Question

The modern model of the atom describes electrons in a little less specific detail than earlier models did. Why is it that being less sure about the placement of electrons in an atom is actually an improvement over earlier models?

Electrons do not follow specific paths, so describing the area where an electron is likely to be is more scientifically accurate.
Electrons were thought to be negatively charged, but now scientists know that their charge depends on their energy level.
The modern model is based on mathematical equations, so the results become less clear when the decimals are rounded.
The position of electrons in atomic models has changed so much that it is better to have a less specific model than to be wrong again.

Answer 1

"Electrons do not follow specific paths, so describing the area where an electron is likely to be is more scientifically accurate."

Explanation: Quantum mechanics shows electrons behave like waves as well as particles. You cannot simultaneously know an electron's exact position and momentum (Heisenberg uncertainty principle), and the electron's state is described by a wavefunction that gives probabilities (orbitals), not fixed orbits. This probabilistic model matches experimental results (spectra, chemical behavior) far better than earlier definite-path models.