Using the Bohr model: Calculate the wavelength of the first spectral lines from the Lyman, Palmer and Passion series of hydrogen atom and helium ion.
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Using the Bohr model: Calculate the wavelength of the first spectral lines from the Lyman, Palmer and Passion series of hydrogen atom and helium ion.
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- The gravitational attraction between electron and proton in a hydrogen atom is weaker than the coulomb attraction by a factor of about 10-40. An alternative way of looking at this fact is to estimate the radius of the first Bohr orbit of a hydrogen atom if the electron and proton were bound by gravitational attraction. You will find the answer interesting.3. The ground state wavefunction for a hydrogen atom can be written as µ=Be*/a where B is a constant and a is the Bohr radius. (a) Show that the probability density of this wavefunction is: P(r)=Cre 2r/0 where C is a constant. (b) Calculate the value of r for which this is a maximum.The so-called Lyman-? photon is the lowest energy photon in the Lyman series of hydrogen and results from an electron transitioning from the n = 2 to the n = 1 energy level. Determine the energy in eV, in joules, and the wavelength in nm of the Lyman-? line. (a) the energy in eV eV(b) the energy in joules J(c) the wavelength in nm nm
- Use the Bohr model and determine the wavelength of light that would ionize a hydrogen atom if the electron were in an excited state (n = 3).Give only typing answer with explanation and conclusion using the Bohr model, determine the energy in joules of the photon produced when an electron in a He+ ion moves from the orbit with n=10 to the orbit with n = 5. (assume that the Bohr constant and radius are 2.179X10^-18J and 5.292X10^-11m)Physics please written by hand.
- Why is the analysis of the helium atom much more complex than that of the hydrogen atom, either in a Bohr type of model or using the Schrödinger equation?please help as soon as possible1a) Use the table below to determine the energy in eV of the photon absorbed when an electron jumps up from the n = 1 orbit to the n = 2 orbit of a hydrogen atom. =_________ eV 1b ) Use the table shown below to determine the energy in eV of the photon emitted when an electron jumps down from the n = 3 orbit to the n = 2 orbit of a hydrogen atom.=___________ eV
- Determine the wavelengths of the photons from the transition of hydrogen electron from n1 = 2 to n2 = 7.What is the wavelength of the radiation absorbed when an electron move from n = 2 to n = 5 for a helium +1 ion?O 6.21 * 10-19 J For which of the following transitions does the light emitted have the longest wavelength? On=4 to n = 3 O n- 4 to n = 2 On= 4 to n = 1 O n= 3 to n = 2 O n = 2 to n = 1 Whish f tho following ic bvdrogen like atom (to which Bohr's model could