Choose correct graph to show a wave whose frequency is twice as large as the first light wave in the figure below, but whose amplitude is the same. Figure Wavelength- Lower amplitude Dim light Wavelength- The amplitude of a light wave repre- sents the intensity of the light. A bright light is more intense and has greater amplitude than a dim light. -2- OQuestlon #3: Convert the following frequencies into wavelengths, expressing the result in the indicated unit. a. 2.?2 MHz (mm) b. 85.2kHz(m} c. 51.4 Hz(km} d. 3.15 GHz (urn) Question #4: Calculate the energy in joules per photon and kilojoules per mol for the following. a. energy of one photon of red light with wavelength 660.? nm (ji'photon) b. energy of one mole photons of red light with wavelength 660.? nm (ij mol photon) c. energy of one photon of infrared radiation whose wavelength is 1258 m ( jlphoton) d. energy of one mole photons of infrared radiation whose wavelength is 1256 m {ij mol photon) e. energy of one photon of ultraviolet light with a frequency of4921GGDDDDODOOGG Hz {jlphoton} f. energy of one mole photons of ultraviolet light with a frequency of 4921000000000000 Hz (ij mol photon) Question #5: A nitrogen laser puts out a pulse containing 23.4 ml of energy at a wavelength of 337.1 nm. How many photons is this? x 10 photons Question #8: A phototube delivers an electrical current when a beam of light strikes a metal surface inside the tube. Phototubes do not respond to infrared photons. In order for a phototube to generate an electric current, the energy of the photon striking the metal surface of the tube. Highlight the correct option in each underlined statement. Must not or must exceed the binding energy. Infrared light has lower or higher energy than visible light and consequently cannot or m eject electrons from the metal surface in the phototube. Question #7: It requires a minimum of 216.4 kamol to remove an electron from a potassium metal surface. If UV light at 161 m strikes this surface, what is the maximum speed (in mls) of the ejected electrons? Question #8: Determine the frequencies that hydrogen atoms emit in transitions from n = o and n = 5 levels to the n = 3 level. For the l | atom. U\" = 2.18F1st1m2) J. a. What is the frequency (in Hz) of light emitted in the transition from n = 6 to n = 3 level in hydrogen? b. What is the frequency (in Hz) of light emitted in the transition from n = 5 to n = 3 level in hydrogen? c. In what region of the electromagnetic spectrum do these photons lie? Do not abbreviate the name of the spectral region. Infrared, visible, or ultraviolet? Question #1: The density of platinum is 21.45 x 10"3 kg/mAS. d. Calculate the volume (in mASIatom) occupied per platinum atom; e. Estimate the atomic diameter (in m); (The estimate uses the approximation that it is a cubic volume) f. Using this estimation, calculate the thickness of a metal foil (in m) containing 6.7 x 10"6 atomic layers of platinum. Question #14: For each of the following sets of the quantum numbers n and I, write the corresponding orbital notation. For example, n = 1, 1 = 0 would be entered as 15. Question #9: Using the figure below, explain why more lines appear in emission spectra than in absorption spectra. Infrared F (>700 nm) 656 nm 486 nm 434 nm 410 nm Ultraviolet (