How is the term "oxidation state" defined?

The oxidation state is defined as the charge an atom would have if all bonds were ionic. This concept is crucial in understanding redox reactions and the behavior of elements in different chemical environments. When considering a compound, if we imagine that all bonding electrons are completely transferred to the more electronegative atom, the resulting charge on the atom is its oxidation state.

This definition helps to assess how electrons are being used or transferred in chemical reactions, allowing chemists to keep track of electron flow and to manipulate oxidation and reduction processes effectively. This understanding is fundamental when balancing redox reactions and determining the reactivity of different substances in various chemical conditions.

The other definitions provided do not accurately capture the essence of oxidation state. For instance, while the number of electrons an atom can gain or lose is relevant to its reactivity, it does not define how oxidation state is calculated. Similarly, the total number of protons in an atom relates to atomic number rather than oxidation state, and the relative mass of an atom compared to carbon-12 pertains to atomic mass, not chemical behavior.