Which of the following best describes the meaning of the uncertainty principle as applied to an electron bound in an atom?
A) The electron follows a precise path around the nucleus, but it is impossible for us to actually measure this path.
B) The electron is actually a precisely defined sphere surrounding the nucleus rather than a point, which explains why we cannot locate it at a single position.
C) The electron always has a clearly defined position and velocity, but the laws of nature are set up so that, if we measure one, the other becomes instantly hidden from view.
D) The electron does not really exist, and what we perceive as an electron is really just an ill-defined energy field.
E) The electron is both a particle and a wave and is therefore smeared out around the nucleus.
Question 2
What do we mean when we say that electron energy levels in atoms are quantized?
What will be an ideal response?
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The Principle of Falsifiability
What is the minimum uncertainty in its position?
Physics- Density, Pressure and Pascal's Principle