From the modern day Quantum theory of the atom, which theory postulates that the mass of the electron and its exact position cannot be deduced simultaneously and that we must be satisfied with the probability of finding the electron?

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The Heisenberg uncertainty principle postulates that the more precisely we know the position of an electron, the less precisely we can know its momentum, and vice versa. This is due to the wave-particle duality of matter, where electrons can behave as both particles and waves. Therefore, we must be satisfied with the probability of finding the electron in a specific location within the atom.

From the Modern Day Quantum Theory of the Atom, Which