Final answer:
The statement that electrons exhibit wave-particle duality is correct and is a fundamental aspect of quantum mechanics. Electron diffraction experiments like the Davisson-Germer experiment support the concept that electrons demonstrate both wave-like and particle-like properties. Quantum mechanics describes the probability distribution of electrons using wave functions, reflecting their wavelike nature.
Step-by-step explanation:
The statement "Electrons exhibit wave-particle duality" is indeed correct and is a central concept in quantum mechanics. The phenomenon of wave-particle duality suggests that particles such as electrons display both wave-like and particle-like properties, depending on the experimental conditions. This concept was first proposed by Louis de Broglie, which led to the discovery that the wavelength of a particle is related to its momentum. Furthermore, electron diffraction experiments, such as the Davisson-Germer experiment, demonstrate this duality by showing patterns that could only be explained if the electrons have a wave nature.
When electrons travel through a crystalline structure and form a diffraction pattern, they are exhibiting their wave properties. The capacity of electrons to interfere with each other is evidence of their wave nature and forms the basis for the modern quantum mechanical description of electrons in atoms, involving three-dimensional wave functions, or orbitals. The quantum mechanical model of the atom is based on the probability distribution of electrons, which denotes the likelihood of finding an electron in a certain region of space, further emphasizing the significance of their wave characteristics.
To integrate this understanding in real-world applications, scientists can calculate the separation of planes in a crystal by analyzing the interference patterns produced by electrons, which directly links to the concepts of wave-particle duality and quantum mechanics.