Q15) The energy in (eV) of n=3 state of He atom is: A)-1.510 eV B) -1.812 eV C)-6.040 eV D) -6.795 eV Q16) If there are n wave functions corresponding to a certain energy E.. Which of the following is correct? A) The wave functions are orthogonal B) The state is n-fold degenerate C) The eigenvalues (E) are all the same of the Hamiltonian operator D) All of the above are correct

Q15) The energy in (eV) of n=3 state of He atom is: A)-1.510 eV B) -1.812 eV C)-6.040 eV D) -6.795 eV Q16) If there are n wave functions corresponding to a certain energy E.. Which of the following is correct? A) The wave functions are orthogonal B) The state is n-fold degenerate C) The eigenvalues (E) are all the same of the Hamiltonian operator D) All of the above are correct

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter12: Atoms And Molecules

Section: Chapter Questions

Problem 12.16E: Spin orbitals are products of spatial and spin wavefunctions, but correct antisymmetric forms of...

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Similar questions

Suppose that the spin quantum number had three allowed values (ms=0,+12,12) . Give the atomic numbers of the first three noble-gas atoms in this case.
What are the degeneracies of the H atom wavefunctions when spin is accounted for? Give a general formula.
Is the spin orbital 1s for the H atom still spherically symmetric? Explain your answer.
Spin orbitals are products of spatial and spin wavefunctions, but correct antisymmetric forms of wavefunctions for multielectron atoms are sums and differences of spatial wavefunctions. Explain why acceptable antisymmetric wavefunctions are sums and differences that is, combinations instead of products of spatial wavefunctions.
Based on the trend shown in Figure 11.5, draw the probability distribution of a harmonic oscillator wavefunction that has a very high value of n. Explain how this is consistent with the correspondence principle.
Why does the wavefunction 4,4,0 not exist? Similarly, why does a 3f subshell not exist? See exercise 11.73 for notation definition.
For the Li atom, the energy difference between the ground state and the first excited state, in which the outermost electron is in a 2p orbital, is 2.961019J . In the Li2+ ion, the energy difference between the 2s and 2p levels is less than 0.00002 of this value. Explain this observation.
Suppose an electron had three possible values of ms, designated , and . What is the Slater determinant for Li? For Be?
Explain why the wave model for radiation cannot account for the photoelectric effect.
Using Table 5.2, write down the mathematical expression for the 2px wave function for an electronically excited H atom. Estimate the probability of finding the 2px electron if you look in a cubical box of volume of 0.8(pm)3 centered at a distance of 0.5001010m in the =/2 , =0 direction. Does this probability change as you change ? At what angles is the probability of finding the electron smallest and at what angles is the probability the largest? (Note that =2 is the same location as =0 , so don’t double count.)
The helium ion He+ is a one-electron system whose wave functions and energy levels are obtained from those for H by changing the atomic number to Z=2 . Calculate the average distance of the electron from the nucleus in the 2s orbital and in the 2p orbital. Compare your results with those in Problem 11 and explain the difference.
Explain why assuming an effective nuclear charge, as used for our treatment of the helium atom in Example 12.11, is unnecessary for a treatment of the hydrogen atom.