A hydrogen vapour lamp emits four lines in the visible light range (the Balmer series). These correspond to transitions from nu = 3, 4 ,5 and 6 to nl= 2.Each of the lines correspond to a different colour as listed below. For the transition from nu = 3, what colour is the photon of light produced?

In a hydrogen atom, a transition from the 2nd to the 1st excited state will produceGroup of answer choicesan ultraviolet spectral line.no emission line.the Balmer series line in visible light..three different emission lines.a dark absorption line.

The spectrum from a hydrogen vapour lamp is measured and four lines in the visible light range are observed. These lines are the so-called Balmer series, where an electron makes a transition from a higher level to the second energy level (nl= 2).From the measurements of the wavelengths of these four lines, four determinations of the Rydberg constant R were made. These are:For nu= 3, R = 9.96 µm-1For nu= 4, R = 9.65 µm-1For nu= 5, R = 9.72 µm-1For nu= 6, R = 11.9 µm-1An average value of R can be found. Calculate the uncertainty in this average R (use the mean error technique).Express you answer in µm-1 to two decimal places.

In which transition of hydrogen atom is the wavelength of 486.1 nm produced?A. Balmer SeriesB. Paschen SeriesC. Lyman seriesD. Pfund series

A hydrogen spectrum is observed using a hydrogen lamp, an emission line with a wavelength of 398 nm is associated with excited electrons dropping down to the n = 2 shell. The initial n value for this transition is [Ans].

Which transition occurs when light with a wavelength of 434 nm is emitted by a hydrogen atom? Group of answer choicesThe electron falls from n=5 to n=2The electron falls from n=4 to n=2The electron jumps from n=2 to n=4The electron jumps from n=2 to n=5