1 Answer
The de Broglie hypothesis applies to all matter, not just light or electromagnetic waves. It suggests that particles like electrons, protons, and even larger objects (though practically imperceptible for large objects) have wave-like properties, just like light does.
In simple terms, de Broglie proposed that any moving particle has a wavelength associated with it, which is given by the formula:
\[
\lambda = \frac{h}{p}
\]
Where:
This was a groundbreaking idea because, before de Broglie, we thought of particles and waves as completely separate things. He showed that particles (which we usually think of as solid, localized objects) can actually behave like waves under the right conditions, especially when they're moving at high speeds or are very small (like electrons).
In practical terms, this wave-particle duality is central to quantum mechanics. It's why electrons in atoms don't just orbit in neat circular paths like planets, but instead exist in "clouds" or orbitals based on probabilities, as their wave-like nature affects their behavior.
In simple terms, de Broglie proposed that any moving particle has a wavelength associated with it, which is given by the formula:
\[
\lambda = \frac{h}{p}
\]
Where:
- \( \lambda \) is the wavelength of the particle
- \( h \) is Planck's constant (\(6.626 \times 10^{-34} \, \text{Js}\))
- \( p \) is the momentum of the particle (which is mass × velocity)
This was a groundbreaking idea because, before de Broglie, we thought of particles and waves as completely separate things. He showed that particles (which we usually think of as solid, localized objects) can actually behave like waves under the right conditions, especially when they're moving at high speeds or are very small (like electrons).
In practical terms, this wave-particle duality is central to quantum mechanics. It's why electrons in atoms don't just orbit in neat circular paths like planets, but instead exist in "clouds" or orbitals based on probabilities, as their wave-like nature affects their behavior.