Exploring Quantum Numbers, Bohr Model, and Electron Diffraction | Homework Help

[smity711]

Just stuck on a few problems on my homework, any help?

1. How many different sets of quantum numbers are possible for an electron for which:

a) n=1
b) n=2
c)n=3
d)n=4
e)n=5


2. For a hydrogen atom in its ground state, use the Bohr model to compute:

a) the orbital speed of the electron
b) the KE of the electron
c) the electrical potential energy of the atom


3. A monoenergetic bema of electrons is incident on a single slit of width 0.500nm. A diffraction pattern is formed on a screen 20.0cm from the slit. If the distance between successive minima of the diffraction pattern is 2.10cm, what is the energy of the incident electrons?

Thanks for any help you can give!

 

[Hootenanny]

Hi there,

For future reference we have https://www.physicsforums.com/forumdisplay.php?f=152" specifically for such questions. Also, according to the rules of the forums (which you have agreed to); you are required to show some effort in solving the problems yourself.

Perhaps if you posted your ideas we could direct you down the right path...

 

[m2003]

I am happy to provide assistance with your homework problems on quantum numbers, the Bohr model, and electron diffraction.

1. There are four quantum numbers that describe the energy state and location of an electron: n, l, ml, and ms. The possible values for each quantum number are as follows:

a) n=1: Since n=1, l can only have a value of 0, and ml can only have a value of 0. This means there is only one set of quantum numbers possible for an electron with n=1: (n=1, l=0, ml=0, ms=±1/2).

b) n=2: With n=2, l can have values of 0 or 1, and ml can have values of -1, 0, or 1. This gives a total of four possible sets of quantum numbers: (n=2, l=0, ml=0, ms=±1/2), (n=2, l=1, ml=-1, ms=±1/2), (n=2, l=1, ml=0, ms=±1/2), (n=2, l=1, ml=1, ms=±1/2).

c) n=3: Similarly, with n=3, l can have values of 0, 1, or 2, and ml can have values of -2, -1, 0, 1, or 2. This gives a total of nine possible sets of quantum numbers: (n=3, l=0, ml=0, ms=±1/2), (n=3, l=1, ml=-1, ms=±1/2), (n=3, l=1, ml=0, ms=±1/2), (n=3, l=1, ml=1, ms=±1/2), (n=3, l=2, ml=-2, ms=±1/2), (n=3, l=2, ml=-1, ms=±1/2), (n=3, l=2, ml=0, ms=±1/2), (n=3, l=2, ml=1, ms=±1/2), (n=3, l=2, ml