For a hydrogen atom in its ground state, use the Bohr model to compute the orbital speed of th
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- (1) Find the average orbital radius for the electron in the 3p state of hydrogen. Compare your answer with the radius of the Bohr orbit for n=3. (2) What is the probability that this electron is outside the radius given by the Bohr model?Chapter 39, Problem 044 A hydrogen atom in a state having a binding energy (the energy required to remove an electron) of -1.51 eV makes a transition to a state with an excitation energy (the difference between the energy of the state and that of the ground state) of 10.200 eV. (a) What is the energy of the photon emitted as a result of the transition? What are the (b) higher quantum number and (c) lower quantum number of the transition producing this emission? Use -13.60 eV as the binding energy of an electron in the ground state. (a) Number Units (b) Number Units (c) Number UnitsThe radial probability density of a hydrogen wavefunction in the 1s state is given by P(r) = |4rr2 (R13 (r))²| and the radial wavefunction R1s (r) = a0 , where ao is 3/2 the Bohr radius. Using the standard integral x"e - ka dx n! calculate the standard deviation in the radial position from the nucleus for the 1s state in the Hydrogen atom. Give your answer in units of the Bohr radius ao.
- (a) What is the magnitude of the orbital angular momentum in a state with e = 2? (b) What is the magnitude of its largest projection on an imposed axis? (a) Number 2.50998008 Units J.s (b) Number 2.11 Units J.sCompute and compare the electrostatic and gravitational forces in the classical hydrogen atom, assuming a radius 5.3 x 10-11 m.