Import Question JSON

$\text{Hint: The Heisenberg Uncertainty Principle discredits the aspect of the Bohr atom model.}$\n\n$\text{Explanation:}$\n\n$\text{In the Bohr model, an electron is regarded as a charged particle moving in well-defined circular orbits around the nucleus. An orbit can completely be defined only if both the position and the velocity of the electron are known exactly at the same time.}$\n\n$\text{This is not possible according to the Heisenberg uncertainty principle, which states that it is impossible to simultaneously determine the exact position and momentum of an electron. Mathematically, it is expressed as } \Delta x \cdot \Delta p \geq \frac{h}{4\pi} \text{, where } \Delta x \text{ is the uncertainty in position, } \Delta p \text{ is the uncertainty in momentum, and } h \text{ is Planck's constant.}$\n\n$\text{Furthermore, the wave character of the electron is not considered in the Bohr model. The Bohr model treats electrons as particles, while modern quantum mechanics recognizes the wave-particle duality of electrons.}$\n\n$\text{The Rutherford Model preceded Bohr's model and described the atom as having a central nucleus with electrons orbiting around it, but it did not address the stability of these orbits, which Bohr attempted to solve.}$\n\n$\text{J.J. Thomson's Model (plum pudding model) proposed that an atom consists of electrons embedded in a positive sphere, but it was disproven by Rutherford's gold foil experiment before Bohr's model was developed.}$\n\n$\text{The Photoelectric Effect actually supported aspects of quantum theory that Bohr incorporated into his model, such as the quantization of energy.}$\n\n$\text{Therefore, Heisenberg's Uncertainty Principle fundamentally contradicts the Bohr Model's assumption about precisely defined electron orbits.}$