emitted or absorbed when the following electronic transitions occur in hydrogen:
ID: 556622 • Letter: E
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emitted or absorbed when the following electronic transitions occur in hydrogen: (a) from n-4 to n 2, (b) from an orbit of radium 2.12 A to one of radius 8.46 A, (e) an electron adds to the H' ion and ends up in the n 3 shell? 67) (a) What is the wavelength in meters of ultraviolet light with V 5.5 x 10's (b) what is the wavelength (in nanometers) of light having a frequency of 8.6 × 1013 Hz? (c) What is the frequency of a microwave with -4.33 x 103 m (d) What is the frequency (in Hz) of light having a wavelength of 566 nm? (e) Calculate the energy of a photon of radiation whose wavelength is 161 nm. 68) A photon has a frequency of 6.0 x 10 Hz. (a) Convert this frequency into wavelength (nm),. Does this frequency fall in the visible region? (b) Calculate the energy (in joules) of this photon. (c) Calculate the energy (in joules) of I mole of photons all with this frequency 69) when light of frequency equal to 2.1 1 x 10s st shines on the surface of gold metal, the kinetic energy of ejected electrons is found to be 5.83 × 10-19 J. What is the work function ofgod? 70) Consider the following energy levels of a hypothetical atom - 1.0×10-19J _ 5.0 x 10 19 J E 10x 10-19 J E 15 x10-19 J (a)) What is the wavelength of the photon needed to excite an electron from Ei to Es? (b) What is the energy (in joules) a photon must have in order to excite an electron from E2 to Es? (c) When an electron drops from the E level to the E level, the atom is said to undergo emission. Calculate the wavelength of the photon emitted in this process. 71) Calculate the frequeney (Hz) and wavelength (nm) of the emitted photon when an electron drops from the n -4 to the n-2 level in a hydrogen atom. (Hint: The value of Rydberg's constant is 2.18 x 10-18 J) wavelength in the hydrogen emission spectrum is 1280 nm. What are the initial and final states of the 72) One transition responsible for this emission? (Hint. The value of Rydberg's constant is 2.18 x 10-18 73) Calculate the de Broglie wavelength of a helium atom whose speed is equal to the root-mean-square speed at 20°C. 74) (a) Protons can be accelerated to speeds near that of light in particle accelerators. Estimate the wavelength (in nm) of such a proton moving at 2.90x 10 m/s. (Mass of a proton 1.673 x 102 kg.) (b) What is the de Broglie wavelength, in cm , of a 12.4-g hummingbird flying at 1.20 × 102 mph? ( 1 mile = 1.61 km ) (Hint: Planck's constant, 6.63 x 10 J-s)Explanation / Answer
(a) from n=4 to n=2
Answer: Since the electron is being moved from higher energy state to lower energy state, the energy will be released.
The answer is energy emitted.
(b) from an orbit of radius 2.12 A to one of the radius 8.46 A
Here, the radius of the atom is increasing from 2.12 A to 8.46 A. That means, the principal quantum number will be large when the radius is increased. Therefore, the electron is moving from lower n value to higher n value. Hence, the electron is being excited to a higher energy state. SO, energy is absorbed.
(C) an electron adds to the H+ ion and ends up in the n=3 shell
Here, the energy is Emitted. Becuase, After adding an electron to H+, it gains neutrality. However, the n=3 shell is not the lowest energy level.
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