The CO molecule loses hv = 0.2690 eV of vibrational energy and gains 0.000479 eV of rotational energy. Hence the energy E that goes into the emitted photon equals 0.2690 eV less 0.000479 eV, or 0.2685 eV. The photon wavelength is?
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The CO molecule loses hv = 0.2690 eV of vibrational energy and gains 0.000479 eV of rotational energy. Hence the energy E that goes into the emitted photon equals 0.2690 eV less 0.000479 eV, or 0.2685 eV. The photon wavelength is?
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- where ?∞ = 1.097 × 10^7 m−1is the Rydberg constant and ? is the atomic number (thenumber of protons found in the nucleus). Calculate the ground state energy of a triplyionised beryllium atom, Be3+ (a beryllium atom with three electrons removed).While most transition metals have work functions corresponding to photon frequencies that are larger (higher) than visible light, alkali and alkaline earth metals have low-energy work functions. For example, calcium has a work function of Po = 4.3419x10-19 J. (a) What is the initial state n; for the hydrogen emission lines at visible wavelengths (i.e., those with nf = 2) for the lowest-energy photon that would eject an electron from calcium? (b) If the colors of the visible hydrogen emission lines (n; = 3 to n; = 6) are red, green, blue and violet, which colors are capable of ejecting the electrons from calcium? (c) The energy of the emitted photon you identified in part (a), is not identical to the workfunction of calcium. Therefore, the electron is ejected from the metal surface with some kinetic energy (i.e., energy is conserved in the photoelectric effect process). What would the velocity of the electron ejected from calcium (in meters per second)?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 Units
- An electron is in a hydrogen atom with n = 2 and ℓ = 1. (a) Find all the possible angles between the orbital angular momentum vector and the z-axis. (b) Suppose the atom absorbs a photon and rises from the n = 2 and ℓ = 1 state to the n = 3 state. Using conversation of angular momentum, what are the possible values of the final value of ℓ in the n = 3 state?What is the energy of the photon that, whenabsorbed by a hydrogen atom, could cause anelectronic transition from the n = 3 state tothe n = 5 state?Answer in units of eV. What energy could cause an electronic transition from the n = 5 state to the n = 7state?Answer in units of eV.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.
- Answer the following. (a) Write out the electronic configuration of the ground state for nitrogen (Z = 7). 1s22s22p11s22s22p2 1s22s22p31s22s22p41s22s22p51s22s22p6 (b) Write out the values for the set of quantum numbers n, ℓ, m, and ms for each of the electrons in nitrogen. (In cases where there are more than one value, enter the positive value first. Enter positive values without a '+' sign in front of them. Include all possible values.) 1s states n = ℓ = m = ms = ms = 2s states n = ℓ = m = ms = ms = 2p states n = ℓ = m = ms = ms = m = ms = ms = m = ms = ms =A researcher observes hydrogen emitting photons of energy 1.89 eV. What are the quantum numbers of the two states involved in the transition that emits these photons?