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Sp3 Hybridisation Video Lecture | Physical Chemistry for NEET

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FAQs on Sp3 Hybridisation Video Lecture - Physical Chemistry for NEET

1. What is sp3 hybridization?
Ans. Sp3 hybridization refers to the mixing of one s orbital and three p orbitals in order to form four hybrid orbitals with equal energy. This type of hybridization occurs when an atom has four electron groups around it, resulting in a tetrahedral arrangement.
2. Which elements commonly exhibit sp3 hybridization?
Ans. Sp3 hybridization is commonly observed in elements such as carbon (C), nitrogen (N), and oxygen (O). These elements frequently form compounds with tetrahedral or trigonal pyramid geometries due to their sp3 hybridized orbitals.
3. How does sp3 hybridization affect the bond angles in a molecule?
Ans. Sp3 hybridization leads to bond angles of approximately 109.5 degrees in a molecule. This angle is consistent with the tetrahedral arrangement of the hybrid orbitals. By adopting this arrangement, the electron pairs in the molecule are maximally spread apart, resulting in greater stability.
4. What are some examples of molecules that exhibit sp3 hybridization?
Ans. Some examples of molecules that exhibit sp3 hybridization include methane (CH4), ammonia (NH3), and water (H2O). In methane, carbon undergoes sp3 hybridization to form four sigma bonds with hydrogen. Similarly, in ammonia and water, nitrogen and oxygen undergo sp3 hybridization, respectively, to accommodate the lone pairs of electrons.
5. How does sp3 hybridization contribute to the molecular geometry of a compound?
Ans. Sp3 hybridization determines the molecular geometry of a compound by influencing the arrangement of atoms around the central atom. The tetrahedral arrangement of sp3 hybrid orbitals leads to a tetrahedral molecular geometry. However, the presence of lone pairs of electrons can distort the geometry, resulting in trigonal pyramid or bent geometries.
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