2. are -6.00 eV, -4.00 eV, and -1.00 eV. The allowed energy levels of a hypothetical hydrogenic (i.e. one electron) atom (a) Draw this atoms energy level diagram. Label each level with the energy and the quantum number. (b) What wavelengths appear in the emission spectrum for this atom? (c) What wavelengths appear in the absorption spectrum for this atom? (d) Are the wavelengths the same in (b) and (c)? EXPLAIN why or why not.

2. are -6.00 eV, -4.00 eV, and -1.00 eV. The allowed energy levels of a hypothetical hydrogenic (i.e. one electron) atom (a) Draw this atoms energy level diagram. Label each level with the energy and the quantum number. (b) What wavelengths appear in the emission spectrum for this atom? (c) What wavelengths appear in the absorption spectrum for this atom? (d) Are the wavelengths the same in (b) and (c)? EXPLAIN why or why not.

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)...

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4. A particular atom has two energy levels with a transition wavelength of 420 nm. At 297 K there are 2.5 1021 atoms in the lower state. (a) How many atoms are in the upper state? (b) Suppose that 1.8 1021 of the atoms in the lower state are pumped to the upper state. How much energy could this system release in a single laser pulse?
Find the largest possible wavelength for electrons (m = 9.11 x 10-31kg emitted from sodium (work function is 3.68 x 10-19 J) when ultra-violet light (E = 5.90 x 10-19 J) shines on it.A. 6.39 x 10-10 mB. 8.10 x 10-10 mC. 1.04 x 10-9 mD. 1.47 x 10-9 mE. There is no maximum wavelength.
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The image represents the gaps between allowed energy levels for electrons. Which model best describes this phenomenon? A. the wave model because electrons orbit the atom's nucleus in a continuous way B. the particle model because electrons are particles C. the wave model because the arrows show that the energy transfer is continuous D. the particle model because the arrows represent discrete particle-like jumps
15 b. Suppose an electron is in a spin state given by x = A(). 8i Find i. the normalization constant A ii. (S.) iii. (S.) and iv. the probability that a measurement of S, will yield h/2.
1a. One photon of light emitted from a hydrogen lamp is measured to have an energy of 0.6618eV. What electron transition is responsible for this photon? Hint: one of the energy levels involved is n = 3. 1b. What is the emission spectrum for a given element and why do different elements have different emission spectra?
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/3.4
4. An H-atom is in is state. a. What is the probability that the electron is found in sphere given by r ≤ ao b. What is (r) ? c. calculate ().
2. Consider the states of hydrogen atom given by (n, l, m) where n a. What is the maximum value of l? If L² is measured what is the maximum possible value that can be obtained? b. What is the maximum value of L₂?
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.
An electron jumps from the n = 4 to the n = 1 level in the hydrogen atom. In a second atom and electron jumps from n = 4 to n = 3. a. Which transition produces a photon with the larger energy? b. Which transition produces the shorter wavelength photon?