Q. explain sp3 hybridization in formation of ethane ( c2h6 ) molecule.
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Answer:
The 1 s orbital, as well as the px, py, and pz orbitals, undergo sp3 hybridization during the creation of C2H6.
Explanation:
- For each carbon atom, this results in the production of four hybridized orbitals. The electrons in the molecular hybrid orbitals now form distinct bonds.
- One hybrid orbital of one carbon atom will overlap with one s-orbital of the hydrogen atom to generate three sigma bonds among the four sp3 hybrid orbitals.
- Furthermore, the last orbital will overlap with one of another carbon atom's sp3 orbitals, establishing a sigma bond between two C-atoms.
- In C2H6, hybridization involves one s orbital and three p-orbitals (px, py, pz).
- A cluster of four sp3 hybridized orbitals has formed.
- When ethane is hybridized, four identical bonds form in a flawless tetrahedral shape.
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Answer:
Orbital hybridization is the concept of mixing atomic orbital into new hybrid with different energies , shape etc then the component atomic orbital suitable for the pairing of electron to form chemical bond in valence bond theory.
For example, in ethane molecules , the bonding structure according to valance orbital theory is very similar to that of methane . Both are sp³- hybridized , meaning that both have four bonds arranged with tetrahedral geometry.
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