"In chemistry, the oxidation state, or oxidation number, is the hypothetical charge of an atom if all of its bonds to other atoms were fully ionic."
A number assigned to an atom in a molecule or ion to indicate the general distribution of electrons among the bonded atoms.
Valence Electrons: Valence electrons are the electrons present in the outermost shell of an atom that are involved in chemical reactions and determine the oxidation state of the atom.
Electronegativity: The electronegativity of an element is a measure of its ability to attract electrons towards itself during a chemical reaction.
Octet Rule: The octet rule states that atoms tend to gain, lose, or share electrons in order to achieve a stable configuration with eight electrons in their valence shell.
Lewis Structures: Lewis structures are diagrams that represent the valence electrons of atoms and their bonds in a molecule. They are useful for determining the oxidation state of an atom in a compound.
Ionic Bonding: Ionic bonding is the transfer of electrons from one atom to another resulting in the formation of ions with opposite charges.
Covalent Bonding: Covalent bonding is the sharing of electrons between atoms to form a stable molecule.
Oxidation: Oxidation is the loss of electrons by an atom, which leads to an increase in its oxidation state.
Reduction: Reduction is the gain of electrons by an atom, which leads to a decrease in its oxidation state.
Half-Reactions: Half-reactions show the oxidation or reduction process of a chemical reaction separately.
Redox Reactions: Redox reactions involve the transfer of electrons from the reducing agent to the oxidizing agent.
Balancing Redox Reactions: Balancing redox reactions involves balancing the number of electrons transferred along with the other reactants and products.
Galvanic Cells: Galvanic cells convert chemical energy into electrical energy through redox reactions.
Electrochemical Cells: Electrochemical cells involve the use of redox reactions to produce electrical energy.
Nernst Equation: The Nernst equation is used to calculate the potential of an electrochemical cell at non-standard conditions.
Biochemical Redox Reactions: Biochemical redox reactions involve redox reactions in living organisms, such as cellular respiration and photosynthesis.
Reduction: The gaining of electrons by a molecule or atom, resulting in a decrease in oxidation state.
Oxidation: The loss of electrons by a molecule or atom, resulting in an increase in oxidation state.
Redox: Abbreviation for reduction-oxidation, a reaction that involves both reduction and oxidation processes simultaneously.
Single displacement: Also known as single replacement, a reaction in which one element replaces another element in a compound, resulting in a change in oxidation state.
Double displacement: Also known as double replacement, a reaction in which two compounds exchange ions, resulting in a change in oxidation state.
Acid-base: A reaction in which an acid and a base react to form a salt and water, with no change in oxidation state.
Combustion: A reaction in which a substance reacts with oxygen gas, resulting in a release of energy and an increase in oxidation state.
Precipitation: A reaction in which two soluble salts are combined and a solid precipitate is formed, with no change in oxidation state.
Hydrolysis: A reaction in which a compound reacts with water to form two products, with no change in oxidation state.
Addition: A reaction in which two or more substances combine to form a single product, with no change in oxidation state.
"It describes the degree of oxidation (loss of electrons) of an atom in a chemical compound."
"Yes, conceptually, the oxidation state may be positive, negative, or zero."
"While fully ionic bonds are not found in nature, many bonds exhibit strong ionicity."
"Oxidation state is a useful predictor of charge in many bonds that exhibit strong ionicity."
"The oxidation state of an atom does not represent the 'real' charge on that atom or any other actual atomic property."
"No, high oxidation states are not common as the ionization energy required to produce a multiply positive ion is far greater than the energies available in chemical reactions."
"Yes, the oxidation states of atoms in a given compound may vary depending on the choice of electronegativity scale used in their calculation."
"Yes, the oxidation state of an atom in a compound is purely a formalism."
"It is nevertheless important in understanding the nomenclature conventions of inorganic compounds."
"The highest known oxidation state is reported to be +9, displayed by iridium in the tetroxoiridium(IX) cation (IrO+4)."
"Yes, it is predicted that even a +10 oxidation state may be achieved by platinum in tetroxoplatinum(X), PtO2+4."
"The lowest oxidation state is -5, as for boron in Al3BC and gallium in pentamagnesium digallide (Mg5Ga2)."
"The oxidation state is represented by a Roman numeral placed after the element name inside parentheses or as a superscript after the element symbol, e.g. Iron(III) oxide."
"The term oxidation was first used by Antoine Lavoisier to signify the reaction of a substance with oxygen."
"Later, it was realized that the substance, upon being oxidized, loses electrons, and the meaning was extended to include other reactions in which electrons are lost, regardless of whether oxygen was involved."
"The increase in the oxidation state of an atom, through a chemical reaction, is known as oxidation."
"A decrease in oxidation state is known as a reduction."
"Such reactions involve the formal transfer of electrons: a net gain in electrons being a reduction, and a net loss of electrons being oxidation."
"For pure elements, the oxidation state is zero."