Orbital overlap is a concept used in theories of the chemical bond. It refers to the concentration of orbitals on adjacent atoms in the same region(s) of space, which can lead to bond formation. The importance of orbital overlap was emphasized by Linus Pauling to explain the molecular bond angles observed through experimentation and is the basis for the concept of orbital hybridisation. s orbitals are spherical and have no directionality while p orbitals are oriented 90° to one another. A theory was needed therefore to explain why molecules such as methane (CH4) had observed bond angles of 109.5°. Pauling proposed that s and p orbitals on the carbon atom can combine to form hybrids (sp3 in the case of methane) which are directed toward the hydrogen atoms. The carbon hybrid orbitals have greater overlap with the hydrogen orbitals, and can therefore form stronger C–H bonds.
A quantitative measure of the overlap of two atomic orbitals on atoms A and B is their overlap integral, defined as
The overlap matrix is a square matrix, used in quantum chemistry to describe the inter-relationship of a set of basis vectors of a quantum system, such as an atomic orbital basis set used in molecular electronic structure calculations. In particular, if the vectors are orthogonal to one another, the overlap matrix will be diagonal. In addition, if the basis vectors form an orthonormal set, the overlap matrix will be the identity matrix. The overlap matrix is always n×n, where n is the number of basis functions used. It is a kind of Gramian matrix.
In general, each overlap matrix element is defined as an overlap integral:
- is the j-th wavefunction, defined as :.
In particular, if the set is normalized (though not necessarily orthogonal) then the diagonal elements will be identically 1 and the magnitude of the off-diagonal elements less than or equal to one with equality if and only if there is linear dependence in the basis set as per the Cauchy–Schwarz inequality. Moreover, the matrix is always positive definite; that is to say, the eigenvalues are all strictly positive.
- Anslyn, Eric V./Dougherty, Dennis A. (2006). Modern Physical Organic Chemistry. University Science Books.
- Pauling, Linus. (1960). The Nature Of The Chemical Bond. Cornell University Press.
Quantum Chemistry: Fifth Edition, Ira N. Levine, 2000