A hypothetical molecular laser works in 3 level energy system. The energies of the levels. E₁, E2, and E3 are 0 eV, 0.18 eV and 0.30 eV respectively. If the laser transition takes place between the levels E2 and E₁ find the (1) wavelength of radiation that excites the molecules for the laser action.
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- A laser emits light at a wavelength of 678 nm. How many photons are required to emit 1 joule of energy?These are energy levels in a laser (not to scale). Level 1, 2, 3, are: -13, -5, -3 eV respectively. Electronic transition A emits a photon of wavelength Ch. 29.3 nm.A hypothetical molecular laser works in 3 level energy system. The energies of the levels. E₁, E2, and E3 are 0 eV, 0.18 eV and 0.30 eV respectively. If the laser transition takes place between the levels E₂ and E₁ find the (1) wavelength of radiation that excites the molecules for the laser action. 1
- Chapter 39, Problem 017 An electron in the n, state in the finite potential well of of Figure (a) absorbs 650 eV of energy from an external source. U U(x) Ug L. (a) Using the energy-level diagram of Figure (b), determine the electron's kinetic energy after this absorption, assuming that the electron moves to a position for which x > L.Chapter 39, Problem 044 A hydrogen atom in a state having a binding energy (the energy required to remove an electron) of -1.51 eV makes a transition to a state with an excitation energy (the difference between the energy of the state and that of the ground state) of 10.200 eV. (a) What is the energy of the photon emitted as a result of the transition? What are the (b) higher quantum number and (c) lower quantum number of the transition producing this emission? Use -13.60 eV as the binding energy of an electron in the ground state. (a) Number Units (b) Number Units (c) Number UnitsA certain laser emits light of wavelength 632.8 nm. What is the frequency of radiation and energy difference between lasing levels?
- Suppose you recently discovered a hydrogen like element that has only one electron orbiting around a nucleus containing a proton and a neutron. You found the ground state energy of the electron to be -16 eV. What will be the energy of this electron when it is on the excited state shown in the sketch? Note that all other possible intermediate states are shown by dashed lines. Electron is here Ground state 1.0 eV 16 eV - 1.0 eV -4.0 eV 4.0 eVInfrared light with a wavelength of 1870 nm is emitted from hydrogen. What are the quantum numbers of the two states involved in the transition that emits this light?Rose bengal is a chromophore used in biological staining that has an absorption maximum at 559.1 nm and several other shorter wavelength absorption bands in the ultraviolet and visible regions of the spectrum when dissolved in ethanol. What is the energy difference, in kilojoules per mole, between the absorption maximum at 559.1 nm and a band at 221.5 nm? E = kJ/mol
- Some of the most powerful lasers are based on the energy levels of neodymium in solids, such as glass, as shown . (a) What average wavelength light can pump the neodymium into the levels above its metastable state? (b) Verify that the 1.17 eV transition produces1.06 μm radiation.A laser emits a pulse of light with wavelength 532 nm. If the total energy contained in the pulse is 1.2 J, the number of photons in the pulse is?A monochromatic laser is exciting hydrogen atoms from the n = 2 state to the n = 5 state. PART A: What is the longest wavelength that is observed? PART B: What is the shortest wavelength observed?