Question

When an electron moves from level n= 4 to level n =5 in an excited hydrogen atom, what amount of energy is required for this electronic transition?

Please show your full work!! Where you got number from step by step

Answer 1

Here photon will be captured and it will excite the atom

1/wavelength = -R* (1/nf^2 - 1/ni^2)

R is Rydberg constant. R = 1.097*10^7

1/wavelength = - R* (1/nf^2 - 1/ni^2)

1/wavelength = - 1.097*10^7* (1/5^2 - 1/4^2)

wavelength = 4.077*10^-6 m

wavelength = 4077 nm

we have:

wavelength = 4.077*10^-6 m

we have below equation to be used:

Energy = Planck constant*speed of light/wavelength

=(6.626*10^-34 J.s)*(3.0*10^8 m/s)/(4.077*10^-6 m)

= 4.88*10^-20 J

Answer: 4.88*10^-20 J