Determine the oxidation number of the boldface element in...

Determine the oxidation number of the boldface element in these ions.
$$
\begin{array}{ll}{\text { a. IO} _{4}^{-}} & {\text { c. } B_{4} 0_{7}^{2-}} \\ {\text { b. MnO} _{4}-} & {\text { d. NH} _{2}-}\end{array}
$$

Key Concepts

Oxidation Numbers

Oxidation numbers, also known as oxidation states, are assigned to atoms in a compound or ion to indicate the number of electrons lost or gained by an atom in comparison to its elemental form. They are a useful tool for keeping track of electron transfer in redox reactions and for understanding the bonding and structure of chemical species.

Rules for Assigning Oxidation Numbers

There is a set of agreed?upon rules for assigning oxidation numbers. These typically include that the oxidation number for a pure element is zero, oxygen is usually assigned a value of -2 (with some exceptions), hydrogen is usually +1 (except in certain hydrides), and the sum of the oxidation numbers in a neutral compound must be zero, while in a polyatomic ion it equals the overall charge of the ion.

Polyatomic Ions and Charge Balancing

When dealing with polyatomic ions, the total of the oxidation numbers for all the atoms must equal the ion’s net charge. This concept is crucial for calculating unknown oxidation numbers within the group of atoms, ensuring that the oxidation numbers reflect the overall electric charge of the ion.

Electronegativity and Electron Distribution

The assignment of oxidation numbers is influenced by the relative electronegativities of the atoms involved. Atoms with higher electronegativity are more likely to attract electrons and are often assigned negative oxidation states, while atoms with lower electronegativity generally lose electrons and are assigned positive oxidation numbers. This helps in predicting reaction pathways and the direction of electron flow during chemical processes.

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