Prelaboratory Exercise for the Atomic Emission and Absorption Experiment The spe

Question

Prelaboratory Exercise for the Atomic Emission and Absorption Experiment The spectroscopes used in our lab are scaled in nanometer units. You will work with three of the four possible Balmer series transitions of Hydrogen whose lines are in the visible region of the electromagnetic spectrum. Answer the following questions about the faint purple line whose wavelength is 410.1nm that is noted in the emission spectrum of hydrogen. This is the line you will not be able to see with our spectroscopes. 1. A. Since n1 -2 for all the lines in the Balmer series of hydrogen, use the Rydberg equation to calculate n2. B. Caleulate the energy (J) associated with this wavelength (Elight emitted). C. Recognizing that the energy of n-2 in hydrogen equals 16.3 x101" J, caleulate the energy of the level found in question 1A. from which the electron is falling when the energy calculated in 1B is emitted. OVER

Explanation / Answer

wavenumber(1/l) = 109737(1/n1^2 - 1/n2^2)   (n2>n1)

rydberg constant = 109737 cm-1

wavenumber = 1/ wavelength(l)

n1 = 2 , n2 = ?

(1/(410.1*10^-7)) =109737((1/2^2)-(1/x^2))

   n2 = x = 6

b. Energy(E) = hc/l

   h = planks constant = 6.625*10^-34 j.s

   c = light velocity = 3*10^8 m/s

   l = wavelength = 410.1 nm = 410.1*10^-9 m

E = (6.625*10^-34)*(3*10^8)/(410.1*10^-9)

     = 4.85*10^-19 joule

c. energy electron in n2 = 6 th level = 16.3*10^-19+4.85*10^-19

                          = 2.115*10^-18 joule

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