Question

For each of the questions, four choices have been provided. Select the correct alternative. "The simultaneous location of both the position and the velocity of an electron in motion cannot be found with desired accuracy." This was proposed by (a) Bohr (b) Heisenberg (c) Sommerfeld (d) de Broglie

Short answer

Answer: Heisenberg

Step-by-step solution

Identifying the statement

The statement is: "The simultaneous location of both the position and the velocity of an electron in motion cannot be found with desired accuracy." This statement is associated with the uncertainty principle, a key concept in quantum mechanics.

Matching the statement with the correct scientist

The uncertainty principle was formulated by Werner Heisenberg, one of the pioneers of quantum mechanics. Therefore, the correct choice is: (b) Heisenberg

Key concepts

Quantum Mechanics

Quantum mechanics is a fundamental theory in physics that provides a description of the physical properties of nature at the scale of atoms and subatomic particles. Unlike classical physics, which can predict the exact position and momentum of a particle, quantum mechanics deals with probabilities.

It's in the realm of the very small that particles like electrons display behavior that doesn't conform to classical laws. For example, it's not possible to measure the exact position and velocity of a particle at the same time—as you'll see in the Heisenberg Uncertainty Principle. Quantum mechanics embraces this uncertainty and provides mathematical frameworks, like wave functions, to describe particle behavior that seems strange to our everyday experiences.

Heisenberg

Werner Heisenberg was a German theoretical physicist and one of the key pioneers of quantum mechanics. He's most famous for his Uncertainty Principle, which fundamentally challenges the classical notions of measurement and observation.

Heisenberg proposed that there's a limit to how precisely certain pairs of physical properties (like position and momentum) can be known about a particle. This isn't due to experimental errors, but rather a reflection of intrinsic properties of nature. The principle has profound implications, not just for the philosophy of science, but also for the practical development of quantum technologies like those found in quantum computing and cryptography.

Electron Behavior

Electrons, as quantum particles, behave very differently than objects we observe in our daily lives. They display both particle-like and wave-like characteristics—a phenomenon known as wave-particle duality.

When electrons are not being observed, they can be described by a wave function which predicts a probability distribution of where the electron might be located at any given time. It's only when a measurement takes place that the wave function 'collapses' and the electron appears to have specific properties, such as a definite position. This behavior challenges our classical intuition and drives much of the research and discussion in quantum physics.

Position and Velocity of an Electron

According to classical physics, you could measure both the position and velocity of an electron to any degree of accuracy. However, in the quantum world, this is fundamentally impossible due to the Heisenberg Uncertainty Principle.

The principle states that the more precisely the position of some particle is determined, the less precisely its momentum can be known, and vice versa. Mathematically, it's expressed as \( \triangle x \triangle p \textgreater \frac{\text{h}}{4\text{\textpi}} \), where \( \triangle x \) represents the uncertainty in position, \( \triangle p \) represents the uncertainty in momentum, and h is Planck's constant. This intrinsic uncertainty has to be accounted for in all experiments and calculations involving an electron's position and velocity.