Do hybrid orbitals (such as sp, sp2, sp3) possess higher energy than unhybridized ones (such as 2s, 2p)?
I believe, for example in sp3 hybrids, that the sp3 hybrids are higher than the pure s but lower than the pure p orbitals. I tried to find something on the web but this site is about the best I could do.
http://lsc.ucdavis.edu/~holliste/Jim2c/HybridizationCarbon.pdf
Thank you for clarifying! I understand this concept now.
To determine whether hybrid orbitals possess higher energy than unhybridized ones, we need to consider the underlying electronic structure and bonding in an atom.
Hybrid orbitals result from the mixing of atomic orbitals to form new hybrid orbitals. The most common hybrid orbitals are sp, sp2, and sp3, which result from the mixing of s and p orbitals.
In general, the energy of hybrid orbitals is different from that of unhybridized ones. Hybrid orbitals are higher in energy compared to the pure s and p orbitals that are used to create them. This can be explained by the concept of hybridization.
When hybridization occurs, energy is required to promote an electron from the lower energy atomic orbital to the higher energy hybrid orbital. The energy required for this process is obtained from the conversion of some electronic energy into a different form, such as the energy of molecular bonds.
After hybridization, the resulting hybrid orbitals have a higher energy than the original unhybridized orbitals. This increase in energy allows for efficient bonding with other atoms in compounds.
In summary, hybrid orbitals generally possess higher energy than unhybridized atomic orbitals due to the energy required for the process of hybridization.