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Why sodium is a reducing agent

In a chemical compound classification reaction, sodium is the reducing agent (it furnishes electrons), and Chlorine is the oxidizing agent (it consumes electrons). The most common reducing agents are metals, which tend to lose electrons in their reactions with nonmetals. At first sight, lithium having a high value of ionization energy amongst alkali metals acts as the strongest reducing agent in solution. Hydrogen acts as a reducing agent because it donates its electrons to fluorine, which allows fluorine to be reduced. Reducing agents, also known as oxidizing agents, include sodium bisulfite, sodium hydrosulfite, and ferrous sulfate. They are typically used to remove harmful substances from wastewater, such as ozone, hydrogen peroxide, Chlorine, and biological contaminants. Disinfection. After the water has been filtered, water treatment plants may add one or more chemical disinfectants (such as Chlorine, chloramine, or chlorine dioxide) to kill any remaining parasites, bacteria, or viruses.

Hence, Chlorine is not a reducing agent. But Nitrogen can have oxidation states from −3 to +5. So it is in between the maximum and minimum oxidation state. So it can either get reduced or oxidized, depending on the conditions. So it can act both as oxidizing and reducing agent. Chlorine is a strong oxidizing agent. Its effectiveness depends on temperature, residual Chlorine, and reaction time. Before discharging ballast water it should be dechlorinated by using sulfur dioxide which reacts with residual Chlorine to form chlorine ions. Strong reducing agents are electropositive elements that can lose electrons easily in chemical reactions. Strong reducing agents are weak oxidizing agents. If you are looking for high quality, high purity and cost-effective water-reducing agent, or if you require the latest price of water-reducing agent, please feel free to email contact mis-asia.

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