Uncertainty principle, electrons and the nucleus.

I have a question I'm not entirely sure how to answer, if I work out the uncertainty of an electron's momentum confined in a space of one femtometer using the uncertainty principle, why does this result tell me that an electron cannot be bound inside a nucleus? I don't really understand why. Any help/tips appreciated.

Well work out the uncertainty of the electron's momentum...

Well yeah I know to do that bit, I got $1.055*10^{-19} kgm/s$..how does that show it won't be within the nucleus?

You know that for a particle to be confined in a potential, the wavefunction must be a standing wave, and you need to be able to fit an integer number of half wavelengths within the distance over which is it confined. You can work out the electron's wavelength from the momentum, and then compare it to a typical nuclear radius.

Work out what speed it would have to be moving at. (Ignore SR)

Non-relativistically that would be $1.158*10^{11}$ which is clearly wrong, I do not have the formulas for relativistic speeds.

Basically, ignoring SR, it would have to be travelling about 10^3 times the speed of light. The point is it would be travelling too fast to be bound. What level is this by the way?

Oh right. That's what has confused me. I wasn't sure how a femtometer linked to the size of a nucleus - after all, isn't one fm close to the value of a proton's radius? How big is a nucleus?

This is first year university stuff, I've just left my notes at my home for relativity.

A nucleus is of the order of 10^-15 m (a femtometre) if I remember correctly, and it would make sense.