LED’s (20-40% efficient) We’ll review Heat and Light first. Later in this part we will consider Atoms and Light.

  3. Blackbody Radiation: Heat loss by radiation was discussed in PHYS 201 in the Thermo part. The light from a blackbody is light that comes solely from the object itselfrather than being reflected from some other source. A good way of making a blackbody is to force reflected light to make lots of reflections: inside a bottle with a small opening. [Even if light loses only 5% on each reflection, after 25 reflections the light is down to 28% of its original intensity.]

  4. Blackbody Radiation: Recall that a good absorber is also a good emitter, and a poor absorber is a poor emitter. We use the symbol  to indicate the blackness (=1) or the whiteness (=0) of an object.

  5. Blackbody Radiation: What are the parameters associated with the making of light from warm objects? • Temperature of the object, T. • Surface area of the object, A. • Color (black versus white) of the object, 

  6. Blackbody Radiation:Experimental Results At 310 Kelvin, only get IR Intensity blue yellow red IR UV wavelength

  7. Blackbody Radiation:Experimental Results At much higher temperatures, get visible - look at blue/red ratio to get temperature Intensitylog scale blue yellow red IR UV wavelength

  8. Experimental Results The preceding graph is a little misleading in that the scales for the Intensity axis are not the same for the different temperatures. For example, comparing peaks: the peak of the T=300 K curve is about 160,000 times smaller than the peak of the T=6,000 K curve. At   9.7 microns (in the IR) which is the peak of the 300 K curve, the 300 K curve is about 120 times lower than the 6,000 K curve at that same wavelength.

  9. Blackbody Radiation:Experimental Results Ptotal = AT4 where  = 5.67 x 10-8 W/m2 *K4 peak = b/T where b = 2.9 x 10-3 m*K Intensitylog scale blue yellow red IR UV wavelength

  10. Example If you eat 2,000 calories per day, that is equivalent to about 100 joules per second or about 100 Watts - which must be emitted. Let’s see how much radiation you emit when the temperature is comfortable, say 75oF=24oC=297K, and pick a surface area, say 1.5m2, that is at a temperature of 93oF=34oC=307K: Pemitted =AT4 = (5.67x10-8W/m2K4)*(.97)*(1.5m2)*(307K)4 = 733 Watts emitted!

  11. Example continued But this is not the whole story: besides emitting radiation, we receive radiation from the outside: Pabsorbed =AT4 = (5.67x10-8W/m2K4)*(.97)*(1.5m2)*(297K)4 = 642 Watts absorbed! Hence, the net power emitted by the body via radiation is: Pnet =733 Watts -642 Watts = 91 Watts.The peak of this radiation is at: peak = b/T = 2.9x10-3m*K / 307K = 9.5m which is in the infrared (as expected).

  12. Blackbody Radiation:Wave Theory Certain waves resonate in an object (due to standing wave), such that n(/2) = L. From this it follows that there are more small wavelengths that fit than long wavelengths. (see next slide for example)

  13. Blackbody Radiation:Wave Theory n(/2) = L Example: for L = 1 meter, we have the following wavelengths that “fit”: 1 = 2 m; 2 = 1 m; 3 = .67 m; 4 = .50 m; 5 = .40 m; 6 = .33 m; 7 = .29 m; 8 = .25 m; etc. For the range of ’s, we have permitted 1 - 1.99 m; 1 .50 - .99 m (half the range size), 2 .25 - .49 m (half again the range size), 4 etc.

  14. Blackbody Radiation:Wave Theory From thermodynamics, we have the equipartition of energy: Each mode on average has an energy proportional to the Temperature of the object: Emode = kT, where k = 1.38 x 10-23 Joules/Kelvin.

  15. Blackbody Radiation:Wave Theory The standing wave theory and the equipartition of energy theory together predict that the intensity of light should increase with decreasing wavelength: This works very well at long wavelengths, but fails at short wavelengths. This failure at short wavelengths is called the ultraviolet catastrophe.

  16. Blackbody Radiation:Wave Theory wave theory: UV catastrophe Intensitylog scale experiment wavelength

  17. Blackbody Radiation:Planck’s idea • Need to turn the Intensity curve down when  gets small (or frequency gets large). • Keep standing wave idea and number of modes. • Look at equipartition theory and how the energy per mode got to be kT (where k is Boltzmann’s constant: k = 1.38 x 10-23 J/K).

  18. Blackbody Radiation:Planck’s idea Eavg = Ei /1 = P(E)*E / P(E) where P(E) is the probability of having energy, E. From probability theory we have the Boltzmann probability distribution function: P(E) = Ae-E/kT (this is demonstrated in the next few slides). If we assume that energy is continuous, then the summation can become an integral, and we can get a value for the average energy (which we do after discussing the Boltzmann probability distribution).

  19. BOLTZMANN DISTRIBUTION Probability of one atom having n units of energy P(En) = P(n*E1) is based on equal likelihood of any atom having any of the n units. Following is a listing of all possible cases for 4 atoms (called A, B, C and D) having three units of energy. After that we will state the results of 4 atoms having five units of energy.

  20. BOLTZMANN DISTRIBUTION CASE I: four atoms having three units of energy: ABCD ABCD ABCD ABCD ABCD ABCD 3000 2100 1200 1020 1002 1110 0300 2010 0210 0120 0102 1101 0030 2001 0201 0021 0012 1011 0003 0111 (3000) 4 (2100) 12 (1110) 4

  21. BOLTZMANN DISTRIBUTION Case I: Probability of atom A having n units: P(n): P(3) = 1/20 = .05 P(2) = 3/20 = .15 P(1) = 6/20 = .30 P(0) =10/20 = .50 Note that the sum of probabilities equals 1 as it should: P(n) = 20/20 = 1.00

  22. BOLTZMANN DISTRIBUTION Note that this distribution is different than the distribution based on straight probability. For example, it may seem that the probability of an atom getting a unit of energy would be ¼ for each of the three units available, so the probability that one atom would get a unit of energy in all three distributions would be (1/4)3 = .0156 (compared to the Boltzmann probability of .050). But we can’t have all four atoms having 3 units of energy since that would mean we would need 12 units of energy when we only have 3 units total!

  23. BOLTZMANN DISTRIBUTION Likewise, the straight probability of one atom getting no units of energy in each distribution would be (3/4), so the straight probability of one atom getting zero after three distributions would be (3/4)3 = .422 (compared to the Boltzmann’s probability of .500), but we can’t have all four atoms having zero units since we do have 3 units of energy that must be distributed.

  24. BOLTZMANN DISTRIBUTION CASE II: Case I: four atoms having five units of energy: Prob of atom A having: P(5) = 1/56 = .018 P(5) = .000 P(4) = 3/56 = .054 P(4) = .000 P(3) = 6/56 = .107 P(3) = .050 P(2) =10/56 = .179 P(2) = .150 P(1) =15/56 = .268 P(1) = .300 P(0) =21/56 = .375 P(0) = .500

  25. Plot of P(E) vs E 4 units 5 units

  26. P(E) vs E • Note that both of these look approximately like dying exponentials. • Note that P(E) for large values of E gets bigger and P(E) for small values of E gets smaller if there is more energy to share. • Note that since the sum of P(E) over all E gives 1, the value of P(0) decreases as E gets bigger. The function P(E) = Ae-E/kT is consistent with all of these. What is important in calculating the average energy is the product of E and P(E). We look at this on the next slide.

  27. Plot of E*P(E) vs E P(E) E*P(E)

  28. Blackbody Radiation:Sum goes to Integral Eavg =LIME→0 [P(E) / P(E)] = = = Area under the curve / 1 = kT .

  29. Blackbody Radiation:Planck’s idea Planck recalled that the SUM only became the INTEGRAL if you let E go to zero. Planck’s idea was NOT to let E go to zero. If you require P(E) to be evaluated at the end of each E, then the SUM will decrease as E increases!

  30. Blackbody Radiation:Planck’s idea As E gets bigger, Eavg gets smaller: E*P(E) = A*E*e-E/kT . Area under red curveis more thanarea under blue is more thanarea under green. E*P(E) E

  31. Blackbody Radiation:Planck’s idea It’s easy to see on the leading edge that as E gets bigger, the total Energy under the curve and hence the average energy gets smaller. This is in fact confirmed by an actual summation. Eavg ↓ as E ↑

  32. Blackbody Radiation:Planck’s idea To get the curve to fall at small wavelengths Planck tried the simplest relation: E α 1/l , or E = (constant) * f since we need to decrease the average energy per mode more as the wavelengths get smaller - and the frequency gets bigger: Eavg ↓ as E ↑ as l ↓ as f ↑ .

  33. Blackbody Radiation:Planck’s idea Planck found that he could match the curve and DERIVE the empirical relations: • P = AT4where = 5.67 x 10-8 m2 *K4 • max = b/T whereb = 2.9 x 10-3 m*K with the simplest relation: E = (constant) * f if the constant = 6.63 x 10-34 J*sec = h. The constant, h, is called Planck’s constant.

  34. How to Make Light The wave theory combined with the equipartition of energy theory failed to explain blackbody radiation. Planck kept the wave idea of standing waves but introduced E = hf, the idea of light coming in discrete packets (or photons) rather than continuously as the wave theory predicted.

  35. How to Make Light From this theory we now have a way of relating the photon idea to the wave idea for color and type: E = hf . • Note that high frequency (small wavelength) light has high photon energy, and that low frequency (large wavelength) light has low photon energy.

  36. How to Make Light E = hf High frequency light tends to be more dangerous than low frequency light(UV versus IR, x-ray versus radio).The photon theory gives a good account of why the frequency of the light makes a difference in the danger. Individual photons cannot break bonds if their energy is too low while big photons can!

  37. Photons and Colors • Electron volts are useful size units of energy 1 eV = 1.6 x 10-19 Coul * 1V = 1.6 x 10-19 J. • radio photon: hf = 6.63 x 10-34 J*s * 1 x 106 /s = 6.63 x 10-28 J = 4 x 10-9 eV • red photon: f = c/3 x 108 m/s / 7 x 10-7 m = 4.3 x 1014 Hz, red photon energy = 1.78 eV • blue: = 400 nm; photon energy = 3.11 eV .

  38. Power and photonsExample How many photons are emitted every second from one watt of yellow light? Power = Energy / time = Energy per photon * number of photons / time = hf * n/sec; f=c, so f = c/ Power = (hc/) * n/sec P = 1 Watt = (6.63 x 10-34 J-s * 3 x 108 m/s / 5.5 x 10-7m) * n/sec; n/sec = 2.8 x 1018 photons per second.

  39. Making and Absorbing Light • The photon theory with E = hf was useful in explaining the blackbody radiation. • Is it useful in explaining other experiments? • We’ll consider next the photoelectric effect.

  40. Photoelectric Effect Light hits a metal plate, and electrons are ejected. These electrons are collected in the circuit and form a current. light ejected electron A + - V

  41. Photoelectric Effect The following graphs illustrate what the wave theory predicts will happen: current light intensity current Voltage current frequency of light

  42. Photoelectric Effect We now show in blue what actually happens: current lightintensity V-stop current Voltage current f-co frequency of light

  43. Photoelectric Effect In addition, we see a connect between V-stop and f above fcutoff: V-stop frequency fcutoff

  44. Photoelectric Effect Einstein received the Nobel Prize for his explanation of this. (He did NOT receive the prize for his theory of relativity.)

  45. Photoelectric Effect Einstein suggested that light consisted of discrete units of energy, E = hf. Electrons could either get hit with and absorb a whole photon, or they could not. There was no in-between (getting part of a photon). If the energy of the unit of light (photon) was not large enough to let the electron escape from the metal, no electrons would be ejected. (Hence, the existence of f-cutoff.)

  46. Photoelectric Effect If the photon energy were large enough to eject the electron from the metal (here, W is the energy necessary to eject the electron), then the following equation would apply: hf = W + KE The Energy of the photon absorbed (hf) goes into ejecting the electron (W) plus any extra energy left over which would show up as kinetic energy (KE).

  47. Photoelectric Effect This extra kinetic energy (KE) would allow the electron to climb up a “hill”, but the size of the hill that the electron could climb up would be limited to the extra kinetic energy the electron had. By measuring the highest hill, we could arrive at the extra energy of the electron. Hill sizes in electrical terms are in VOLTS: KE = PE = qVstop.

  48. Photoelectric Effect Put into a nice equation: • hf = W + e*Vstop • where f is the frequency of the light • W is the “WORK FUNCTION”, or the amount of energy needed to get the electron out of the metal • Vstopis the stopping potential • When Vstop = 0, f = fcutoff , and hfcutoff = W.

  49. Photoelectric Effect - Example Most metals have a work function on the order of several electron volts. Copper has a work function of 4.5 eV. Therefore, the cut-off frequency for light ejecting electrons from copper is: hfcutoff = 4.5 eV, or fcutoff = 4.5 x (1.6 x 10-19 C) x (1 V) / 6.63 x 10-34 J-sec = 1.09 x 1015 Hz,

  50. Photoelectric Effect - Example or cutoff = c/ fcutoff , or cutoff = (3 x 108 m/s) / (1.09 x 1015 cycles/sec) = 276 nm (in the UV range) Any frequency lower than the cut-off (or any wavelength greater than the cut-off value) will NOT eject electrons from the metal.

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