9. Quantum Mechanics

An electron in the n=7 level

Using the Bohr equation, calculate the wavelength (in nm) for the electron transition from n=4 to n=1 in the Lyman series.

Using the Bohr equation, calculate the wavelength of light emitted when an electron in a hydrogen atom transitions from n=2 to n=1.

Using the Bohr equation, calculate the wavelength of light emitted when an electron in a hydrogen atom transitions from n=3 to n=1.

Calculate the wavelength of the light emitted when an electron in a hydrogen atom makes the transition from n=4 to n=2 using the Bohr equation.

Calculate the wavelength of the light emitted when an electron in a hydrogen atom makes the transition from n=5 to n=2 using the Bohr equation.

Calculate the wavelength of the radiation released when an electron moves from n = 4 to n = 2 in a hydrogen atom using the Bohr equation.

Using the Bohr Equation, determine the energy change associated with the electron transition from n=2 to n=5 in the hydrogen atom.

Determine the wavelength of light emitted when an electron in a hydrogen atom makes a transition from n = 5 to n = 3 energy levels.

For hydrogen, what is the wavelength of the photon emitted when an electron drops from the n=3 level to the n=2 level? The Rydberg constant is 1.097 × 10^7 m^-1.

For the electronic transition from n = 3 to n = 8 in the hydrogen atom, calculate the energy change using the Bohr equation.

Which electron transition in a hydrogen atom, starting from n = 10, will produce light of wavelength 3040 nm?

What is ΔE for the transition of an electron from n = 8 to n = 5 in a hydrogen atom using the Bohr equation?

What is the energy (in J) of a photon required to excite an electron from n = 2 to n = 6 in a He⁺ ion? Submit an answer to three significant figures.

What is the energy change of a hydrogen atom undergoing a transition from n=1 to n=3 according to the Bohr model?