Hybridisation Research Articles
In chemistry, orbital hybridisation is that the concept of blending atomic orbitals into new hybrid orbitals (with different energies, shapes, etc., than the component atomic orbitals) suitable for the pairing of electrons to make chemical bonds in valence bond theory. Chemist Pauling first developed the hybridisation theory in 1931 to elucidate the structure of straightforward
molecules like methane (CH4) using atomic orbitals. Pauling acknowledged that an atom forms four bonds by using one s and three p orbitals, in order that "it could be inferred" that an atom would form three bonds at right angles (using p orbitals) and a fourth weaker bond using the s orbital in some arbitrary direction. actually, methane has four bonds of equivalent strength separated by the tetrahedral bond angle of 109.5°. Pauling explained this by supposing that within the presence of 4 hydrogen atoms, the s and p orbitals form four equivalent combinations or hybrid orbitals, each denoted by sp3 to point its composition, which are directed along the four C-H bonds. This idea was developed for such simple chemical systems, but the approach was later applied more widely, and today it's considered an efficient heuristic for rationalizing the structures of organic compounds. It gives an easy orbital picture like Lewis structures.
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