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In quantum mechanics, an atomic orbital (/ ˈɔːrbɪtəl /) 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 the nucleus.
Checked. In chemistry, orbital hybridisation (or hybridization) is the concept of mixing atomic orbitals to form new hybrid orbitals (with different energies, shapes, etc., than the component atomic orbitals) suitable for the pairing of electrons to form chemical bonds in valence bond theory. For example, in a carbon atom which forms four ...
Bent's rule. Shape of water molecule showing that the real bond angle 104.5° deviates from the ideal sp 3 angle of 109.5°. In chemistry, Bent's rule describes and explains the relationship between the orbital hybridization and the electronegativities of substituents. [1][2] The rule was stated by Henry A. Bent as follows: [2] Atomic s ...
Molecular orbital diagram of HF. Hydrogen fluoride is another example of a heteronuclear molecule. It is slightly different in that the π orbital is non-bonding, as well as the 2s σ. From the hydrogen, its valence 1s electron interacts with the 2p electrons of fluorine. This molecule is diamagnetic and has a bond order of one.
Electron configuration. In atomic physics and quantum chemistry, the electron configuration is the distribution of electrons of an atom or molecule (or other physical structure) in atomic or molecular orbitals. [1] For example, the electron configuration of the neon atom is 1s2 2s2 2p6, meaning that the 1s, 2s, and 2p subshells are occupied by ...
This notation is used to specify electron configurations and to create the term symbol for the electron states in a multi-electron atom. When writing a term symbol, the above scheme for a single electron's orbital quantum number is applied to the total orbital angular momentum associated to an electron state.
The type of bonding can be explained in terms of orbital hybridisation. In ethylene each carbon atom has three sp 2 orbitals and one p-orbital. The three sp 2 orbitals lie in a plane with ~120° angles. The p-orbital is perpendicular to this plane. When the carbon atoms approach each other, two of the sp 2 orbitals overlap to form a sigma bond.
An isolated p-or sp x-orbital (unfilled or filled, symbol ω) A conjugated π system (symbol π) A σ bond (symbol σ) The electron count of a component is the number of electrons in the orbital(s) of the component: The electron count of an unfilled ω orbital (i.e., an empty p orbital) is 0, while that of a filled ω orbital (i.e., a lone pair ...