Transition Metals

Transition metals are elements that have a partially filled d orbital. Iron is a transition metal because it has a partially filled 3d orbital.

Transition metals have a general electron configuration of ns^2 np^6 nd^1-10, where n is the principal quantum number and d is the d orbital.

Transition metals typically have high melting points due to the strong metallic bonds between their atoms.

The most common oxidation state for transition metals is +2.

A transition metal complex is a compound that contains a transition metal ion surrounded by ligands. Iron(III) chloride is an example of a transition metal complex because it contains an iron(III) ion surrounded by chloride ligands.

Oxidation is the process by which transition metals lose electrons.

Platinum is an example of a transition metal catalyst because it is used to catalyze a variety of chemical reactions.

Coloration is the phenomenon in which transition metals can change color when exposed to different wavelengths of light.

Steel is an example of a transition metal alloy because it is made up of iron and other elements, such as carbon and manganese.

The d-block elements are the group of transition metals that are located in the middle of the periodic table.

Gold is an example of a transition metal that is used in jewelry.

Hybridization is the process by which transition metals can form multiple bonds with other atoms.

Copper is an example of a transition metal that is used in electronics.

The actinides are the group of transition metals that are located at the bottom of the periodic table.

Iron is an example of a transition metal that is used in medicine.