The following is by my understanding.<\/p>\n
\nI mention in my post from July 13, 2024<\/a> the idea of some atoms having more than an octet of electrons in the outer shell. The reason turns out to be that the central atom has access to a d orbital.<\/p>\n \nIn the case of sulfate, the sulfur atom has twelve electrons in its outer shell. Yet, we are told that the shape-determining hybridization is sp3, so that the molecule is tetrahedral. The other two bonds are pi bonds. Then, what about those pi bonds? What orbitals do they involve?<\/p>\n \nIt turns out that said pi bonds are dπ-pπ bonds, specifically from d orbitals on the sulfur atom to p orbitals on the oxygen atoms. Some d orbitals have shapes that permit them to overlap with p orbitals, making dπ-pπ bonds possible.<\/p>\n \nSource:<\/p>\n Haas, K. (n.d.) “Quantum Numbers and Atomic Wavefunctions.” https:\/\/chem.libretexts.org\/Courses\/East_Tennessee_State_University\/CHEM_3110%3A_Descriptive_Inorganic_Chemistry\/02%3A_Atomic_Theory\/2.01%3A_Quantum_Numbers_and_Atomic_Wavefunctions#Angular_nodeschem.libretexts.org<\/a><\/p>\n chem.libretexts.org: “Orbital Overlap.”<\/a><\/p>\n chem.libretexts.org: “Hybrid Atomic Orbitals.”<\/a><\/p>\nJack of Oracle Tutoring by Jack and Diane,<\/a> Campbell River, BC.\n","protected":false},"excerpt":{"rendered":" Tutoring chemistry, one might be asked about the nature of bonds. The tutor mentions hybridization and overlap. The following is by my understanding. I mention in my post from July 13, 2024 the idea of some atoms having more than …<\/p>\n