11. In the Balmer series, during which of the following energy state changes of the hydrogen atom is the photon with the most energy emitted? (A) n = 5 directly to n = 2 (B) n = 4 directly to n = 2
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A: ni = 7 nf = 4 λ = ?
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- A hydrogen atom makes a downward transition from the n 19 state to the n-5 state. Find the wavelength of the emitted photon. O 2 45 um 2.94 μm O 147 um O1.96 umThe Lyman series in the hydrogen emission spectrum is formed by electron transitions from n;> 1 to nf= 1. What is the wavelength of the series limit (the lower bound of the wavelengths in the series)? nmThe so-called Lyman-a photon is the lowest energy photon in the Lyman series of hydrogen and results from an electron transitioning from the n = 2 to the n = 1 energy level. Determine the energy in eV and the wavelength in nm of a Lyman-a photon. HINT (a) the energy in eV eV (b) the wavelength in nm nm
- 3. Suppose an electron in a hydrogen atom is in a 2p state, and the radial wavefunction is (2a.)3/2 /3a. 2ao , where a, is the Bohr radius. (a) 2-axis? What possible angles might the angular momentum vector L make with the (b) What is the most probable radius (in terms of a,) at which the electron is found? (c) What is the expectation value of r in this state? Note: xe-"dx = 120. (p) S° x*e-dx = 23.91. What is the probability of finding such an electron between a, and oo? Note:An electron is excited from the n=1 ground state to the n=3 state in a hydrogen atom. Which of the following statements are true? Correct the false statements to make them true. (It may help to draw the Bohr model of the atom with the corresponding electron orbits.)a. It takes more energy to ionize (completely remove) the electron from n = 3 than from the ground state.b. The electron is farther from the nucleus on average in the n = 3 state than in the n = 1 state.c. The wavelength of light emitted if the electron drops from n = 3 to n = 2 will be shorter than the wavelength of light emitted if the electron falls from n = 3 to n = 1.d. The wavelength of light emitted when the electron returns to the ground state from n = 3 will be the same as the wavelength of light absorbed to go from n = 1 to n = 3.e. For n = 3, the electron is in the first excited state.ご A 国 Using the Rydberg equation provided below determine the wavelength as well as the energy for a single photon emitted by the hydrogen atom's electron moving fromn 6 to n = 2. (more than one choice) %3D 1 = 1.10x10' m 1 1 where n>m 1 E=h c where h=6.63x10-3* J•s c=3.00 x10° m/s
- 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.- - - The first five energy levels of the hydrogen atom are at n 1, 13.6 eV; n = 2, 3.4 eV; n = 3, 1.51 eV; n = 4, -0.85 eV; n = 5, -0.54 eV. A hydrogen discharge lamp gives an infrared spectrum that includes a sharp line at a wavelength of 4 μm, coming from electrons excited by the discharge to a higher level, and then jump down to a lower level. Determine the energy lost by these electrons, and identify the higher and lower levels involved.In the series of hydrogen; a) What value of n is associated with the 550-nm spectral line? b) Could this wavelength be associated with the Paschen series or the Balmer 16 series? c) Find the shortest wavelength of the radiation emitted with the Lyman series?