In TiCl3, each titanium atom has one d electron, rendering its derivatives paramagnetic, that is, the substance is attracted into a magnetic field.

Its structure consists of chains of TiCl6 octahedra that share opposite faces such that the closest Ti–Ti contact is 2.91 Å.

The three violet "layered" forms, named for their color and their tendency to flake, are called alpha (α), gamma (γ), and delta (δ).

Finally, disorder in shift successions, causes an intermediate between alpha and gamma structures, called the δ form.

In contrast, the trihalides of the heavier metals hafnium and zirconium engage in metal-metal bonding.

The reaction is driven by the loss of volatile TiCl4:[9] The ternary halides, such as A3TiCl6, have structures that depend on the cation (A+) added.

The catalytic activities depend strongly on the polymorph of the TiCl3 (α vs. β vs. γ vs. δ) and the method of preparation.

[12] TiCl3 is also a specialized reagent in organic synthesis, useful for reductive coupling reactions, often in the presence of added reducing agents such as zinc.

[15] TiCl3 and most of its complexes are typically handled under air-free conditions to prevent reactions with oxygen and moisture.