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Chemistry Forums for Students => Physical Chemistry Forum => Topic started by: slee on July 09, 2017, 08:56:19 PM

Title: Hydrogen spectral series - Energy levels
Post by: slee on July 09, 2017, 08:56:19 PM

I am using the equation E=hc/λ to calculate the photon energy for each wavelength in Hydrogen spectral series.

What I found was that energy required for electrons to jump to a particular level differed for Lyman, Balmer and Paschen series.

For example, energy required to transition to n4 are 2.048x10^-18 joules (Lyman), 4.577x10^-19 joules (Balmer) and 1.059x10^-19 joules (Paschen).

My questions are:

• Can you explain to me why energy required to transition to the same levels differed for each experiment?
• I know Lyman's experiment was conducted in a vacuum and Balmer/Paschen in air, so how does a vacuum effect the required energy for electrons to transition states?
• Did temperature also play a part in the differences in these experiments?

Thanks.


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Title: Re: Hydrogen spectral series - Energy levels
Post by: Irlanur on July 10, 2017, 03:43:28 AM

Quote

Can you explain to me why energy required to transition to the same levels differed for each experiment?

It's a TRANSITION, this involves two levels. The energy of the radiation is given by the energy difference of the two levels.