a. The energy of a photon emitted in a transition from the n = 3 state to the n = 2 state is b. The energy of the most energetically possible photon emitted is C. The smallest energy of an absorbed photon that will raise a hydrogen atom from its ground state to its first excited state is

1. The two prominent yellow lines in the spectrum of sodium result from transitions to the ground state from the 3p state with the electron spin-up, and from the 3p state with the electron spin-down. The wavelengths these two lines are 589.0 nm and 589.6 nm. (a) Calculate the energies in eV of the photons corresponding to these wavelengths, and the difference in energy of these photons AE. (b) The energy difference you found in part (a) is due to the spin-orbit effect. An electron in the 3p state of sodium experiences an internal magnetic field B, due to the orbital angular momentum. For a magnetic field B₁, the spin-orbit energy splitting is AE = 2µBB₁, where B is the Bohr magneton. Find the orbital magnetic field By from the energy difference AE you found in part (a).

10. A singly ionized helium atom is in the ground state. It absorbs energy and makes a transition to the n = 3 excited state. The ion returns to the ground state by emitting three possible photons. What is the wavelength of the highest energy photon? 3 ƒ60 ssfo f60ª f60 ssf ) ssf60°

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 (C) n = 2 directly to n = 4 (D) n = 2 directly to n = 5 12. What is the minimum energy needed to ionize a hydrogen atom when it is in the n = 2 state? (A) 1.9 eV (B) 3.4 eV (C) 12.2 eV (D) 13.6 eV