H-like atom: Bohr's model part 1
You carry out a theoretical work on absorption of alpha rays, passing on to a study of the structure of atoms on the basis of Rutherford's discovery of the atomic nucleus. By introducing conceptions borrowed from Quantum Theory established by Planck, you succeeded in working out and presenting a picture of atomic structure that, with later improvements, still fitly serves as an elucidation of the physical & chemical properties of the elements.
You started with H-like atom (ie - 1 electron circulating around nucleus carrying +Z charge). You realize Coulomb force of attraction on the electron, Fcoul, provides the acceleration a towards the nucleus: Fcoul = Ze2/(4*pi*epsilon0*r2) = mea = mev2/r
In order to quantize the energy level of the electron to
generate discrete spectra to fit the experimental observation, you
propose 2nd Bohr condition, quantization of angular momentum:
angular momentum = mevr = nh/2pi where n = 1,2,3,...
a) Given the above 2 equations, please show by algebra that the radius of the electron (ie - the distance between the electron and nucleus) is quantized (ie - only some specific values are allowed):
rn = (epsilon0*n2h2)/(nZe2me) = (n2/Z)a0
b) Calculate the value of the constant, ao, in the SI units. (This constant is later called Bohr radius)
c) Since radius is quantized, following the 2nd Bohr condition, the velocity of the electron must be quantized, too. Please show by algebra that vn=nh/(2pi*mern) = Ze2/(2*epsilon0*nh)
H-like atom: Bohr's model part 1 You carry out a theoretical work on absorption of alpha...
please Solve part D and E!!!!! PLEASE AND THANK YOU acc1 Our discussion of the Bohr model of the hydrogen atom was non-relativistic throughout, which was justified because the velocity of the electron in the nth state of Bohr's hydrogen atom was v= (1) 1377 where a = 1 is the fine-structure constant, and qe is the electron charge, ħ is (the reduced) Planck's constant, and c is the speed of light. Clearly, as n grows, the speed does become...
3 (b) The energy of a Bohr atom in the n-th excited state is given by the formula E--a2mc2 2,7, where α-e2/(4πέρ,10hc)-1 /137, m is the electron mass and e denotes the electron electric charge. i) Why is the total energy negative? Explain briefly your answer. ii) What is the radius of the electron in the n-th excited state in the Bohr atom? To answer that correctly follow the next steps Use Bohr's angular momentum quantization principle to obtain an...