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

Oxidation Numbers

Oxidation numbers are numerical values assigned to atoms in a molecule or ion that indicate the degree of oxidation or electron loss typically relative to their elemental state. They are essential for keeping track of electrons in complex reactions and serve as a tool to determine which atoms are oxidized or reduced during a redox process.

Oxidation

Oxidation is the process in which a chemical species loses electrons, leading to an increase in its oxidation number. This loss of electrons occurs simultaneously with the reduction of another species, and tracking these changes through oxidation numbers is key to understanding redox reactions.

Reduction

Reduction is the process in which a chemical species gains electrons, resulting in a decrease in its oxidation number. This gain is accompanied by the oxidation of a different species, and identifying these changes through assigned oxidation states helps clarify the electron transfer during redox reactions.

Redox Reactions

Redox reactions are chemical processes that involve simultaneous oxidation and reduction where one species loses electrons while another gains electrons. By assigning oxidation numbers to the atoms involved, one can determine which species undergo changes in electron count, providing clarity on how and where the reaction proceeds.

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