Calculate Oxidation Numbers definitions Flashcards
Calculate Oxidation Numbers definitions
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Oxidation Number
Indicates an element's ability to gain, lose, or share electrons in its elemental or compound form. Redox Reactions
Chemical reactions involving the transfer of electrons between two species, encompassing oxidation and reduction processes. Standard State
The natural form of an element where its oxidation number is zero. Diatomic Molecules
Molecules composed of two atoms, such as H2, N2, O2, F2, Cl2, Br2, and I2, with an oxidation number of zero. Cations
Positively charged ions formed when an element loses electrons. Anions
Negatively charged ions formed when an element gains electrons. Monoatomic Ion
An ion consisting of a single atom with an oxidation number equal to its charge. Peroxide
A compound with two oxygen atoms bonded together, typically with an oxidation number of -1 for oxygen. Superoxide
A compound with one oxygen atom bonded to a group 1A element, with an oxidation number of -1/2 for oxygen. Group 1A Elements
Elements with an oxidation number of +1 when bonded to other elements. Group 2A Elements
Elements with an oxidation number of +2 when bonded to other elements. Group 7A Elements
Elements like chlorine, bromine, and iodine with an oxidation number of -1, except when bonded to oxygen. Hydrogen
Has an oxidation number of +1 when bonded to nonmetals and -1 when bonded to metals. Oxygen
Typically has an oxidation number of -2, except in peroxides and superoxides. Noble Gases
Elements that typically have no charge due to their stable electron configuration.
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