![]() ![]() ![]() As a result, the sp3 orbitals that form when one s- and three p-orbitals combine will be arranged at an angle reflecting a mixture between these two types of orbitals (in this case, 109.5º): Let's take a look at the orbital filling diagram for the valence electrons on carbon (see The Modern Atom for more on orbital filling diagrams).įigure 10.4 When orbitals combine to form hybrid orbitals, both their shapes and energies are averaged.Īs you can see from this diagram, the hybridized orbital configuration of carbon allows room for four covalent bonds, which matches well with the four hydrogen atoms covalently bonded in methane.Īs we mentioned in The Modern Atom, s-orbitals are spherical and p-orbitals are at 90-degree angles to one another. It's probably easiest to understand how hybrid orbitals work by showing you an example. Subsequently, all orbitals within an atom that contain valence electrons combine with one another to form "hybrid orbitals." As you might expect, the electrons in covalent bonds, as is the case with electrons everywhere, prefer to be as far apart from each other as possible because they repel each other. However, when atoms form covalent compounds, atomic orbitals are insufficient because they force the bonded atoms to be too close to each other. Up to now, we've learned the shapes and relative energies of s-, p-, d-, and f-orbitals. In order for the electrons to spread further than 90º from each other, we have to come up with a new model that allows for this.
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