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HYBRIDIZATION
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HYBRIDIZATION
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| The phenomenon of mixing up of different orbitals of same energy level of an atom to produce equal number of hybrid-orbitals of same energy and identical properties is known as hybridization. A hybrid orbital contains maximum two electrons with opposite spin. | ||||
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In hybridization, only those orbital take part that have very little difference of energy. Hybridization takes place in the orbitals of a single atom. Two different atoms cannot produce hybrid orbitals by overlapping their orbitals. |
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TYPES
OF HYBRIDIZATION IN CARBON ATOM
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There are three categories of hybridization : Sp3-hybridization. Sp2- hybridization. Sp- hybridization. |
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Sp3-
HYBRIDIZATION
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| The process of hybridization in which one s-orbital and three p-orbitals overlap to produce four hybrid-orbital is known as Sp3-hybridization. | ||||
| These hybrid-orbital are identical in shape and energy. These orbital are known as Sp3-hybrid orbitals. Sp3-orbitals are at an angle of 109.5o from each other. Sp3-orbital are arranged in tetrahedral fashion. | ||||
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Sp3-
HYBRIDIZATION
AND METHANE |
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Methane molecule composed of one carbon atom and four hydrogen atom i.e. CH4. In methane molecule central atom is carbon. Here carbon atom is Sp3-hybridized. One s-orbital (2s) and three p-orbital (2px, 2py, 2pz) overlap to produce four Sp3-hybrid orbitals. These Sp3- hybrid orbital are at a angle of 109.5o from each other. These Sp3-orbitals are attached at the corner of a tetrahedron. Each Sp3-orbital of carbon atom overlaps 1s-orbital of hydrogen atom. In this way four sigma bonds (Sp3-S bonds) are generated. The final geometry of methane molecule is tetrahedral as shown. |
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