An electron is in the sixth energy level of a hydrogen atom. The atom emits a photon which causes the electron to drop directly to the third energy level. Find the change in the Bohr radius of the electron's orbit in units of nm. (A) 3.17 (B) 4.18 (C) 1.428 (D) 2.29 Find the frequency of the emitted photon in units of 10¹4 Hz. (A) 9.53 (B) 8.36 (C) 4.51 (D) 2.74 (E) 5.41 (E) 5.96
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- The electron of a hydrogen atom requires 1.633*10-18 J to be excited from n = 1 Bohr energy level to the n = 2 level. This energy can be obtained from the absorption of a photon. What would be the wavelength of this photon?Consider a Bohr model of doubly ionized lithium. (a) Write an expression similar to E, = -13.6/n² eV for the energy levels of the sole remaining electron. (Use the following as necessary: n.) 122.4 E, v ev n° (b) Find the energy corresponding to n = 5. (Enter your answer to at least one decimal place.) -4.89 ev (c) Find the energy corresponding to n = 3. (Enter your answer to at least one decimal place.) -13.6 ev (d) Calculate the energy of the photon emitted when the electron transitions from the fifth energy level to the third energy level. Express the answer both in electron volts and in joules. 8.71 V ev 1.395e-18 (e) Find the frequency and wavelength of the emitted photon. 6.2e15 Your response differs from the correct answer by more than 100%. Hz 48 Your response differs from the correct answer by more than 10%. Double check your calculations. nm (f) In what part of the spectrum is the emitted light? O visible light region O infrared region O gamma ray region O x-ray region…Give only typing answer with explanation and conclusion using the Bohr model, determine the energy in joules of the photon produced when an electron in a He+ ion moves from the orbit with n=10 to the orbit with n = 5. (assume that the Bohr constant and radius are 2.179X10^-18J and 5.292X10^-11m)
- Which of these expressions would yield the wavelength of light in meters emitted when an electron drops from orbit n = 3 to n = 2 in a Bohr hydrogen atom? Given h = 4.14 x 10-15 eVs and c = 3.00 x 108 m/s. a. 1.89/hxc b. hc/1.89 c. 1.89 x h x c d. (1.51 + 3.4)/hc e. hc/3.45 6 À (x10-² nm) 7 8 9 10 Relative intensity Mo 9 9 12 vith → To 15.2 → To 37.24. In a hydrogen atom, the electron makes ω = 6×1015 rev/s (recall that this is the angular velocity) around the nucleus. We want to calculate how much current flows through a point in the orbit. (a) Calculate the time period of the orbit. Start by converting ω into rad/s. (b) Use the definition of current to calculate I due to the revolution of the electron around the nucleus.
- Which of these expressions would yield the wavelength of light in meters emitted when an electron drops from orbit n = 3 to n = 2 in a Bohr hydrogen atom? Given h = 4.14 x 10-15 eVs and c = 3.00 x 108m/s. a. 1.89 x h x c b. hc/3.4 c. (1.51 + 3.4)/hc d. hc/1.89 e. 1.89/hxcWhat wavelength of light is emitted by a hydrogen atom in which an electron makes a transition from the n = 5 to the n = 2 state? Enter this wavelength expressed in nanometers to one decimal place. 1 nm = 1 x 10-9 m Assume the Bohr model.The Balmer series in hydrogen includes the Paschen series. has four lines in the ultraviolet. O includes both the Paschen series and the Lyman series. O has four lines in the visible. O includes the Lyman series.