de Broglie wavelength is the wavelength associated with any moving particle. It's given by λ = h/p, where h is Planck's constant (6.63 × 10⁻³⁴ J·s) and p is momentum (mass × velocity). It shows that particles like electrons have wave properties.
In 1924, Louis de Broglie had a bold idea: if light (which we thought was a wave) can behave like particles (photons), then electrons (which we thought were particles) might behave like waves. Every moving particle has an associated wavelength, given by λ = h/p, where h is Planck's constant and p is momentum. This wave-particle duality is why electrons create diffraction patterns and why orbitals exist.
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Your baseball has a de Broglie wavelength, but it's incredibly tiny — about 10⁻³⁴ m. This is far too small to detect. For electrons, the wavelength is about 10⁻¹⁰ m, which is comparable to atomic sizes, so wave behavior becomes visible through diffraction and interference patterns.
Both concepts point to the same truth: electrons are not just particles. Their wave nature (de Broglie) and the impossibility of knowing both position and momentum (Heisenberg) are two sides of the same coin. Wave-particle duality is fundamental.
Yes. You need mass (m) and velocity (v). Calculate momentum p = m × v. Then λ = h/p. For electrons: m = 9.109 × 10⁻³¹ kg. For a ball: m = 0.1 kg. The smaller the mass, the larger the wavelength at the same velocity.
Bohr assumed electrons move in definite circular orbits (particle view). But if electrons are waves, they can't have definite orbits — waves are spread out. The quantum mechanical model treats electrons as matter waves, described by the Schrödinger equation, giving us orbitals (probability distributions) instead of orbits (definite paths).
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