Which of the following does not result from applying the ...

[luvbio]

Which of the following does not result from applying the Schrdinger equation to the electron in the hydrogen atom?
  a. Finding the Bohr radius.
  b. Deriving the correct energy level dependence.
  c. Finding the probability distribution functions for the electron in the hydrogen atom
  d. Defining the rules restricting the quantum numbers n, l, and m_l
  e. Finding the value of the intrinsic spin quantum number of the electron

Question 2

Why is the Schrdinger equation so much simpler to solve for electrons in atoms like H and He⁺ than for Na or even B⁺?
 

 

a.The strong force and Coulomb forces are nearly in balance for the smaller atoms.
  b.The electrons in larger atoms affect each other by Coulomb repulsion.

 

c. Nuclear charge is distributed in significantly larger volume in larger atoms and therefore the Coulomb force is diminished on the electrons.
  d.Gravity affects each electron of larger atoms more, making the approximation of only Coulomb potential grossly inaccurate.
  e. More principal quantum numbers are allowed for all electrons in the larger atoms.

 

[sarah_brady415]

Answer to Question 1

e.
This statement is not true. Goudsmit and Uhlenbeck proposed that the electron have an intrinsic spin quantum number of s = 1/2. Schrdinger's equation fully solved did not include this quantum number.

Answer to Question 2

The Coulomb potential field that is approximated as the only one affecting the electron in the cases with one electron around the nucleus gets far more complicated with the addition of even one more electron. The Schrdinger equation becomes very difficult to process.

[luvbio]

Thanks for the timely response, appreciate it

[tranoy]

Wow, this really help