The transition metals are compounds that form at least 1 stable ion where the compound has an incomplete d subshell. The electronic configuration for a zinc atom is 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 2, 3d 10. Start studying Transition Metals. By definition, a transition metal must do this. Zinc is not consider as a transition metal because its compounds or ions (Zn2+) contain a full filled d-orbital or sub shell and are unstable.Moreover it have only one ion which is the (Zn2+). These metals tend to be very hard. The transition metals are malleable (easily hammered into shape or bent). The chemistry of zinc is almost entirely governed by its +2 ion charge. Zinc has full d orbits and therefore does not meet the definition of a transition metal, which is "a metal that forms one or more stable ions with incomplete d orbits". Hence zinc do not form colored aqueous ions because it do not have at least one vacant d-orbital in which it can receive an electron in a reaction. This is because it has a relatively low melting and boiling point; in general transition metals have HIGH melting and boiling points, melting at 420 °C, and boiling at 900 °C, and has the lowest melting point of all the transition metals aside from mercury and cadmium. A Zn 2+ cation has shed the two electrons in … Zinc is not consider as a transition metal because its compounds or ions (Zn2+) contain a full filled d-orbital or sub shell and are unstable.Moreover it have only one ion which is the (Zn2+). 13.2.2 Explain why Sc and Zn are not considered to be transition elements. The elements of group 12 i.e., Zinc, Cadmium, and Mercury are generally not regarded as transition elements as their atoms and all ions formed have completely filled d-orbitals i.e., these do not have partially filled d-orbitals in atomic state or common oxidation state (Zn 2+, Cd 2+, Hg 2+). Explain why Zinc is not classified as a transition metal but is classified as a d block element. A transition metal element is defined as an element that possesses an incomplete d sub-level in one or more of its oxidation states. Scandium and zinc are not transition metals simply because they do not form ions with incomplete d-subshells. Hence zinc do not form colored aqueous ions because it do not have at least one vacant d-orbital in which it can receive an electron in a reaction. Transition elements are defined as elements that form at least one ion that contains partially filled d orbitals. Therefore, Scandium is not a transition metal, because it forms only Sc3+ ions with n d-electrons, and Zn is not a transition metal because it forms only Zn2+ ions with all the 3d electrons present. Hello, it's Gloria! Transition metals look shiny and metallic. Scandium is not a typical transition metal as its common Sc 3+ has no d electrons. 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