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The de Broglie wavelength is the wavelength associated with a moving particle, calculated using the formula λ = h/p, where h is Planck's constant and p is the particle's momentum (mass times velocity). This relationship shows that wavelength depends inversely on velocity: faster particles have shorter wavelengths. The de Broglie hypothesis extends to all matter, though macroscopic objects have wavelengths too small to observe.

De Broglie proposed that electrons behave as circular standing waves orbiting the nucleus. For stable orbits, an integer number of wavelengths must fit exactly within the orbit's circumference. This standing wave condition explains why only certain orbits are allowed, providing a wave-based foundation for the quantization that Bohr postulated. Points on the wave with zero amplitude are called nodes.

Davisson and Germer demonstrated electron wave behavior by directing an electron beam at a crystalline nickel target. Initially, few electrons showed particle-like behavior with localized spots. As more electrons accumulated, a clear interference pattern emerged—the hallmark of wave-like behavior. This interference and diffraction pattern proved electrons exhibit wavelike properties similar to X-rays passing through crystals.

Macroscopic objects have extremely large masses and velocities. When applying the de Broglie relation to a golf ball, Planck's constant divided by its mass and velocity yields an incredibly small wavelength—far too small to observe or measure. Only subatomic particles with extremely small masses, like electrons, have wavelengths large enough for their wave nature to be experimentally detected.

When electrons pass through two closely spaced slits, initially only a few electrons create localized particle-like spots on a screen. However, as more electrons accumulate, an interference pattern emerges between the spots—characteristic of waves. This demonstrates that electrons simultaneously exhibit particle and wave properties, fundamentally different from classical objects that behave as either particles or waves.

The de Broglie wavelength is inversely proportional to electron velocity. As electron velocity increases, the wavelength decreases, and vice versa. This inverse relationship means faster-moving electrons have shorter wavelengths and are less likely to exhibit observable wave behavior, while slower electrons have longer wavelengths that may be more readily detected experimentally.

De Broglie's hypothesis applies the wave-particle duality concept to all matter, not just electrons. These associated waves are called matter waves. However, the de Broglie wavelength depends on mass and velocity; larger, faster objects have wavelengths too small to observe. This fundamental behavior is intrinsic to all quantum particles and represents a departure from classical mechanics governing macroscopic objects.