Identify what is being oxidized and reduced in this redox...

Identify what is being oxidized and reduced in this redox equation by assigning oxidation numbers to the atoms.
$$
2 \mathrm{KrF}_{2}+2 \mathrm{H}_{2} \mathrm{O} \rightarrow 2 \mathrm{Kr}+4 \mathrm{HF}+\mathrm{O}_{2}
$$

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Key Concepts

Redox Reactions

Redox reactions, or oxidation-reduction reactions, encompass processes in which electrons are transferred from one species to another. Assigning oxidation numbers to atoms allows chemists to identify which species are oxidized (lose electrons) and which are reduced (gain electrons), offering a systematic approach to analyzing these reactions.

Reduction

Reduction is the gain of electrons by an atom, ion, or molecule, leading to a decrease in its oxidation number. As the counterpart to oxidation, reduction occurs simultaneously with oxidation in redox reactions, ensuring that the overall electron balance is maintained.

Oxidation Numbers

Oxidation numbers (or oxidation states) are values assigned to atoms in a compound that indicate the degree of oxidation (loss of electrons) of an atom. They are essential for determining which atoms undergo changes during a redox reaction by comparing their initial and final states.

Oxidation

Oxidation is the process in which an atom, ion, or molecule loses electrons, resulting in an increase in its oxidation number. It typically involves the transfer of electrons to another species and is fundamental to understanding how redox reactions proceed.

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