Question

Determine the wavelength of the light absorbed when an electron in a hydrogen atom makes a transition from an orbital in which n = 3 to an orbital in which n =6.

Answer in nm please. Thank you.

Answer 1

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)*(1/6^2 – 1/3 ^2)

E = 1.815*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)/(1.815*10^-19 ) = 0.0000010952 m

WL = 0.0000010952*10^9 = 1095.2 nm