Evidence for the Quantized Electronic Energy Levels - Atomic Spectra

Heat treatment of muscular pain involves radiation of a wavelength of about 900 nm. Which spectral line of H-atom is suitable for this purpose?

[R_H = 1 × 10⁵ cm⁻¹, h = 6.6 × 10⁻³⁴ Js, c = 3 × 10⁸ ms⁻¹]

Emission transitions in the Paschen series end at orbit n = 3 and start from orbit n and can be represented as v = 3.29 × 10¹⁵ (Hz) [1/3² – 1/n²]

Calculate the value of n if the transition is observed at 1285 nm. Find the region of the spectrum.

What transition in the hydrogen spectrum would have the same wavelength as the Balmer transition n = 4 to n = 2 of He⁺ spectrum?

The spectral lines of atomic hydrogen wave number is equal to the difference between the wave numbers of the following two lines of the Balmer series: 486.1 and 410.2 nm. The wavelength of that line is  ______ × 10^-4 cm.

Calculate the wavelength for the emission transition if it starts from the orbit having radius 1.3225 nm and ends at 211.6 pm. Name the series to which this transition belongs and the region of the spectrum.

Calculate the wave number for the longest wavelength transition in the Balmer series of atomic hydrogen.

What is the wavelength of light emitted when the electron in a hydrogen atom undergoes a transition from an energy level with n = 4 to an energy level with n = 2?

The emission spectrum of hydrogen discovered first and the region of the electromagnetic spectrum in which it belongs, respectively are ______.