An electron (a) falls from the n=4 to the n=2 orbit in a hydrogen atom and an electron (b) fell from the n=4 orbit to the n=1 orbit.  a. Which electron will produce a photon with a longer wavelength?

g. Diagram the electron transition that occurs when photons having energy equal to 5.00 x 10-¹⁹ J are released n = 5 n = 4 n = 3 n = 2 n=1

A hydrogen atom makes a transition from n=4 to n=1. The wavelength of the photon emitted by the atom is?

Consider  hydrogen atoms with electrons randomly distributed in the n=1, 2, 3 and 4 orbits. Calculate the frequencies and wavelengths of the light produced by the transitions described above.

What wavelength of light is required to excite an electron to the n = 6 state in hydrogen? b. If that electron then relaxes to the n = 3 state, what is the energy of the photon emitted? What region of the electromagnetic spectrum is this emitted photon in?

4.Make a prediction using your model. If an electron were to emit a photon and move from the n=3 level to the n=1 level, what wavelength of light would it emit? (Hint: use the Ryberg equation) Would this be a bigger energy What would be the energy change for this transition? change or a smaller energy change that the transition from the n=3 to the n=2 transition? Would you be able to see this energy change (will it be visible light?) What part of the electromagnetic spectrum should you look in to find these photons, the ultraviolet or the infrared?

5. An electron in a hydrogen atom makes a transition from ann= 2 orbital to an n = 5 orbital. a. For this electron transition, is energy being absorbed or released? Circle one. ABSORBED RELEASED b. Calculate the energy difference for this transition and the wavelength (in nanometers) of the photon involved in this transition.

8. If you have light that travels with a frequency of 9x1012 Hz. What is the energy of this light?

The electron in an (unbound) hydrogen atom (H(g)) is excited from the ground state to the n=3 state.Which of the following statements are true and which are false. 1. it takes less energy to ionize the electron from n=3 than it does from the ground state.2. The wavelength of the light emitted when the electron returns to the ground state from n=3 is the same as the wavelength of light absorbed to go from n=1 to n=3.3. the electron is farther from the nucleus on average in the n=3 state than in the ground state.4. The first excited state corresponds to n=3.5. The wavelength of light emitted when the electron drops from n=3 to n=2 is shorter than the wavelength of light emitted if the electron falls from n=3 to n=1.

A hydrogen atom in its ground state absorbs a photon with a wavelength (A) of 122 nm. In what energy level does the electron now reside? O n = 1 On=2 O n = 3 On = 4 none of the above