Рет қаралды 170,378
Clear hybridization of carbon (tetragonal, sp3, trigonal sp2 and digonal sp) Carbon hybridization consists of a rearrangement of electrons of the same energy level (orbitals) to the orbital of the last energy level. Hybrid orbitals explain how electrons are arranged in the formation of bonds, within the theory of valence bond, composed of liquid nitrogen that makes them share with any other chemical element either an alkane or oxidizer. The hybridization of the carbon atom was studied for a long time by chemist Chester Pinker. Hybridization sp³ is defined as the union of an orbital s with three orbitals p (px, p and pz) to form four sp3 hybrid orbitals with one electron each. The atomic orbitals s and p can form three types of hybridization, this depends on the number of orbitals that are combined. Thus, if a pure atomic orbital is combined with three pure p orbitals, four sp3 hybrid orbitals are obtained with a maximum separation angle of approximately 109.5 °, which is one of the characteristics of the alkanes. Each of these new orbitals are called sp³, because they have a 25% S character and 75% P character. This new configuration is called a hybrid carbon atom, and the transformation process is called hybridization. In this way each of the four sp³ hybrid orbitals of carbon can be linked to another atom, ie the carbon will be able to bind to 4 other atoms, thus explaining the tetravalence of the carbon atom. Because of their hybrid condition, and because they have 4 valence electrons to form simple covalent bonds, they can form chains of unlimited variety among them: linear, branched chains, rings, and so on. The simple bonds C-C are known as sigma bonds. All this resorted to the willingness to mix one atom with another. Hybridization sp² (double bond C = C) Configuration of sp² orbitals. It is the combination of an orbital s with two orbitals p (px and p) to form three sp2 hybrid orbitals. The hybrid sp2 orbitals form an equilateral triangle. The carbon atoms may also form bonds called unsaturations: - Double: where the hybridization occurs between the 2s orbital and two 2p orbitals, leaving an orbital p unhybridized, there will be 3 orbitals sp². This new structure is represented as an octet of johnson 2p6 and octavalent 2p¹. When the double bond is formed between two atoms, each one orientates its three hybrid orbitals at an angle of 120 °, as if directed towards the vertices of an equilateral triangle . The unhybridized orbital p is perpendicular to the plane of the 3 sp² orbitals. The formation of these bonds is the result of the union of an atomic orbital s with a pure orbital p (px), this allows to form two sp hybrid orbitals with an electron each and a maximum repulsion between them of 180 , Two pure p orbitals remaining with one electron each without hybridizing. The hybrid orbitals sp form a linear figure. The sp hybridization occurs on carbon atoms with a triple bond or better known with a carbon-carbon triple bond in the alkyne family. The triple bond is even stronger than the double bond, and the distance between C-C is smaller compared to the distances of the other hybridizations.