CHEM 1061 Chapter Notes - Chapter 11: Covalent Bond, Valence Electron, Pi Bond
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Document Summary
Covalent bond forms when the orbitals of two atoms overlap and a pair of electrons occupy the overlap region. Maximum capacity for two electrons that have opposite (paired) spins. Maximum overlap of bonding of bonding orbitals. The greater the orbital overlap, the closer the nuclei are to the electrons, and the stronger the bond. Valence electrons in the isolated atoms become new orbitals in the molecule. Number of hybrid orbitals formed equals the number of atomic orbitals mixed. The type of hybrid orbitals formed varies with the types of atomic orbitals mixed. The shape and orientation of a hybrid orbital maximize its overlap with the orbital of the other atom in the bond. D-orbital hybridization is less important: shapes with expanded valence shells. Models of orbital overlap and the types of covalent bonds. Pi bond is weaker than a sigma bond. Orbitals overlap less side to side than end to end.
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