The transition metals are malleable (easily hammered into shape or bent). Start studying Transition Metals. Transition metals look shiny and metallic. These metals tend to be very hard. :D. Okay, I did my research and I found the reason why 'Zinc is not considered to be a transition metal'. 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+). 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+). The transition metals are compounds that form at least 1 stable ion where the compound has an incomplete d subshell. Hello, it's Gloria! Scandium and zinc are not transition metals simply because they do not form ions with incomplete d-subshells. 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. A Zn 2+ cation has shed the two electrons in … By definition, a transition metal must do this. 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. 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+). 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. Sc forms 3+ ions, losing the two 4s electrons and a 3d electron (1s2, 2s2, 2p6, 3s2, 3p6) Zn forms 2+ ions, losing only the two 4s electrons (1s2, 2s2, 2p6, 3s2, 3p6, 3d10) The chemistry of zinc is almost entirely governed by its +2 ion charge. 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. Scandium is not a typical transition metal as its common Sc 3+ has no d electrons. Learn vocabulary, terms, and more with flashcards, games, and other study tools. 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". The electronic configuration for a zinc atom is 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 2, 3d 10. 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