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In quantum mechanics, an atomic orbital (/ ˈ ɔːr b ɪ t ə l / ⓘ) is a function describing the location and wave-like behavior of an electron in an atom. [1] This function describes an electron's charge distribution around the atom's nucleus, and can be used to calculate the probability of finding an electron in a specific region around ...
Orbital radius = 1 a.u. of length; Orbital velocity = 1 a.u. of velocity [44]: 597 Orbital period = 2π a.u. of time; Orbital angular velocity = 1 radian per a.u. of time; Orbital momentum = 1 a.u. of momentum; Ionization energy = 1 / 2 a.u. of energy; Electric field (due to nucleus) = 1 a.u. of electric field; Lorentz force (due to ...
Early results about relative orbital motion were published by George William Hill in 1878. [3] Hill's paper discussed the orbital motion of the moon relative to the Earth.. In 1960, W. H. Clohessy and R. S. Wiltshire published the Clohessy–Wiltshire equations to describe relative orbital motion of a general satellite for the purpose of designing control systems to achieve orbital rendezvous.
The orbital period (also revolution period) is the amount of time a given astronomical object takes to complete one orbit around another object. In astronomy , it usually applies to planets or asteroids orbiting the Sun , moons orbiting planets, exoplanets orbiting other stars , or binary stars .
The orbital wave functions are positive in the red regions and negative in the blue. The right column shows virtual MO's which are empty in the ground state, but may be occupied in excited states. In chemistry, a molecular orbital (/ ɒr b ə d l /) is a mathematical function describing the location and wave-like behavior of an electron in a ...
Orbital elements are the parameters required to uniquely identify a specific orbit. In celestial mechanics these elements are considered in two-body systems using a Kepler orbit . There are many different ways to mathematically describe the same orbit, but certain schemes are commonly used in astronomy and orbital mechanics .
The energy difference between the HOMO and LUMO is the HOMO–LUMO gap. Its size can be used to predict the strength and stability of transition metal complexes, as well as the colors they produce in solution. [1] As a rule of thumb, the smaller a compound's HOMO–LUMO gap, the less stable the compound. [2]
The localized orbital corresponding to one O-H bond is the sum of these two delocalized orbitals, and the localized orbital for the other O-H bond is their difference; as per Valence bond theory. For multiple bonds and lone pairs, different localization procedures give different orbitals .