CHEM 1A Lecture Notes - Lecture 10: Valence Bond Theory, Xenon Difluoride, Xenon Tetrafluoride

• School: UC-Irvine
• Department: Chemistry
• Course: CHEM 1A
• Professor: Craig Martens

Document Summary

These molecules are combinations of the shapes around each central atom. Ch3ch3 (ethane) has a tetrahedral arrangement around each carbon atom. Fractional charge distribution in polar bonds may lead to a dipole moment of the molecule. Dipolar covalent bonds have a dipole moment. A covalent bond forms when orbitals of two atoms overlap and the overlapping region contains an electron pair. Because of the pauli exclusion principle, the region between two atoms can only contain two electrons and they must have opposing spins. The strength of a chemical bond depends on the amount of overlap between the two orbitals, which depends on their shape and orientation. Bonds involving p- or d- orbitals are oriented in the direction that maximizes orbital overlap and bond strength. The number of hybrid orbitals formed must be equal to the orginal number of atomic orbitals.