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Unformatted text preview: Light/Quantum Theory/Electronic Structure 1. Calculate the frequency of bluegreen light having a wavelength of 520 nm. c c 3.00 x 10 m / s 520 x 10 m 5.77 x 10 s 8 9 14 1 = = = = 2. What is the wavelength of yellow light having a frequency of 5.2 x 10 14 s1 ? nm 10 x 5.8 m 10 x 5.8 s 10 x 5.2 m/s 10 x 3.00 c 2 7 1 14 8 = = = = 3. The frequency of most commercially available microwave ovens is 2.45 x 10 9 Hz. Calculate the wavelength in nm of the microwave. = = = c 3.00 x 10 m / s 2.45 x 10 s 0.122 m = 1.22 x 10 nm 8 91 8 4. What is the energy of a photon of violet light with = 412 nm? What is the energy of one mole of photons with this wavelength? E hc (6.626 x 10 J s)(3.00 x 10 m / s) 412 x 10 m 4.82 x 10 J / photon 34 8 9 19 = = = 4.82 x 10 J 1 photon 6.022 x 10 photons 1 mol 291 kJ mol 19 23 = 5. Calculate the frequency and wavelength of the photon emitted when an electron undergoes a transition from the n=4 to the n=2 level in a hydrogen atom. J x10 4.08 4 1 2 1 J 10 x 2.178 n 1 n 1 J 10 x 2.178 E 19 2 2 18 2 initial 2 final 18 =  =  = The negative energy simply means that the energy is given off by the electron. Use the absolute value of the energy when calculating wavelength/frequency! nm 487 m 10 x 4.87 J 10 x 4.08 m/s) 10 x s)(3.00 J 10 x (6.626 E hc hc E 7 19 8 34 = = = = = 1 14 7 8 s 10 x 6.16 m 10 x 4.87 m/s 10 x 3.00 c  = = = 6. What is the DeBroglie wavelength in cm of a 12.4 gram hummingbird flying at 1.20 x 10 2 mph? Mass must be in kg so (12.4 g)(1 kg/1000 g) = 0.0124 kg Speed must be in m/s so: m/s 53.6 km 1 m 1000 mi 0.6214 km 1 s 3600 hr 1 hr 1 mi 10 x 1.20 2 = m 10 x 9.97 m/s) kg)(53.6 (0.0124 s J 10 x 6.626 mu h 34 34 = = = 7. Which of the following sets of quantum numbers are unacceptable? Explain your answers. a. (1, 0, +, ) Unacceptable since m l , must be in range l b. (3, 0, 0, +) Acceptable c. (2, 2, 1, +) Unacceptable since l n, but must be from 0 to n1. d. (4, 3, 2, +) Acceptable e. (3, 2, 1, 1) Unacceptable since m s can only be 1/2 f. (2, 3, 2, ) Unacceptable since l cannot be greater than n, must be 0 to n1 g. (5, 3, 3, ) Acceptable 8. For the following subshells give the values of the quantum numbers ( n, l, m l ) and the number of orbitals in each subshell:...
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This note was uploaded on 11/15/2010 for the course CHEM Chem 150 taught by Professor Karenkreutzer during the Winter '05 term at Shoreline.
 Winter '05
 KarenKreutzer
 Electron

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