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Please answer the whole question with clear workings, thank you.

Answer this none test homework question. Blacked out info is inrellavant to the problem.

3. Excited Ground state state 4. 4.85E-19 J 1 (ground state) 4.42E-19J 4. 1. 3.98E-19 J 3. 3.03E-19J 1. 1 (ground state) Energy Energy emitted paquosqe 2) [30] Energy Levels Above is a schematic of a Hydrogen atom with its first 5 energy levels. On the right is the energy emitted from the transitions (lines pointing down on the diagram). Using the knowledge that energy and wavelength are hc, connected ( E =") you will figure out the wavelength for each of these %3D transitions. E- %3D h = Planck constant = 6.63E-34 J*s C = speed of light = 3E8 m/s 2 = wavelength in meters E = energy in Joules (J) %3D %3D %3D %3D hc %3D E. will be in meters! Divide by 10-9 for nm %3D If you need help converting this to a color easier, try this website once you get the wavelength in nm: https://academo.org/demos/wavelength-to- colour-relationship/