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A list of metals in order of their reactivity as reducing agents.
A rapid reaction with oxygen accompanied by a flame and the evolution of heat and light.
The slow oxidation of metals exposed to air or water.
A hypothetical reaction that constitutes exclusively either the oxidation or the reduction half of a redox reaction and in whose equation the correct formulas for all species taking part in the change are given together with enough electrons to give the correct electrical balance.
A method for balancing redox reactions that uses half-reactions.
An acid in which the anion is a poorer oxidizing agent than the hydrogen ion
A change in which an oxidation number increases (becomes more positive). A loss of electrons.
The charge that an atom in a molecule or ion would have if all of the electrons in its bonds belonged entirely to the more electronegative atoms; the oxidation state of an atom.
A chemical reaction in which changes in oxidation numbers occur.
An acid in which the anion is a stronger oxidizing agent than H+
The substance that causes oxidation and that is itself reduced.
An oxidation–reduction reaction.
A substance that causes reduction and is itself oxidized
A change in which an oxidation number decrease (becomes less positive and more negative). A gain of electrons.
single replacement reaction
A reaction in which one element replaces another in a compound; usually a redox reaction
An unbalanced equation showing only the formulas of reactants and products.