- #1
ciubba
- 65
- 2
I'm seeing conflicting answers among various textbooks. I would predict that it forms SP3 hybrid orbitals, and yet its bond angles are far from 109.5.
Edit: H2S, rather.
Edit: H2S, rather.
Last edited:
I see. How does one determine whether pure hybridization is a more appropriate model to describe orbital shape?Borek said:No hybridization at all and pure sp3 are just two ends of a continuum.
For some highly symmetrical molecules (say, CH4) hybridization of the central atom is a pure sp3. But for some other molecules, like H2S, what we observe is just some partial hybridization, in which bonds are not equivalent.
Hybrid orbitals are a combination of atomic orbitals that are formed when atoms bond together to form molecules. They are important because they help explain the shapes and bonding properties of molecules.
Hybrid orbitals are formed through a process called hybridization, where the atomic orbitals of different energy levels combine to form new hybrid orbitals with different properties.
These are different types of hybridization that occur when an atom forms different numbers of bonds. sp hybridization is when an atom forms 2 bonds, sp2 is when an atom forms 3 bonds, and sp3 is when an atom forms 4 bonds.
The hybridization of an atom can be determined by looking at the number of bonds and lone pairs around the atom. The number of hybrid orbitals needed is equal to the number of bonds and lone pairs.
Yes, the type of hybridization and the resulting shape of a molecule can help predict its properties, such as polarity and reactivity. This information is important in understanding the behavior of molecules in various chemical reactions.