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

Quizplus · Accepted Answer

The uncertainty principle, particularly as it applies to electrons in atoms, suggests that we cannot precisely determine both the position and momentum of an electron simultaneously. This principle leads to the concept of electrons being "smeared out" or existing in a probability cloud around the nucleus, rather than having a definite path or precise location, which aligns with the wave-particle duality of electrons.

Which of the Following Best Describes the Meaning of the Uncertainty