identify the substance that is is the oxidizing agent and the substance that is the reducing agent
Oxidized species: lost electrons
Oxidizing agent: gained electrons. Normally, it is the species which is reduced.
The reducing agent is what is oxidized and the oxidizing agent is the reduced.
To identify the oxidizing agent and the reducing agent in a chemical reaction, you need to determine which substance gains electrons (reducing agent) and which substance loses electrons (oxidizing agent). Here's how you can do it:
1. Write down the balanced equation for the chemical reaction.
2. Identify the atoms that change their oxidation state. In other words, look for atoms that either lose or gain electrons.
3. Assign oxidation numbers to each atom in the reactants and products. The oxidation number is a positive or negative number representing the electron distribution around an atom.
4. Compare the oxidation numbers of the changing atoms in the reactants and products.
- If an atom in a reactant has a higher oxidation state and decreases its oxidation number in the product, it is the reducing agent.
- If an atom in a reactant has a lower oxidation state and increases its oxidation number in the product, it is the oxidizing agent.
- The reducing agent is oxidized (loses electrons), and the oxidizing agent is reduced (gains electrons).
For example, let's consider the reaction between hydrogen gas (H2) and oxygen gas (O2) to produce water (H2O):
2H2 + O2 -> 2H2O
In this reaction, hydrogen gas (H2) is oxidized to form water (H2O), while oxygen gas (O2) is reduced to water (H2O). Therefore, hydrogen gas (H2) acts as the reducing agent and oxygen gas (O2) acts as the oxidizing agent.
Remember, these assignments are based on the concept of oxidation and reduction, and the species involved as oxidizing or reducing agents can vary depending on the specific reaction you are considering.