The following wavelengths are found among the many radiations emitted by singly ionized helium: 24.30 nm, 25.63 nm, 102.5 nm, 320.4 nm. If we group the transitions in helium as we did in hydrogen by identifying the final state n0 and initial state n, to which series does each transition belong?

The following wavelengths are found among the many radiations emitted by singly ionized helium: 24.30 nm, 25.63 nm, 102.5 nm, 320.4 nm. If we group the transitions in helium as we did in hydrogen by identifying the final state n0 and initial state n, to which series does each transition belong?

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter1: Units, Trigonometry. And Vectors

Section: Chapter Questions

Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...

See similar textbooks

Similar questions

The average speed of a hydrogen molecule at 20o C is 1930 m/s. What is the wavelength of the H2 molecule at this temperature?
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
A single electron ion MZ-1)+ with atomic number Z<84 emits a photon during an unknown electronic transition from some initial state n; to some final state nf. The photon then strikes an osmium surface, which has a work function O = 5.93 eV and causes an electron to be emitted. Many such photons create a beam of electrons (all with the same kinetic energy) that is directed at a single crystal nickel sample at normal incidence. The electrons are scattered from the crystal and it is observed that they do so with only two (2) non-zero diffraction angles (i.e., 2 different values of 0). From the DeBroglie-Bragg relation it is determined that the diffraction corresponds to a lattice spacing of a = 352.4 pm.
A photon is emitted during the transition from the n = 7 state to the n = 1 state in the hydrogen atom. Note: Rydberg constant: 2.18x10-18 J Can this photon eject an electron from cesium metal (work function of Cs is 3.42x10-19 J) and why? What would be the speed of that electron once is ejected (mass electron is 9.109x10-31 kg)?
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.
The L series of the characteristic x-ray spectrum of tungsten contains wavelengths of 0.1099 nm and 0.1282 nm. The L-shell ionization energy is 11.544 keV. Which x-ray wavelength corresponds to an N → L transition? Determine the ionization energies of the M and N shells: If the incident electrons were accelerated through a 40.00 keV potential difference before striking the target, find the shortest wavelength of the emitted radiation:
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.
Calculate the shortest and longest wavelengths of Balmer series of hydrogen atom. Given R = 1.097 × 107m1.
You are doing a senior thesis project that involves research into astronomical observations. In interstellar space, highly excited hydrogen atoms called Rydberg atoms have been observed, and can be useful in analyzing astronomical environments. In these atoms, the quantum number n is very high. In preparation for an upcoming publication, your supervisor asks you to determine the quantum number of a Rydberg atom for which the classical and quantum predictions of the wavelength of a Δn = 1 transition are within 0.500% of each other.
The transition from the first excited state to the ground state in potassium results in the emission of a photon with lambda= 770 nm. If potassium vapor is used in a Franck-Hertz experiment, at what voltage would you expect to see the first decrease in current?
Consider a two-electron spin system in a singlet state. a. If a measurement of one of the electrons shows that it is in a state with sz = 1/2, what is the probability of obtaining another state with sz= +1/2? b. If a measurement of one of the electrons shows that it is in a state with sx = 1/2, what is the probability of obtaining another state with sy = +1/2?