Consider the transition from the energy levels n = 3 to n = 5, What is the wavel

Question

Consider the transition from the energy levels n = 3 to n = 5, What is the wavelength associated with this transition, In nm? You may enter answers using e-notation For example. 1.3 times 10^-8 would be entered as 13e- 8 Determine the energy in J of the lower n level using the equation, E_n = -R_H/n^2? Step 2 Determine the energy in J of the higher n level using the equation E_n = 2_H/n^2 Determine the energy reference between the two n levels by subtracting the energy of the lower in level Use Planck's equation E = hy. to solve for the frequency of light of the energy determined in Step 3 Step 5 Use me equation c = lambda v. to determine the wavelength of light in Units of meters c = 2.998 times 10^8 m/s.

Explanation / Answer

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 – 1/5 ^2)

E = 1.5488*10^-19 J/photon

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)/(1.5488*10^-19)

WL = 1.2834*10^-6 m

to nanometers:

WL = (1.2834*10^-6 )(10^9) = 1283.4 nm

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