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  2. Transition metal - Wikipedia

    en.wikipedia.org/wiki/Transition_metal

    As implied by the name, all transition metals are metals and thus conductors of electricity. In general, transition metals possess a high density and high melting points and boiling points. These properties are due to metallic bonding by delocalized d electrons, leading to cohesion which increases with the number of shared electrons. However ...

  3. Block (periodic table) - Wikipedia

    en.wikipedia.org/wiki/Block_(periodic_table)

    These elements are generally not considered part of any group. They are sometimes called inner transition metals because they provide a transition between the s-block and d-block in the 6th and 7th row (period), in the same way that the d-block transition metals provide a transitional bridge between the s-block and p-block in the 4th and 5th rows.

  4. Valence electron - Wikipedia

    en.wikipedia.org/wiki/Valence_electron

    Similar patterns hold for the (n−2)f energy levels of inner transition metals. The d electron count is an alternative tool for understanding the chemistry of a transition metal. The number of valence electrons

  5. Names for sets of chemical elements - Wikipedia

    en.wikipedia.org/wiki/Names_for_sets_of_chemical...

    Non-ferrous metals - Metals or alloys that do not contain iron in appreciable amounts. Platinum group – Ru, Rh, Pd, Os, Ir, Pt. Post-transition metals – The metals coming after the transition metals. Many other names have been used for this set, and its borders are not agreed on.

  6. Periodic table - Wikipedia

    en.wikipedia.org/wiki/Periodic_table

    [39] [58] From gallium onwards, the 3d orbitals form part of the electronic core, and no longer participate in chemistry. [57] The s- and p-block elements, which fill their outer shells, are called main-group elements; the d-block elements (coloured blue below), which fill an inner shell, are called transition elements (or transition metals ...

  7. Iron - Wikipedia

    en.wikipedia.org/wiki/Iron

    Iron shows the characteristic chemical properties of the transition metals, namely the ability to form variable oxidation states differing by steps of one and a very large coordination and organometallic chemistry: indeed, it was the discovery of an iron compound, ferrocene, that revolutionalized the latter field in the 1950s. [59]

  8. Group 4 element - Wikipedia

    en.wikipedia.org/wiki/Group_4_element

    As is typical for early transition metals, zirconium and hafnium have only the group oxidation state of +4 as a major one, and are quite electropositive and have a less rich coordination chemistry. Due to the effects of the lanthanide contraction, they are very similar in properties. Titanium is somewhat distinct due to its smaller size: it has ...

  9. Actinide concept - Wikipedia

    en.wikipedia.org/wiki/Actinide_concept

    In nuclear chemistry, the actinide concept (also known as actinide hypothesis) proposed that the actinides form a second inner transition series homologous to the lanthanides. Its origins stem from observation of lanthanide-like properties in transuranic elements in contrast to the distinct complex chemistry of previously known actinides.