An electron in a hydrogen atom transitioning from orbit n = 7 releases a photon whose frequency equals 6.44196 x 1013 Hz. Determine the orbit to which the electron transitioned.

use the bohr equation to find the wavelength of the photon emitted when an H atom undergoes a transition from n=5 to n=2

A photon is emitted during the transition from the n = 7 state to the n = 1 state in the hydrogen atom. Note: Rydberg constant: 2.18x10-18 J Calculate the wavelength of this photon

A mercury atom emits light at many wavelengths, two of which are at (1) 404.7 nm and (2) 435.8 nm. Both of these transitions are to the same final state. Determine the energy of each emitted wavelength (in J). A E1 = 7.908 x 10-19 J and E2 = 6.558 x10-19 J B E1 = 5.908 x 10-19 J and E2 = 5.558 x10-19J E1 = 4.908 x 1019 J and E2 = 4.558 x10-19J D) E1 = 4.628 x 10-19 J and E2 = 4.968 x10-19 J

An electron in a hydrogen atom relaxes to the n = 4 level, emitting a photon of 114 THz. What is thevalue of n for the level in which the electron originated?

COMPLETE THE TABLE. Reactions: (1) K2Cr2O7 + SnCl2 + HCl → CrCl3 + SnCl4 + KCl + H2O(2)    KClO3 + C12H22O11 → KCl + H2O + CO2

An electron makes a transition from ground state to n=5 state. Now the same electron makes a spontaneous emission and comes back to the ground state. Determine the frequency of the photon emitted during the process.