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Wave-particle duality is a fundamental concept in quantum mechanics that describes how every particle or quantum entity exhibits both wave and particle properties. This duality is exemplified by experiments such as the double-slit experiment, where particles like electrons create interference patterns, a characteristic of waves, yet also behave as discrete particles when observed.
The Heisenberg uncertainty principle is a fundamental theory in quantum mechanics stating that it is impossible to simultaneously know both the position and momentum of a particle with absolute precision. This principle highlights the intrinsic limitations of measuring quantum systems, suggesting that the act of measurement affects the system being observed.
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The Schrödinger Equation is a fundamental equation in quantum mechanics that describes how the quantum state of a physical system changes over time. It is essential for understanding wave functions and predicting the behavior of particles at the quantum level, providing a mathematical framework for phenomena such as superposition and entanglement.
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The Electron Cloud Model is a quantum mechanical model of the atom where electrons are described as occupying a cloud-like region around the nucleus, rather than fixed orbits. This model reflects the probabilistic nature of electron positions and energy levels, providing a more accurate depiction of atomic structure than previous models.
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Quantum numbers are a set of numerical values that describe the unique quantum state of an electron in an atom, providing insights into its energy, angular momentum, and magnetic moment. They play a crucial role in understanding the arrangement of electrons in atoms and the resulting chemical properties of elements.
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Probability density refers to the function that describes the likelihood of a random variable taking on a particular value in a continuous probability distribution. It is crucial for determining the probability of the variable falling within a specific range, which is calculated by integrating the density function over that range.
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Atomic orbitals are regions in an atom where there is a high probability of finding electrons, and they are defined by quantum numbers that describe their size, shape, and orientation. These orbitals form the basis for understanding chemical bonding and the electronic structure of atoms.
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The Pauli Exclusion Principle, formulated by Wolfgang Pauli in 1925, states that no two fermions can occupy the same quantum state simultaneously within a quantum system. This principle is fundamental in explaining the structure of atoms and the behavior of electrons in atoms, leading to the diverse properties of matter.
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Quantum entanglement is a phenomenon where particles become interconnected in such a way that the state of one particle instantaneously influences the state of another, regardless of the distance between them. This non-local interaction challenges classical intuitions about separability and locality, and is a cornerstone of quantum mechanics with implications for quantum computing and cryptography.
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Superposition is a fundamental principle of quantum mechanics where a quantum system can exist in multiple states simultaneously until it is measured. This principle leads to the probabilistic nature of quantum mechanics, where the act of measurement collapses the system into one of the possible states.
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The atomic model is a scientific representation of the structure of an atom, evolving over time from early philosophical ideas to sophisticated quantum mechanical models. It plays a crucial role in understanding chemical reactions, bonding, and the fundamental nature of matter.
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