The wave-particle duality of electrons can indeed lead to some conceptual challenges when it comes to understanding their behavior. While it is true that electrons exhibit wave-like properties, such as diffraction and interference, it is important to note that these wave-like properties do not imply that the electron itself is physically "spread out" like a classical wave.
The idea of an electron traveling in a circular path is typically associated with the classical model of an electron orbiting the nucleus in an atom, similar to the way planets orbit the sun. However, this classical model is an oversimplification and is not accurate at the quantum level. In quantum mechanics, electrons are described by wavefunctions, which are mathematical representations that contain information about the probability distribution of finding an electron in different locations.
When an electron is in a bound state, such as within an atom, its wavefunction can be quantized into discrete energy levels. These energy levels are represented by atomic orbitals, which have different shapes (spherical, dumbbell-shaped, etc.) and describe the probability of finding the electron in different regions around the nucleus. The motion of the electron within these orbitals is not a literal circular path but rather a probability distribution of the electron's position.
It's important to note that the wave-particle duality does not mean that an electron is simultaneously a classical wave and a classical particle. Instead, it means that in certain situations, electrons can exhibit wave-like behavior (interference, diffraction) and in other situations, they exhibit particle-like behavior (localized interactions, discrete energy levels).
In summary, the wave-particle duality of electrons does not imply that the electron itself is physically traveling in a circular path like a classical wave. Rather, it is the probability distribution of the electron's position that exhibits wave-like properties.