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As is observed for most elements, a diatomic scandium hydride has been observed spectroscopically at high temperatures in the gas phase. [5] Scandium borides and carbides are non-stoichiometric, as is typical for neighboring elements. [41] Lower oxidation states (+2, +1, 0) have also been observed in organoscandium compounds. [42] [4] [43] [44]
However there are numerous exceptions; for example the lightest exception is chromium, which would be predicted to have the configuration 1s 2 2s 2 2p 6 3s 2 3p 6 3d 4 4s 2, written as [Ar] 3d 4 4s 2, but whose actual configuration given in the table below is [Ar] 3d 5 4s 1.
3d 1 4s 2: Electrons per shell: 2, 8, 9, 2: ... (t 1/2) mode product; 44m2 Sc synth: 58.61 h: IT: 44 Sc ... ("noble gas") and E173 would be the beginning of period ...
The chemistry of scandium is almost completely dominated by the trivalent ion, Sc 3+, due to its electron configuration, [Ar] 3d 1 4s 2. The radii of M 3+ ions in the table below indicate that the chemical properties of scandium ions have more in common with yttrium ions than with aluminium ions. In part because of this similarity, scandium is ...
Scandium concentrates in the liver and is a threat to it; some of its compounds are possibly carcinogenic, even though in general scandium is not toxic. [80] Scandium is known to have reached the food chain, but in trace amounts only; a typical human takes in less than 0.1 micrograms per day. [80]
In chemistry and atomic physics, an electron shell may be thought of as an orbit that electrons follow around an atom's nucleus.The closest shell to the nucleus is called the "1 shell" (also called the "K shell"), followed by the "2 shell" (or "L shell"), then the "3 shell" (or "M shell"), and so on further and further from the nucleus.
Element Negative states Positive states Group Notes −5 −4 −3 −2 −1 0 +1 +2 +3 +4 +5 +6 +7 +8 +9 Z; 1 hydrogen: H −1 +1: 1 2 helium: He 0 18
The molecular orbitals are labelled according to their symmetry, [e] rather than the atomic orbital labels used for atoms and monatomic ions; hence, the electron configuration of the dioxygen molecule, O 2, is written 1σ g 2 1σ u 2 2σ g 2 2σ u 2 3σ g 2 1π u 4 1π g 2, [39] [40] or equivalently 1σ g 2 1σ u 2 2σ g 2 2σ u 2 1π u 4 3σ g ...