4.11:
Oxidation Numbers
Redox reactions between metals and nonmetals typically involve a complete transfer of electrons to form ionic compounds; hence, they are easy to identify. However, redox reactions involving only nonmetals with a partial transfer of electrons are not as easily identifiable.
Redox reactions are characterized by changes in the oxidation states of the atoms, which indicates electron movement between the atoms.
The oxidation state, or oxidation number, of an atom in a compound is the charge it would have if the shared electrons in each heteronuclear bond were completely transferred to the more electronegative atom. Homonuclear bonds are divided equally.
For instance, in gaseous hydrogen chloride, chlorine is more electronegative. If hydrogen’s electron is transferred completely to chlorine, chlorine gets a 1− charge, corresponding to the −1 oxidation state, and hydrogen gets a 1+ charge, corresponding to the +1 oxidation state.
Oxidation states can be assigned to atoms in elemental form and in most ions and compounds using specific rules. The first three rules are always followed. The remaining rules are applied one by one until the first three rules are satisfied.
These rules will now be applied to identify whether the formation reactions of sulfur dioxide and calcium carbonate are redox reactions.
According to rule number 1, elements in the free state have an oxidation number of zero, so elemental sulfur and oxygen are both assigned the oxidation number zero.
According to rule number 3, the sum of the oxidation numbers in a neutral compound is zero so the oxidation numbers of sulfur and oxygen in SO2 must sum to zero.
In accordance with rule number 6, the oxidation number of each oxygen is −2 in SO2. Two oxygen atoms sum to −4. The oxidation number of sulfur is, therefore, +4.
The oxidation number of sulfur increases from zero to +4, so it is oxidized, while the oxidation number of oxygen decreases from zero to −2, so it is reduced. Thus, this is a redox reaction.
In the case of calcium carbonate, the oxidation number of oxygen is −2 in all three compounds, and calcium is +2 in calcium oxide and calcium carbonate. According to rule 3, carbon must be +4 in carbon dioxide and calcium carbonate.
Since there is no change in the oxidation numbers of the atoms during the reaction, this is not a redox reaction.
4.11:
Oxidation Numbers
In redox reactions, the transfer of electrons occurs between reacting species. Electron transfer is described by a hypothetical number called the oxidation number (or oxidation state). It represents the effective charge of an atom or element, which is assigned using a set of rules.
Oxidation Number (Oxidation State)
In the case of an ionic compound, oxidation numbers are assigned based on the number of electrons transferred between reacting species. For example, in the formation of calcium chloride (CaCl2), calcium loses two valence electrons, and the two chlorine atoms gain one electron each. In CaCl2, calcium’s oxidation state is +2, and each chlorine’s oxidation state is −1.
In the case of covalent compounds, electrons are not gained or lost but instead are shared between the atoms. The atom with a greater attraction for electrons pulls the shared pair more strongly. Reactions involving covalent compounds are identified as redox by applying the concept of oxidation number to track electron movements. Oxidation states help us easily identify the species being oxidized and reduced in redox reactions.
The Rules for Assigning Oxidation Number
Oxidation numbers can be positive, negative, or zero. They are assigned based on the following rules:
- All free elements have an oxidation number zero. The elements could be monoatomic, diatomic, or polyatomic.
- In a compound, group 1A elements (all alkali metals) have an oxidation number of +1, while group 2A elements (all alkaline earth metals) have an oxidation number of +2.
- Halogens usually have an oxidation number of −1, except in their compounds with oxygen, where they have a positive oxidation state.
Fluorine is the most electronegative element. It has a −1 oxidation state in all its compounds. - For monoatomic ions, the oxidation number is the same as the charge on the ion.
- Oxygen always has an oxidation number of −2, except in peroxides, where its oxidation number is −1.
- Hydrogen has an oxidation state of +1 with nonmetals and −1 with metals.
- The sum of the oxidation number for a neutral compound is zero, while for a polyatomic ion, it is equal to the charge on the ion.
This text is adapted from Openstax, Chemistry 2e, Section 4.2: Classifying Chemical Reactions.