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Because Group 1 metals always have an oxidation state of +1 in their compounds, it follows that the hydrogen must have an oxidation state of -1 (+1 -1 = 0). The oxidation state of a simple ion like hydride is equal to the charge on the ion-in this case, -1.Īlternatively, the sum of the oxidation states in a neutral compound is zero. Here the hydrogen exists as a hydride ion, H. Hydrogen in the metal hydrides: Metal hydrides include compounds like sodium hydride, NaH. Some elements almost always have the same oxidation states in their compounds:.Remember that electronegativity is greatest at the top-right of the periodic table and decreases toward the bottom-left. The less electronegative element is assigned a positive oxidation state.
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The oxidation state of an uncombined element is zero.Here the sulfur has an oxidation state of -2. This is impossible for vanadium, but is common for nonmetals such as sulfur: If electrons are added to an elemental species, its oxidation number becomes negative. The ion could be reduced back to elemental vanadium, with an oxidation state of zero. If the process is reversed, or electrons are added, the oxidation state decreases. \]Įach time the vanadium is oxidized (and loses another electron), its oxidation state increases by 1.