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Chemist Linus Pauling first developed the hybridisation theory in 1931 to explain the structure of simple molecules such as methane (CH 4) using atomic orbitals. [2] Pauling pointed out that a carbon atom forms four bonds by using one s and three p orbitals, so that "it might be inferred" that a carbon atom would form three bonds at right angles (using p orbitals) and a fourth weaker bond ...
In organic chemistry, molecules which have a trigonal pyramidal geometry are sometimes described as sp 3 hybridized. The AXE method for VSEPR theory states that the classification is AX 3 E 1. Phosphine, an example of a molecule with a trigonal pyramidal geometry.
In traditional hybridisation theory, the hybrid orbitals are all equivalent. [12] [27] Namely the atomic s and p orbital(s) are combined to give four sp i 3 = 1 ⁄ √ 4 (s + √ 3 p i) orbitals, three sp i 2 = 1 ⁄ √ 3 (s + √ 2 p i) orbitals, or two sp i = 1 ⁄ √ 2 (s + p i) orbitals. These combinations are chosen to satisfy two ...
In chemical bonds, an orbital overlap is the concentration of orbitals on adjacent atoms in the same regions of space. Orbital overlap can lead to bond formation. Linus Pauling explained the importance of orbital overlap in the molecular bond angles observed through experimentation; it is the basis for orbital hybridization.
In fact, the carbon atoms in the single bond need not be of the same hybridization. Carbon atoms can also form double bonds in compounds called alkenes or triple bonds in compounds called alkynes. A double bond is formed with an sp 2-hybridized orbital and a p-orbital that is not involved in the hybridization. A triple bond is formed with an sp ...
Additionally, the surrounding sp3 hybridized carbons can stabilize the carbocation through hyperconjugation. [5] This occurs when adjacent sp3 orbitals have a weak overlap with the vacant p orbital; since there are 3 surrounding carbons with sp3 hybridization , there are more opportunities for overlap, which contributes to increasing ...
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They have three sp 2 orbitals. There exist also sd-hybridised AX 2 compounds of transition metals without lone pairs: they have the central angle about 90° and are also classified as bent. [citation needed] (See further discussion at VSEPR theory#Complexes with strong d-contribution).