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.
sp2 hybridization is one example of the hybrid atomic orbital theory of covalent bonding. Generally, hybrid orbital theory tells us that individual atomic orbitals 'mix' to form new hybrid atomic orbitals. A hybrid atomic orbital can overlap with another atom's hybrid orbital or unhybridized atomic orbital to form a covalent bond.
Hybrid atomic orbital formation occurs as the separate atoms to be bonded approach each other.
One confusing aspect of orbital hybridization theory is the case of multiple bond formation, of which sp2 is one example. sp2 is a mixture of one s-atomic orbital and 2-p atomic orbitals to form three sp2 hybrid orbitals. The observant reader may have noticed that there is one unhybridized p-atomic orbital. In the case of ethene, C2H2, there is a double bond between carbon atoms: one part of the double bond is an end-to-end overlap of a sp2 hybrid orbital pair (a sigma covalent bond) and the other part is a side-to-side overlap of two unhybridized p-atomic orbitals (a pi covalent bond). The pi bond happens because the unhybridized p-atomic orbitals are oriented 90 degrees from the plane of the ("flat") ethene molecular structure.
atom that has four bonds forming a tetrahedral shape, mixture of an s and 3 p orbitals
We should know that S orbitals hold electrons more tightly to nucleus than P orbitals . This implies that S orbitals are effectively more electronegative . Now, in sp2 carbon the character of each orbital has 1/3 or 33% of s orbital characteristics whereas in each sp3 orbital s character is 1/4 or 25% . So sp2 has more s character and therfore more electronegativity. H.Sehgal
Its a polar bond, for the electrons are more pulled towards the fluorines. It is a trigonal planar molecule. Sp2 hybridization. Hope this helped.
Carbonate ion is in a trigonal planar shape (hint: sp2 hybridization)
It's going to be planar due to the sp2 hybridized carbons.
You will need to supply a structural formula for this question to be answered. Or you could simply count the number of other atoms bonded to each carbon: 4 means it's sp3, 3 is sp2, and 2 is sp.
It's a sp2 hybridisation.
its sp2 hybridisation
sp2
sp or sp2 hybridisation se
carbon can have either sp3 ,sp2 or sp1 hybridised orbital depending upon the type of hybridisation hybridisation influences the bond and bond therapy (strength) in the organic compounds
In molecular BH3 the molecule is planar with bond angles of 120o so the hybridisation of the central boron atom is sp2. In the dimer B2H6 the molecule has two bridging hydrogens. The hybridisation of each boron is approxomately sp3 and each bridge has a 3 centre B-H-B bond formed by the overlap of the sp3 orbtals on the B atoms and the s orbital on the hydrogen.
The C atom of HCHO has 3 sigma bonds and a pi bonds. Hence the hybridization of C is sp2.
sp hybridization
ANTHRANALIC ACID IS 2- AMINO BENZOIC ACID.SO CARBON ATOM OF CORBOXYIC GROUP IS SP2 hybridisd
tertiary alcohol is sp3 hybridised. when carbocation is formed hydroxyl takes its as well as carbon atoms electrons as a result one of the p orbital of carbon becomes empty thus carbon atom in order to attain stabilty undergoes hybridisation with one s orbital and remaining two p orbitals and becomes sp2 hybridised
VSEPR - valence shell electron pair repulsion theory Hybridisation- e.g. Sp, Sp2, sp3, Sp3d2 etc Hybridisation predicts regular geometries-- VSEPR has the advantage of predicting how bond angles may deviate from the regular geometries.
haloarenes are less reactive than haloalkanes because: 1. resonance effect more the resonatinsg structures,more the stability 2.difference in hybridisation of the C-X bond i.e.,in haloalkanes,the hybridisation is sp3 whereas in haloarenes it is sp2 hybridised.As sp2 is more electronegative therefore bond length is shorter and hence stronger. these are the major reasons.