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Why is sodium metal stored immersed under kerosene oil?
To prevent evaporation
To prevent reaction with moisture and oxygen in air
To prevent electric shocks
To enhance its lustre
To prevent reaction with moisture and oxygen in air
Sodium is an extremely reactive alkali metal that reacts vigorously with moisture and oxygen present in the atmosphere. Storing it under kerosene acts as a protective barrier to prevent contact with these reactive agents, thereby avoiding accidental fires or degradation.
Sodium is an extremely reactive alkali metal that reacts vigorously with moisture and oxygen present in the atmosphere. Storing it under kerosene acts as a protective barrier to prevent contact with these reactive agents, thereby avoiding accidental fires or degradation.
Think of it like an airtight food container; just as we seal food to prevent it from going bad due to air exposure, we submerge sodium in kerosene to stop it from 'spoiling' via chemical reaction.
K-S (Kerosene-Sodium) = Keep Safe.
2Na+O2тАЛтЖТNa2тАЛO2тАЛ тАФ Reaction with oxygen to form sodium peroxide
2Na+2H2тАЛOтЖТ2NaOH+H2тАЛтЖС тАФ Reaction with moisture to form sodium hydroxide and hydrogen gas
Sodium has a very low ionization energy and readily loses its valence electron to oxygen and water. The chemical reaction with water is highly exothermic and produces flammable hydrogen gas: 2Na+2H2тАЛOтЖТ2NaOH+H2тАЛ+Heat. Because kerosene is an unreactive hydrocarbon that is less dense than sodium, it forms an airtight seal, preventing oxidation and hydrolysis.
Sodium belongs to Group 1 of the periodic table, known as Alkali Metals.
Alkali metals are highly reactive due to their single valence electron.
Kerosene is used because it does not react with sodium and prevents atmospheric contact.
Sodium metal is soft enough to be cut with a knife.
Prevents hazardous runaway exothermic reactions
Preserves the metallic luster of sodium
Ensures safety during laboratory storage
Kerosene is flammable and poses a secondary fire risk
Requires careful disposal to avoid environmental contamination
Used in chemical laboratories for synthesis
Historical use in sodium-vapor lamps (alloyed form)
Sodium has an atomic number of 11.
Option A is incorrect because sodium has a high boiling point and does not evaporate at room temperature.
Option C is incorrect as kerosene is an electrical insulator and not used to prevent shocks.
Option D is incorrect as the primary concern is chemical stability, not aesthetic appearance.
B is correct тАФ Sodium is highly reactive with moisture and oxygen; kerosene serves as an inert, protective shield to prevent contact with these atmospheric substances.
Always remember that all Group 1 elements (Lithium, Sodium, Potassium) are kept in oil or inert atmospheres; for exams, focus on the reaction with H2тАЛO yielding H2тАЛ gas.
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