Which property is NOT characteristic of transition metals?

Transition metals are known for several distinct properties that set them apart from other elements on the periodic table. One key characteristic of transition metals is their ability to form more than one oxidation state or ion. This property arises from their partially filled d-orbitals, which allows for the loss of different numbers of electrons depending on the chemical reaction.

Another notable feature of transition metals is their colorful compounds, resulting from d-d electron transitions when they absorb specific wavelengths of light. This behavior is a common characteristic among many transition metals.

Additionally, transition metals typically have high melting and boiling points compared to elements in other groups. This is due to the strong metallic bonding occurring in these metals, which results from the delocalization of d-electrons throughout the metal lattice.

In contrast, transition metals are actually well-known for their effectiveness as catalysts in various chemical processes, often enhancing reaction rates without being consumed in the reaction. Therefore, stating that they make poor catalysts does not accurately reflect their well-established catalytic properties, which are extensively utilized in industrial applications.

Thus, the property that is not characteristic of transition metals is their ability to make poor catalysts, as they are, in reality, often quite efficient in that role.