What facts are being used in this atomic structure question?

I wish to understand how to solve this atomic structure question:



> 
> For the ground state, the electron in the H-atom has an angular
>  momentum = $\hslash$ , according to the simple Bohr model. Angular
>  momentum is a vector and hence there will be infinitely many
>  orbits with the vector pointing in all possible directions. In
>  actuality, this is not true, because:
> 
> 
> 


1. Bohr model gives incorrect values of angular
momentum.
2. only one of these would have a minimum energy.
3. angular momentum must be in the direction of spin of electron.
4. electrons go around only in horizontal orbits.


Actually, we have been taught Bohr orbits a lot in class, with formulae for everything (atomic radius/electron orbital speed/various energy levels/etc.) and also basics of the quantum mechanical model. However, we didn't go into such a great depth of Bohr orbits as asked in the above question. 


Specifically, I don't know of any reasonable arguments against points 1,2,3. Point 4 is evidently wrong based on the quantum mech model.



> 
> How do I develop any claim for/against the points 1,2,3? What are the facts involved here?
> 
> 
> 




The only correct answer is #1. 


In actuality, the ground state of the hydrogen atom has zero angular momentum. 


Regarding #2 and #4, there is no preferred plane in which one point should orbit another point. By symmetry, they are all equivalent. 


Regarding #3, there is no angular momentum in the ground state, and in a state whether there is angular momentum, it doesn't need to be in the same direction as the electron spin angular momentum. 


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