Transition metal

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Transition Metal

Transition metal (pronunciation: tran-zish-uhn met-l) is a term used in Chemistry to refer to any of the set of metallic elements occupying a central block (Groups IVB–VIII, IB, and IIB, or 4–12) in the periodic table.

Etymology

The term "transition metal" was coined from the fact that the elements in question are the metals that make up the transition series of the periodic table. The transition series is so named because it lies between the "main group elements" on both sides of the periodic table.

Definition

Transition metals are defined as those elements that have (or can have) partially filled d orbitals. They are characterized by multiple oxidation states, colored complexes, and the ability to form stable Coordination compounds.

Properties

Transition metals have several shared properties, including:

  • High melting points and boiling points: This is due to the strong Metallic bonding caused by the delocalization of electrons.
  • High densities: Transition metals have high atomic weights and strong intermolecular forces, leading to high densities.
  • Multiple oxidation states: Transition metals can lose different numbers of electrons from the d-orbitals, leading to multiple oxidation states.
  • Formation of colored compounds: Transition metals can absorb certain wavelengths of light, leading to the formation of colored compounds.

Examples

Examples of transition metals include Iron (Fe), Copper (Cu), Nickel (Ni), Zinc (Zn), and Silver (Ag), among others.

Related Terms

  • Periodic Table: A tabular arrangement of chemical elements, organized based on their atomic number, electron configuration, and recurring chemical properties.
  • Metallic Bonding: The chemical bonding that arises from the attraction between mobile electrons and fixed, positively charged metallic atoms.
  • Coordination Compounds: A type of compound that includes a central atom or ion, which is usually metallic and is called the coordination center, surrounded by a set of ligands.

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