MO theory is discussed at the general chemistry level but only for diatomic molecules and ions from the second period, again because more atoms or higher periods makes it more complicated and it's just meant to give them a taste of what it is. In this way, what are the types of hybridization sp hybridization (beryllium chloride, acetylene) sp2 hybridization (boron trichloride, ethylene) sp3 hybridization (methane, ethane) sp3d. Do note that sp2 hybridisation means the atom possess three regions of electron density. No general chemistry textbook that I have seen (and I have seen quite a few) discusses 4-electron-3-center bonds because it becomes too complicated at the general chemistry level and not necessary for those students who are not chemistry majors. Some examples of sp2 hybridisation would be benzene, ethene, BCl3. In an ethene molecule, a double bond between carbons forms with one sigma and one pi bond. Main group elements do not use their d-orbitals for bonds and thus cannot be hybridised in any d-containing way. What are the examples for sp2 hybridization For boron to bond with three fluoride atoms in boron trifluoride (BF3), the atomic s- and p-orbitals in boron’s outer shell mix to form three equivalent sp2 hybrid orbitals. We can split this into two cases: main group elements and transition elements.
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