NEET > Physical Chemistry for NEET > Redox Reactions & Oxidation Numbers
Redox Reactions & Oxidation Numbers Video Lecture - Physical Chemistry for NEET
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FAQs on Redox Reactions & Oxidation Numbers Video Lecture - Physical Chemistry for NEET
| 1. What are redox reactions? |  |
Ans. Redox reactions, also known as oxidation-reduction reactions, are chemical reactions that involve the transfer of electrons between reactant species. In these reactions, one reactant is oxidized (loses electrons) while another reactant is reduced (gains electrons).
| 2. How can oxidation numbers be determined in a chemical compound? | |
Ans. To determine oxidation numbers, we assign hypothetical charges to each atom in a compound. The rules for assigning oxidation numbers include:
- The oxidation number of an element in its pure form is always 0.
- In a compound, the sum of oxidation numbers must equal the overall charge.
- Oxygen is typically assigned an oxidation number of -2, except in peroxides where it is -1.
- Hydrogen is typically assigned an oxidation number of +1, except in metal hydrides where it is -1.
| 3. What is the significance of oxidation numbers in redox reactions? | |
Ans. Oxidation numbers play a crucial role in determining which species is being oxidized and which is being reduced in a redox reaction. By comparing the changes in oxidation numbers, we can identify the transfer of electrons and determine the overall direction of the reaction.
| 4. Can an element have multiple oxidation numbers in different compounds? | |
Ans. Yes, an element can have multiple oxidation numbers in different compounds. For example, in nitrogen compounds, nitrogen can have oxidation numbers ranging from -3 (in ammonia, NH3) to +5 (in nitric acid, HNO3). The specific oxidation number depends on the compound and its chemical environment.
| 5. How can redox reactions be balanced using oxidation numbers? | |
Ans. Redox reactions can be balanced by assigning oxidation numbers to each species involved and then balancing the changes in oxidation numbers. The number of electrons gained by the reduced species must equal the number of electrons lost by the oxidized species. This balance can be achieved by adjusting coefficients in the chemical equation to ensure the conservation of both mass and charge.
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