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Answer to question 2.9 Part B
Part C : Hydrogen Atom Transitions
The Rydberg formula applies only to hydrogen atoms. It allows us to calculate the wavelengths of radiation that can be emitted or absorbed by the H atom.
Given: Planck's constant h = 6.63×10-34 J·s; speed of light in vacuum c = 3×108 m/s
1.1) Write the Rydberg formula corresponding to the transition from m to p with p > m.
1.2) Calculate the wavelength for the hydrogen transition from n = 5 to n = 2.
1.3) Is the radiation emitted in question 1.2 visible? To which series does it belong?
1.4) Use the Rydberg formula to verify that the energy of the hydrogen atom in energy state n is given by: En = -13.6/n2 eV.
1.5) What transitions compose the Balmer series? What special property do the radiations associated with these transitions have for the H atom?
1.6) Transitions from n > 1 to n = 1 correspond to which series? To which domain do they belong for the H atom (Visible, UV, or IR)?
1.7) What transitions compose the Paschen series? To which domain do they belong for the H atom (Visible, UV, or IR)?
1.8) An atom is characterized by the energy diagram given in document (2). It is in the energy state E2. Can this atom absorb a photon of energy 1.99 eV?
1.9) For the atom in question 1.8, when deexciting from n = 3 to the lowest levels, show with arrows the possible transitions.
1.10) Conversely, if the previous atom undergoes excitation from the ground state to the 3rd excited state, show this transition with an arrow.
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