BMB 207 Lecture Notes - Lecture 23: Sigma Bond, Antibonding Molecular Orbital, Covalent Bond

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Hybrid molecular orbitals: bond type determines shape. Atomic shell 1: shell 1 has 1 subshell- the 1s subshell has 1 orbital which holds 2 electrons. Molecular orbital: atomic orbitals combine to form molecular orbitals, the combination of two atomic orbitals forms 2 molecular orbitals, one bonding orbital and one anti-bonding orbital. We will be concerned with bonding orbitals: molecular orbitals can hybridize to form the best (lowest energy) con guration for the speci c, the combined sp^3 binds form the shape of a regular tetrahedron. Orbital overlap to form sigma bonds: the simplest covalent bond is the sigma bond which can be formed from pairwise overlap of combinations of atomic orbitals, note the directionality and symmetry of the sigma bonds. Bonding pairs: each bonding pair of electrons in a structure may be represented as a line to simplify the structure, add non-binding electrons in lewis structures, each line represents two electrons and should be counted as two electrons.

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