Use equation 3 and then 4 to calculate a wavelength for each of the following el

Question

Use equation 3 and then 4 to calculate a wavelength for each of the following electron transitions from a higher energy level to a lower energy level: n = 6 10 n = 2 corresponds to a A of ___ nm. n = 5 to n = 2 corresponds to a A of. nm. n = 4 to n = 2 corresponds to a A of ___ nm. n = 3 to n = 2 corresponds to a A of_nm. Compare these wavelengths with the corrected wavelengths from your hydrogen discharge bulb and assign a transition to each colored lined you saw. The ___ colored line corresponds to an electron transition from the ____ level to the 2nd level. The ____ colored line corresponds to an electron transition from the _____ level to the 2^nd level. The________colored line corresponds to an electron transition from the ______ level to the 2^nd level. The _____ colored line corresponds to an electron transition from the ______ level to the 2^nd level.

Explanation / Answer

Q4.

for the drop of 3 to 2:

Apply Rydberg Formula

E = R*(1/nf^2 – 1/ni ^2)

R = -2.178*10^-18 J

Nf = final stage/level

Ni = initial stage/level

E = Energy per unit (i.e. J/photon)

E = (-2.178*10^-18)*(1/3^2 – 1/2 ^2)

E = 3.025*10^-19

For the wavelength:

WL = h c / E

h = Planck Constant = 6.626*10^-34 J s

c = speed of particle (i.e. light) = 3*10^8 m/s

E = energy per particle J/photon

WL = (6.626*10^-34)(3*10^8)/(3.025*10^-19)

WL = 6.5712*10^-7 m

to nanometers:

WL = (6.5712*10^-7)(10^9) = 657.2 nm

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