CHEM 1AA3 Lecture Notes - Orbital Hybridisation, Electron Configuration, Lewis Acids And Bases

• School: McMaster University
• Department: Chemistry
• Course: CHEM 1AA3
• Professor: Pippa Lock

Document Summary

Imagine bringing together two h atoms that are initially far apart. When h atoms are far apart, the two do not interact with each other and by convention, the net energy of interaction between the two h atoms is zero. As the two h atoms approach each other, three types of interactions occur: each electron is attracted to the other nucleus, electrons repel each other, the two nuclei repel each other. As two h atoms approach each other, these regions begin to interpenetrate. We say that the two orbitals overlap. Furthermore, we say that a bond is produced between the two atoms because of the high electron density probability found in the region between the atomic nuclei where the 1s orbitals overlap. The increased electron density, with its negative charge, attracts the two positively charged nuclei. In this way, a covalent bond is formed between the two h atoms in the h2 molecule.