Transition metals have unique properties due to their ability to split valence electrons between outer shells. They occupy the d-block of the periodic table, but not all d-block elements are transition metals. They are hard, brittle, and good conductors, and include elements like iron, copper, and gold. Classification can vary, so clarification is important.
Transition metals are chemical elements that share the unusual trait of splitting valence electrons that they can form chemical bonds with other elements between the two outer shells of their structure. Normally, only the outermost shell can supply valence electrons. This unique behavior leads to some distinctive properties that make transition metals stand out from other elements. They have a number of oxidation states, for example, and tend to form very stable bonds with a variety of elements.
These elements are found around the center of the periodic table and occupy most of the region known as the d-block. Some simplistic definitions describe transition metals as simply d-block elements, but this is not entirely correct. Not all d-block elements fall into this categorization, although many do. Some elements, such as zinc, tend to be subjects of controversy and can be variably classified into and out of transition metals. Some of the transition metals are also toxic and can pose a threat to human or environmental health and safety.
With the exception of mercury, which is a liquid, transition metals tend to be very hard. They are also brittle and have an extremely high melting point. Their energy states make them excellent conductors and many are used in the manufacture of electronic components due to their good conduction. These metals can be found in many regions of the world, and many are commercially mined for use in manufacturing.
Some examples of transition metals include iron, copper, cobalt, nickel, gold, platinum and manganese. Within the transitional group, there is tremendous diversity. Some of these items, for example, are necessary dietary nutrients that people need to consume in trace amounts for their health. Others naturally appear in different forms, depending on the structure of their outer shells. The variance within this broad grouping is one reason why it is often difficult to classify transition metals.
Many periodic tables color-code elements by group for convenience. Astute observers may note that the elements coded as transition metals can vary, depending on conventions at any given time or in a particular region. Students should ensure they are using the definition used by their instructors and should request clarification if they are unsure if an element is considered a member of this group. The instructor’s opinion on the subject can be a deciding factor for something like a chemistry test, and it’s important to use the response the instructor would expect.
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