Quantum chemistry mathematically describes the fundamental behavior of matter at the molecular level. In principle, it is possible to describe all chemical systems using this theory. In practice, only the simplest chemical systems may realistically be investigated in purely quantum mechanical terms, and approximations must be made for most practical purposes (eg, Hartree-Fock, post-Hartree-Fock or density functional theory, see computational chemistry for more details) . Therefore, understanding of quantum mechanics is not necessary for most chemistry, as the important implications of the theory (principally the orbital approximation) can be understood and applied in simpler terms.
In quantum mechanics (several applications in computational chemistry and quantum chemistry), Hamiltonian, or physical, of a particle can be expressed as the sum of two operators, one associated with the kinetic energy and the potential energy. Hamiltonian in the Schrödinger wave equation used in quantum chemistry has no terminology for electrons round.
Completion of the Schrödinger equation for the hydrogen atom gives the shape of the wave function for the atomic orbitals, and the relative energies of the 1s, 2s, 2p and 3p. Orbital approximation can be used to understand other atoms such as helium, lithium, and carbon.
In quantum mechanics (several applications in computational chemistry and quantum chemistry), Hamiltonian, or physical, of a particle can be expressed as the sum of two operators, one associated with the kinetic energy and the potential energy. Hamiltonian in the Schrödinger wave equation used in quantum chemistry has no terminology for electrons round.
Completion of the Schrödinger equation for the hydrogen atom gives the shape of the wave function for the atomic orbitals, and the relative energies of the 1s, 2s, 2p and 3p. Orbital approximation can be used to understand other atoms such as helium, lithium, and carbon.
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