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The correct response is a) Ag. The oxidation number of an atom of a pure element is 0. The charge an atom would have if the compound were made up of ions is known as its oxidation number.
The oxidation state, often known as the oxidation number, in chemistry refers to the hypothetical charge that an atom would have if all of its links to other atoms were entirely ionic. It describes how much an atom has oxidized (lost electrons) in a chemical complex. The oxidation state can theoretically be positive, negative, or zero. Although nature does not include entirely ionic bonds, it does contain numerous strong ionic bonds, making the oxidation state a reasonable predictor of charge. The formal charge or any other genuine atomic attribute of an atom is not represented by the oxidation state of that atom. This is especially true for high oxidation states, where the amount of ionization energy needed to create a multiply positive ion is much more than the amount of energy available in chemical reactions. A compound's atoms' oxidation states can also change based on the electronegativity scale that was used to calculate them. An atom's oxidation state in a compound is thus just a formalization. Nevertheless, it is crucial to comprehend inorganic compound nomenclature rules. Additionally, a number of chemical reaction findings can be fundamentally described in terms of oxidation states.
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Assign oxidation states to each atom in each element, ion, or compound. a. Ag, b. Ag^+Ag+ c. CaF_2CaF 2 d. H_2SH2S e. CO_3 {2-}CO32− f. \mathrm{CrO}_{4}^{2-}CrO42−
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