what is the wavelength of a line in the calmer series of the hydrogen spectrum, if the transition occurs from ni= 5 to nf = 2 ? remember the rydberg constant is 1.097 x 10^-2 nm^-1

Calculate E (energy), v (frequency), and the wavelength in nanometer for a H-atom. Rydberg constant is 2.179 x 10-18 . n=1 to n=3 transition. Is this transition absorbance or an emission? Please put your final answers (energy, frequency, wavelength, and whether it is emission or absorbance) here but show your calculations work in a separate sheet.

What is the wavelength in nm of a photon emitted from an H atom if an electron transfers from n=6 to n=3   RH = Rydberg constant = 1.097 x 10 -2  nm-1

Pieces of potassium (Φ  = 3.68 × 10–19 J) and sodium (Φ  = 4.41 × 10–19 J) metal are exposed to radiation of wavelength 315 nm. What is the velocity of the electrons from potassium?   What is the velocity of the electrons from sodium?

Choose the statement which correctly indicates whether energy is emitted or absorbed and the wavelength of the energy emitted or absorbed (in meters) when the following electronic transition occurs in hydrogen:An electron moves from the n=4 to the n=2 energy level. The value of the Rydberg constant is RH = 1.097 x 107 m-1.

which energy level transition for a hydrogen atom would emit the photon with the lowest frequecy n=4 to n=1 n=5 to n=1 n=2 to n=3 n=5 to n=4

Calculate the wavelength of light emitted as an electron undergoes a transition from level n= 110 to n = 109. In what region of the electromagneticspectrum does this lie?

Calculate the predicted wavelength of a photon that is produced due to the transition of a hydrogen electron from the fifth shell to the second shell. The Rydberg constant value is 2.179 x 10-18J.