Hybridization
Question 1: Among sp, sp2, and sp3, which hybrid orbital is more electronegative?
Answer:
The percentage of s character in sp, sp2, and sp3 hybridised carbon is 50%, 33.33%, and 25%, respectively. Because of the spherical shape of the s orbital, it is attracted evenly from all directions by the nucleus. As a result, an s-character hybrid orbital will be closer to the nucleus and thus more electronegative. As a result, the sp hybridised carbon is the most electronegative.
Question 2: What are hybrid orbitals?
Answer:
Hybrid orbitals are formed by combining standard atomic orbitals and resulting in the formation of new atomic orbitals.
Question 3: What are the five shapes of hybridization?
Answer:
Linear, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral are the five basic shapes of hybridization.
Question 4: Why does the amide molecule look like sp3 hybridized but is sp2?
Answer:
If the atom is either enclosed by two or more p orbitals or has a lone pair capable of jumping into a p orbital, the general process of hybridization will change. As a result, in the case of an amide molecule, the lone pair enters a p orbital, resulting in three adjacent parallel p orbitals.
Question 5: What is Bent’s rule?
Answer:
A central atom connected to numerous groups in a molecule will hybridise, causing orbitals with more s character to be directed towards electropositive groups and orbitals with more p character to be directed towards electronegative groups.
Hybridization
The concept of hybridization is defined as the process of combining two atomic orbitals to create a new type of hybridized orbitals. This intermixing typically results in the formation of hybrid orbitals with completely different energies, shapes, and so on. Hybridization is primarily carried out by atomic orbitals of the same energy level. However, both fully filled and half-filled orbitals can participate in this process if their energies are equal. The concept of hybridization is an extension of valence bond theory that helps us understand bond formation, bond energies, and bond lengths.
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