Final answer:
The Heisenberg Uncertainty Principle states that both the position and momentum of an electron cannot be known precisely. According to Werner Heisenberg, accurately measuring one of these properties leads to increased uncertainty in measuring the other. This principle is a fundamental concept in quantum mechanics.
Step-by-step explanation:
The Heisenberg Uncertainty Principle states that it is impossible to know precisely both the position and the momentum of an electron. According to Werner Heisenberg, the more accurately we measure the momentum of a particle, the less accurately we can determine its position at that time, and vice versa. This principle is a fundamental concept in quantum mechanics that highlights the limits of our ability to measure certain properties of microscopic particles.