For a hydrogen atom, calculate the wavelength of light (in m) that would be emitted for the orbital transition of n(initial) = 6 to n(final) = 1. Submit an answer to four significant figures. The Rydberg constant is 1.09678 x 10⁷ m⁻¹.

For a hydrogen atom, calculate the wavelength of light (in m) that would be emitted for the orbital transition of n(initial) = 5 to n(final) = 1. Submit an answer to four significant figures. The Rydberg constant is 1.09678 x 107 m¯¹. 1 4 7 +/- 2 5 8 m 3 6 9 0 X x 100

Gold has a work function, Φ, of 5.47 ev. If a sample of gold is bombarded with 191 nm photons, what will be the velocity (in m/s) of the photo-ejected electrons? (1 eV = 1.60 × 10⁻¹⁹ J, the mass of an electron is 9.109 x 10⁻³¹ kg, and Planck's constant is 6.626 x 10⁻³⁴ Js.)

Consider light at 375 nm.  What is the energy of one mole of photons of light with a wavelength of 375 nm?  Answer in J in scientific notation to 3 significant figures using the format of 6.022E23 for 6.022 x 10 23.   Calculate the wavelength associated with an electron moving at 35% of the speed of light.  The mass of an electron is 9.109 x 10 –28 g.  (HINT:  use the de Broglie equation).  Answer in meters in scientific notation to 3 significant figures using the format of 6.022E23 for 6.022 x 10 23.