Final answer:
The position of an electron in an electron cloud cannot precisely be determined, according to the Heisenberg Uncertainty Principle, developed by Werner Heisenberg. This contrasts with the Bohr model's fixed orbits, being replaced by the probabilistic nature of quantum mechanics and the Schrödinger equation.
Step-by-step explanation:
The concept that Werner Heisenberg developed, which states that the position of an electron in an electron cloud cannot be precisely determined, is known as the Heisenberg Uncertainty Principle. This principle is a fundamental part of quantum mechanics and indicates that it is not possible to know both the position and momentum of an electron with absolute certainty at the same time. The more accurately we try to measure one of these quantities, the less accurately we can know the other.
The Bohr model of the atom was an early model that depicted electrons in fixed orbits. It was later replaced by quantum mechanics, which uses complex mathematical methods like the Schrödinger equation to describe the behavior of electrons. The Schrödinger equation, created by Erwin Schrödinger, provides the basis for understanding the probable locations of electrons in atoms, referred to as orbitals. These orbitals are not fixed paths but areas where there is a higher probability to find an electron.
Therefore, when it comes to determining the principle discussed by Heisenberg, the correct answer is D) Heisenberg Uncertainty Principle.