CHEM101 Lecture Notes - Lecture 7: Aufbau Principle, Bond Energy, Antibonding Molecular Orbital

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CHEM101 Full Course Notes
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CHEM101 Full Course Notes
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Lintroductory university chemistry i (chem 101 / 103) It accounts for, at least qualitatively, the stability of covalent compounds in terms of overlapping atomic orbitals. It uses the concept of hybridization to explain the molecular geometries predicted by the vsepr. It fails to explain the magnetic properties of some covalent compounds such as o2 which is paramagnetic. Molecular orbital formations: molecular orbital theory describes covalent bonds as a result of the interaction of the atomic orbitals (ao) of the bonding atoms forming molecular orbitals (mo) Energy diagram: mo1 is called the bonding mo. It is higher energy due to strong repulsion between the nuclei which are not shielded by the electron: the antibonding mo is called a *1s mo. Basic ideas of mos: the number of mos formed must equal to the number of atomic orbitals, electrons in the aos are assigned into these mos. In the formation of mos, the aos of the atoms no longer exists.

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