The figure below depicts the first four energy levels in a hydrogen atom. The three transitions shown as arrows emit ultraviolet light and occur at wavelengths of 121.566 nm, 102.583 nm, and 97.524 nm, respectively. Planck's constant is 6.62607 × 10-34 Js and the speed of light is 2.99792 × 108 m/s. n = 4 E n = 3 n = 2 n = 1 a Find the frequency of light that would be emitted in a transition from the state labeled as n = 4 to the state labeled as n = 3. Frequency = Hz b Find the wavelength of light that would be emitted when a hydrogen atom undergoes the transition from the state labeled as n = 4 to the state labeled as n =2. Express your answer in nm. Wavelength= nm Previous Next