Charge-transfer complexes tend to have very intense colors for different reasons.

For charge-transfer complexes and conjugated systems the band width is determined by a variety of factors.

With electron donors such as triphenylphosphine and pyridine it forms a charge-transfer complex.

There are a wide range of other organic superconductors including many other charge-transfer complexes.

Mainly due to low mobility, even unpaired electrons may be stable in charge-transfer complexes.

Pigments and dyes like these are charge-transfer complexes.

Hexaphenylbenzenes like H (fig. 3) lend themselves extremely well to forming charge-transfer complexes.

Charge-transfer complexes do not experience d-d transitions.

For example, the classic example of a charge-transfer complex is that between iodine and starch to form an intense purple color.

Pigments and dyes like these tranfers electric charges from one part to another (charge-transfer complexes).

At least locally, charge-transfer complexes often exhibit similar conduction mechanisms to inorganic semiconductors.

The nature of the attraction in a charge-transfer complex is not a stable chemical bond, and is thus much weaker than covalent forces.

These are organic charge-transfer complexes and various linear-backbone conductive polymers derived from polyacetylene.

In inorganic chemistry, most charge-transfer complexes involve electron transfer between metal atoms and ligands.

A Bechgaard salt is any one of a number of organic charge-transfer complexes that exhibit superconductivity at low temperatures.

First, the diazonium reagent adsorbs noncovalently to an empty site on the nanotube surface, forming a charge-transfer complex.

Electrons from other states can also be promoted to a π-system MO (n to π) as often happens in charge-transfer complexes.

The reactant forms a charge-transfer complex at the nanotube surface, where electron donation from the latter stabilizes the transition state and accelerates the forward rate.

Charge-transfer complexes form when iodine is dissolved in polar solvents, modifying the energy distribution of iodine's molecular orbitals, hence changing the colour.

Charge-transfer complexes exist in many types of molecules, inorganic as well as organic, and in solids, liquids, and solutions.

The colors are intense and seem to be caused by Cu(I)-Hg(II) charge-transfer complexes.

Most pigments are charge-transfer complexes, like transition metal compounds, with broad absorption bands that subtract most of the colors of the incident white light.

This method has been typically applied to reaction equilibria that form one-to-one complexes, such as charge-transfer complexes and host-guest molecular complexation.

The electromagnetic theory posits the excitation of localized surface plasmons, while the chemical theory proposes the formation of charge-transfer complexes.

Charge-transfer complexes are formed by weak association of molecules or molecular subgroups, one acting as an electron donor and another as an electron acceptor.