Physics · Quantum Mechanics

In quantum mechanics, Heisenberg's Uncertainty Principle states that it is impossible to simultaneously measure both the position (Δx) and the momentum (Δp) of a particle with absolute precision. The principle is mathematically expressed as: Δx · Δp ≥ h4π where h is Planck's constant. This implies that if the uncertainty in the position (Δx) is very small, the uncertainty in the momentum (Δp) will be large, and vice versa. The principle becomes more significant at microscopic levels, such as with electrons, and has negligible implications in macroscopic systems like airplanes. The principle suggests that the more accurately we know one property, the less accurately we can know the other. Based on the above, which of the following statements are correct? (A) Heisenberg's Uncertainty Principle rules out the exact simultaneous measurement of position and momentum. (B) If the uncertainty in the position of an electron is zero, the uncertainty in its momentum would also be zero. (C) The uncertainty principle has negligible practical implications for macroscopic objects such as airplanes. (D) The principle can be applied effectively only to particles that are visible to the naked eye.