What is sp2 hybridisation?

Answer 1

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.

Answer 2

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.

Answer 3

Sp2 hybridization is a type of atomic bonding in which one s and two p orbitals of an atom combine to form three equivalent hybrid orbitals. These hybrid orbitals have 33% s character and 67% p character, and are responsible for the formation of trigonal planar molecular geometries in organic compounds. This type of hybridization is commonly seen in molecules with double bonds, such as alkenes.

Answer 4

atom that has four bonds forming a tetrahedral shape, mixture of an s and 3 p orbitals

Answer 5

yes, look up MnF7 on Google.