N_(2)+3H_(2)arrow 2NH_(3) For the equation, what is the: (Remember, LEO says GER) element being oxidized square element being reduced square oxidizing agent square reducing agent square : Nitrogen : Hydrogen

To determine the elements being oxidized and reduced, as well as the oxidizing and reducing agents, we need to analyze the changes in oxidation states of the elements involved in the reaction.<br /><br />Given the balanced chemical equation:<br />$N_{2} + 3H_{2} \rightarrow 2NH_{3}$<br /><br />1. Element being oxidized:<br /> The element being oxidized is the one that loses electrons during the reaction. In this case, hydrogen (H) is being oxidized because its oxidation state increases from 0 to +1 in the product NH3.<br /><br />2. Element being reduced:<br /> The element being reduced is the one that gains electrons during the reaction. In this case, nitrogen (N) is being reduced because its oxidation state decreases from 0 to -3 in the product NH3.<br /><br />3. Oxidizing agent:<br /> The oxidizing agent is the substance that accepts electrons and gets reduced. In this reaction, nitrogen (N) is the oxidizing agent because it accepts electrons from hydrogen (H) and gets reduced.<br /><br />4. Reducing agent:<br /> The reducing agent is the substance that donates electrons and gets oxidized. In this reaction, hydrogen (H) is the reducing agent because it donates electrons to nitrogen (N) and gets oxidized.<br /><br />Therefore, the answers are:<br />- Element being oxidized: Hydrogen (H)<br />- Element being reduced: Nitrogen (N)<br />- Oxidizing agent: Nitrogen (N)<br />- Reducing agent: Hydrogen (H)