A.) The relation between different transitions of Hydrogen atom and the corresponding wavelength of the photon emitted is 1/λ = RH [1/n12 - 1/n22 ] where RH is Rydberg's constant whose value is 1.0973731 x 107 m-1
when the transition is from n2 to n1
so putting n2 =3 and n1 =2 , we get
1/λ = 1.0973731 x 107 [ 1/22 - 1/32 ]
λ = 6.561123104 x 10-7 m ~ 656 nm
B.) Given that, the atom is originally in the ground state. So, n1 =1 . For, longest wavelength the energy corresponding should be minimum. Which means if n1 =1 is fixed then n2 should be 2 for minimum energy and hence maximum wavelength.
putting n2 = 2 and n1 =1 , we get
1/λ = 1.0973731 x 107 [ 1/12 - 1/22 ]
λ = 1.215022797 x 10-7 m ~ 121 nm
C.) The same expression for various transitions of hydrogen atom written in terms of energies looks like this
hν = E2 - E1 = -13.6 [ 1/n12 - 1/ n22 ] eV
Also given that the hydrogen atom is in its ground state which means n1 = 1 .
putting n2 = 3 gives - 12.1 eV
which is the closest to the given number (12.2 eV).
Under any circumstances the colliding electron is NOT going to go to one of the energy levels of the atom but, if it can transfer/ deposit 12.1 eV of its energy to the already existing electron in the ground state, then the electron in the ground state might get excited to the third level (n = 3) from the ground state (n = 1). But still, the question says 12.2 eV and not 12.1 eV. So, I would say that nothing really happens here.
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