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Electrons surround nuclei due to the nature and strength of the fundamental forces and laws of physics. They are attracted to the nucleus because of their charge; since opposite charges attract, the negatively charged electrons are attracted to the positive nucleus through the electromagnetic interaction (or, electrostatically). They don't collide spontaneously with the nucleus because of several effects which result in the stability of orbits that don't intersect the location of the nucleus, most significantly the energy they possess, but also including quantum considerations such as the size of the wave function and other wave motion properties, and laws about confinement, and the uncertainties in the balance between potential and kinetic energy; one way of thinking of it is that the probability density of locating the electron in a radial direction away from the nucleus peaks at the Bohr radius -- often regarded as "the size" of the orbital -- and approaches zero as one gets closer to the nucleus.

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