Figure below shows electron energy levels in a hydrogen atom. The arrows show four possible transitions. n= 4 n = 3 B n= 2 E A n= 1 Which transition emits the longest wavelength?

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.

Infrared light with a wavelength of 1870 nm is emitted from hydrogen. What are the quantum numbers of the two states involved in the transition that emits this light?

What is the frequency of light emitted from a hydrogen atom that makes a transition from the the n = 7 state to the n= 2 state (in Hz)?

What wavelength of light is emitted by a hydrogen atom in which an electron makes a transition from the n = 5 to the n = 2 state? Enter this wavelength expressed in nanometers to one decimal place. 1 nm = 1 x 10-9 m  Assume the Bohr model.