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five atomic orbitals must be mixed into one ; one s orbital; three p orbital; one d orbital, forming sp3d orbital
sp3d2
2
Three hybrid orbitals in a plane at 120 0 to each other. One perpendicular to the plane, a p orbital.
sp hybridized orbial
s orbitals are spherical, so there cannot be any angle 'between' an s orbital and a p orbital. However, each lobe of a p orbital is perpendicular (90 degrees in all directions) to the surface of an s orbital.
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there r 2 electrons in the s orbital, their r 6 electrons in p orbital , their r 10 electron's in the d orbital and 14 electrons in f orbital.
hybrid orbital
Hybridization in brief can be said as inter mixing of orbitals. But you may have questions such as why? where ? when it happens and what exactly it is? Its very simple for example as in your question consider methane. The carbon atom has 2 electrons in 1s orbital and; 2 electrons in 2s orbital and; 1 electron in 2px orbital and; 1 electron in 2py orbital.In methane before carbon atom undergo bonding with hydrogen it undergoes hybridization ,that is 2s orbitals and 2p orbitals combines or hybridizes and for methane it is sp3 hybridization that means an s orbital had combined with 3 of the 2p orbitals (2px,2py,2pz). It has an tetrahedral arrangement (like four corners of a triangular pyramid) of four lobes of angles approx 109.5 degrees(The angle between H-C-H). After hybridization you cannot differentiate s orbital and p orbital.And in that sp3 hybrid each lobe has one electron and all the lobes bond with hydrogen atoms containing single electron.Note that all the lobes must be treated as an orbital such that they can maximum hold only of two electrons.Thus methane is formed as an result of head on collision of sp3 hybrids and hydrogen atoms.
five atomic orbitals must be mixed into one ; one s orbital; three p orbital; one d orbital, forming sp3d orbital
Sp3
sp3d2
it is sp3d orbital with about 20% s character
This is the basis of Organic Chemistry. An sp3 hybrid orbital can overlap with another and the result is a COVALENT bond
Oxygen atoms in water form sp3 hybridized orbitals. This configuration of bond angles and bond lengths between the electron pairs and hydrogen atoms on oxygen allow for the least strain.
Hybridization of atomic orbitals is the intermixing of atomic orbitals having a approximate energy to form equal number of hybrid orbitals having the same shape, size and energy but pointing in different directions. The new orbitals which are formed are "hybrids" of the originals and have properties that are somewhere in between. For example, a common hybridization is sp3 where three p orbitals combine with an s orbital to form four new orbitals. Other combinations (such as sp and sp2) are also possible.