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Template: Oxides. 22 languages. ... Print/export Download as PDF; Printable version; ... This page was last edited on 12 November 2024, ...
An oxide (/ ˈ ɒ k s aɪ d /) is a chemical compound containing at least one oxygen atom and one other element [1] in its chemical formula. "Oxide" itself is the dianion (anion bearing a net charge of –2) of oxygen, an O 2– ion with oxygen in the oxidation state of −2. Most of the Earth's crust consists of oxides. Even materials ...
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An oxide is a chemical compound in which one or more oxygen atoms combined with another element, such as H 2 O or CO 2. Based on their acid-base characteristics, oxides can be classified into four categories: acidic oxides, basic oxides, and amphoteric oxides and neutral oxides.
In these cases the oxidation number (the same as the charge) of the metal ion is represented by a Roman numeral in parentheses immediately following the metal ion name. For example, in uranium(VI) fluoride the oxidation number of uranium is 6. Another example is the iron oxides. FeO is iron(II) oxide and Fe 2 O 3 is iron(III) oxide.
An oxyanion, or oxoanion, is an ion with the generic formula A x O z− y (where A represents a chemical element and O represents an oxygen atom). Oxyanions are formed by a large majority of the chemical elements. [1] The formulae of simple oxyanions are determined by the octet rule. The corresponding oxyacid of an oxyanion is the compound H z ...
[1] [2] In simple terms, formal charge is the difference between the number of valence electrons of an atom in a neutral free state and the number assigned to that atom in a Lewis structure. When determining the best Lewis structure (or predominant resonance structure ) for a molecule, the structure is chosen such that the formal charge on each ...
When the electropositive element is a metal, the compounds are sometimes referred to as “metal-rich”. Thus the normal oxide of caesium is Cs 2 O, which is described as a Cs + salt of O 2−. A suboxide of caesium is Cs 11 O 3, where the charge on Cs is clearly less than 1+, but the oxide is still described as O 2−.
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