What principle states that it is impossible to know both the exact position and momentum of an electron at the same time?

The principle that states it is impossible to know both the exact position and momentum of an electron simultaneously is known as the Heisenberg Uncertainty Principle. This principle arises from the fundamental concepts of quantum mechanics and illustrates a key limitation in the precision of measurements at the quantum level. According to this principle, the more accurately one property (like position) is measured, the less accurately the other property (like momentum) can be known.

This principle emphasizes the inherent probabilistic nature of quantum mechanics, indicating that particles such as electrons do not have definite paths or locations as imagined in classical physics. Instead, their behaviors and properties are described by wave functions, giving rise to probabilities of finding them in particular states.

Understanding the Heisenberg Uncertainty Principle is crucial for grasping the behaviors of subatomic particles and for comprehending the limitations imposed by quantum mechanics on the precision of measurements in physical systems. This principle helps explain various phenomena observed in quantum physics, from electron cloud distributions around atomic nuclei to the nature of quantum states.