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Pi is the Greek letter for "p". The nomenclature is defined in this way because it has similar properties as p orbitals, including two electron dense regions seperated by a nodal plane. Pi bond is not shown in the p orbital; it is formed by overlapping two p orbitals from two atoms side-by-side. Hope this help!
So in the event that a molecule such as Te (ground state: 5p4) forms a double bond with an element, would it be only the p orbitals that would take part in the double bond? Are orbitals above p (as in d or f) able to form pi bonds, or are those a different type of bond that we haven't discussed yet? It would be great if anyone could help me with this! Thank you!
Pi bonds show up in the p orbital rather than the s orbital because they occur when two p orbitals overlap side by side. This results in bound atoms being unable to rotate and electron density both above and below the internuclear axis.
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