HEY GUYS :-
HOW TO IDENTITY THE COMPOUND WEATHER IT'S OXIDIZING AGENT OR REDUCING AGENT BY JUST LOOKING AT ITS COMPOUND NAME❗❗❗
---------> DETAIL ANS NEEDED
Answers
What is reducing agent and oxidizing agent?
Oxidizing and Reducing Agents. An oxidizing agent, or oxidant, gains electrons and is reduced in a chemical reaction. ... A reducing agent is typically in one of its lower possible oxidation states, and is known as the electron donor. A reducing agent is oxidized, because it loses electrons in the redox reaction
So to identify an oxidizing agent, simply look at the oxidation number of an atom before and after the reaction. If the oxidation number is greater in the product, then it lost electrons and the substance was oxidized. If the oxidation number is less, then it gained electrons and was reduced.
Reducing Agents
A redox reaction occurs when an electron is transferred from one substance to another.
Oxydation Reduction Ion Image
An oxidation reaction is a reaction the takes an electron from one substance. A reduction reaction is a reaction that gives an electron to a substance. A redox reaction is a reaction in which one substance gives up an electron and another substance takes that electron. I know it is strange that 'oxidation' means 'giving up' and 'reduction' means 'taking in,' but remember that an electron is negatively charged, so everything is kind of backwards. To give up an electron means to become more positively charged. To take in an electron means becoming more negatively charged.
An oxidizing agent is the substance that causes the oxidation in another substance. Common oxidizing agents include oxygen, hydrogen peroxide and halogens. A reducing agent is a substance that causes another substance to reduce. So to identify an oxidizing agent, simply look at the oxidation number of an atom before and after the reaction. If the oxidation number is greater in the product, then it lost electrons and the substance was oxidized. If the oxidation number is less, then it gained electrons and was reduced. The substance that is reduced in a reaction is the oxidizing agent because it gains electrons. The substance that is oxidized in a reaction is the reducing agent because it lost electrons
H2 S + O2 = SO2 + H2 O
1. Identify the reactants and the products and assign oxidation numbers.
null..
2. Write and balance the half-reactions.
Note that sulfur is changing from a -2 oxidation number to a +4 oxidation number, so it had to lose six electrons. -2 + (-4) = -6.
Oxygen is changing from a zero oxidation number to a -2, gaining two electrons. 0 + (-2) = -2. Since free oxygen atoms travel in pairs, the actual number of electrons gained is -4.
▶For finding oxidising agents and reducing agents you have to see the compound clearly.
You have to see the left hand side of the compound and if another side is gaining the oxygen then it oxidation and if it is losing the oxygen the it is reduction.
▶Eg: 2ZnO + C - - - - - - >2Zn + CO2
Oxidizing agent = ZnO
Reducing agent = C