b) Choose the best explanation from among the following:I. The de Broglie wavelength in the nth state is 2pr>n, where r isproportional to n2. Therefore, the wavelength increases withincreasing n, and is greater for n = 2 than for n = 1.II. The de Broglie wavelength of an electron in the nth state issuch that n wavelengths fit around the circumference of theorbit. Therefore, l = 2pr>n and the wavelength for n = 2 isless than for n = 1.III. The de Broglie wavelength depends on the mass of the electron, and that is the same regardless of which state of the hydrogen atom the electron occupies

b) Choose the best explanation from among the following:I. The de Broglie wavelength in the nth state is 2pr>n, where r isproportional to n2. Therefore, the wavelength increases withincreasing n, and is greater for n = 2 than for n = 1.II. The de Broglie wavelength of an electron in the nth state issuch that n wavelengths fit around the circumference of theorbit. Therefore, l = 2pr>n and the wavelength for n = 2 isless than for n = 1.III. The de Broglie wavelength depends on the mass of the electron, and that is the same regardless of which state of the hydrogen atom the electron occupies

Physics for Scientists and Engineers with Modern Physics

10th Edition

ISBN:9781337553292

Author:Raymond A. Serway, John W. Jewett

Publisher:Raymond A. Serway, John W. Jewett

Chapter39: Introduction To Quantum Physics

Section: Chapter Questions

Problem 26P

See similar textbooks

Similar questions

a. Conceptually, discuss the particle-wave duality of light. Discuss the implications of this in combination with the de Broglie (pronounced “de Broy”) equation. b. The electron of a hydrogen atom is usually no further than 1.0 Å from the proton. We can therefore say the upper limit of the radius of an isolated hydrogen atom is roughly 1.0 Å. How does the de Broglie wavelength of the electron compare to this radius? (The velocity of an electron in the first principal energy level is about 2.2 x 106 m/s). Explain why wave-particle duality is so important for quantum mechanics, yet not required in macroscopic systems that are well described by classical mechanics. c. Comment as to whether neutrons with velocity 4.14 x 103 m/s may be used to determine structures of molecules in a diffraction-based experiment. You may consider the relevant distance between atoms in molecules to be on the order of 1 Å.
la) The maximum value of the Planck spectrum for 91 photons at 6 Kelvin is (k=Boltzmann constant) Select one: O a. 182.00 Ob. 16.92k Oc. 546.00 O d. zero Oe. 91.00 b) A box contains 3 identical fermions. What is the partition function if each particle can occupy any of 10 single- particle states? Assume that the energy for each of these states is zero. Select one: O a. 1 Ob. 495.00 Oc. 100 Od. zero Oe. infinity
a) How many ways are there to arrange 3 quanta among 4 atoms in a solid? b) . the ground state energy. What is the Boltzmann factor for this excited state? >At room temperature, the fourth excited state of a microscopic oscillator is o.6 eV above
A hydrogen atom has a radius of 0.05 nm with a position accuracy of 1.0%. Calculate the uncertainty in the atom’s velocity. Use "E" format for scientific notation (i.e. for 1.23 x 10, write as 1.23E–9). Do not Include the units in your answer.
1. We can generalize the Heisenberg Uncertainty principle for position and momentum to in- clude circular motion. If As is the uncertainty in arc length and Ap, is the uncertainty in momentum tangent to the circle, then the circular uncertainty principle is ApsAs > ħ/2. (a) Show that the circular uncertainty principle can be written as ALAO > ħ/2, where AL is the uncertainty in angular momentum and A is the uncertainty in angle. (b) How well can the angular position of the electron be specified in the Bohr atom?
A hydrogen atom has a radius of 0.05 nm with a position accuracy of 1.0%. Calculate the uncertainty in the atom’s velocity. Use "E" format for scientific notation (i.e. for 1.23x10, write as 1.23E-9).
What is the radius in nm of the electron orbit of a hydrogen atom for n = 3? What is the radius in nm of the electron orbit of a hydrogen atom for n = 2? %3D What is the energy in ev of the electron of a hydrogen atom for the orbit designated n = 1?
A)Calculate the frequency when an electron drops from n=5 to the n=4 level in a hydrogen atom. Round your answer to 4 significant digits. B)An electron in the hydrogen atom makes a transition from an energy state of principal quantum number ni to the n=2 state. If the photon emitted has a wavelength of 434nm , what is the value of ni? Round your answer to the nearest whole number.)
a) Calculate the energy of the emissive transition with the lowest energy possible for the Lyman series, for a mole of hydrogen atoms. Express your answer in joules/mol. b) Is this transition in the visible spectral domain? If not, in which region is it located?
·Shown here is the visible part of the spectrum of some gas. There are 11 lines. There could be 6. more, they just aren't in the wavelength range of the spectrum. The wavelength increases toward the right. :.. de f gh k (a) Which line or lines correspond(s) to the two closest spaced energy levels? Explain. (b) Which line or lines correspond(s) to the two farthest spaced energy levels? Explain. (c) What is the minimum number of energy levels in an atom of the gas that could produce the lines in this spectrum? Explain.
1 r e 3 do An electron in a hydrogen atom in the n = 2, I = 1 state has R21 = r/2ao 2 6a0 a) Find the most probable distance of the electron from the nucleus. b) Compute the expectation value and compare it with the value obtained in part a.
If you look at it, there is an Ag atom with an atomic number of 47. Then, there are electrons from outside hitting electrons in the base shell (n=1) : a. how much energy does the electron need to bounce off? and is there any energy absorbed by the electrons? b. How much the radiation energy and wavelength produced by the transition of electrons from the L shell (n=2) to the ground shell (n=1) in filling the electron holes?