Can sodium undergo displacement reaction why

No, in aqueous solution. In the molten state, yes.

First of all, potassium is more reactive than sodium, so displacement cannot occur.

In addition, even metal salts that are weaker than sodium cannot be replaced.

For example, if sodium is added to an aqueous solution of copper ions, the sodium will first interact with the water molecules.

reaction, sodium hydroxide is generated.

It then reacts with copper ions to form copper hydroxide precipitates. It will not be replaced with copper ions to form copper element.

If in the molten state, displacement can occur as long as the temperature is right.

For example, the industrial production of potassium metal is at 850 degrees Celsius.

Sodium is used to reduce molten potassium chloride.

Equation: Na+KCl=NaCl+K (gas symbol) Because the boiling point of sodium is 881 degrees Celsius, and the boiling point of potassium is 759 degrees Celsius, at 850 degrees, sodium is liquid and potassium is gaseous.

If you study chemical equilibrium, you know that potassium vapor escapes the reaction and shifts the equilibrium to the right.

This does not mean that sodium is more active than potassium, it is just that the conditions are too special.

Yes, for example, in the reaction between sodium and water, sodium displaces the hydrogen in the water: 2Na + 2H2O = 2NaOH + H2, which is also the only substitution reaction about sodium in middle school chemistry.

Yes, sodium reacts with water to produce sodium hydroxide and hydrogen gas, which is sodium that displaces hydrogen in water.

The reaction between sodium and water belongs to the redox reaction, because the valency of the element changes during the reaction, the valency of sodium element is high, and the valency of hydrogen element decreases is also a ...... of displacement reactionIn the reaction, an elemental substance (sodium) and a compound (water) react to form another elemental (hydrogen) and another compound (sodium hydroxide). Phenomena in which sodium reacts with water: heating, deflagration, and luminescence.

1 How sodium was discovered.

After Volt invented the battery in the early 19th century, chemists from all over the world have successfully used batteries to split water. David Davy, a British chemist, has been working tirelessly on the use of batteries to decompose various substances. He wanted to use batteries to break down caustic potassium into oxygen and an unknown "base", because chemists at the time considered caustic to be an oxide.

He first experimented with a saturated solution of caustic potassium (potassium hydroxide), but the results were the same as electrolysis of water, only hydrogen and oxygen were obtained. Later, he changed the experimental method, electrolyzed molten caustic potassium, and small beads with metallic luster, similar to mercury, appeared on the cathode, some of the beads immediately burned and occurred, forming a bright flame, and some beads did not burn, but the surface was darkened and covered with a white film.

He threw the tiny metal particle into the water, and immediately flames erupted, leaping rapidly on the surface of the water, making a stabbing sound. In this way, David discovered the metal potassium in 1807, and a few days later, he obtained it from electrolytic sodium carbonate.

The elemental reacts with the compound to form another elemental and compound, which is the displacement reaction 2Na+2H2O=2NaOH+H2 which satisfies the above definition.

Summary. Hello, dear, why sodium can't replace the metal, because: usually sodium can't replace the metal from the salt solution, if the salt is in a molten state, sodium can replace the less active metal The salt solution is water, the amount of water molecules is much greater than the salt ions, the water molecules surround the electrolyzed metal cations, when sodium is put into the water The first thing sodium comes into contact with is the water molecules, so the sodium will react with the water, and eventually it cannot be replaced When the salt melts, the electrostatic force between the ions is released, Sodium can easily displace some metal salts except for extremely reactive elements.

Why can't sodium be displaced?

Sodium reacts with copper sulfate solution, there is less water in copper sulfate solution, more sodium, more copper sulfate, in this case, why can't sodium replace copper sulfate?

Hello, dear, why sodium can't replace the metal, because: usually sodium can't replace the metal from the salt solution, if the salt is in a molten state, sodium can replace the less active metal The salt solution is water, the amount of water molecules is much greater than the salt ions, the water molecules surround the electrolyzed metal cations, when sodium is put into the water The first thing sodium comes into contact with is the water molecules, so the sodium will react with the water, and eventually it cannot be replaced When the salt melts, the electrostatic force between the ions is released, Sodium can easily displace some metal salts except for extremely reactive elements.

Because copper sulfate contains a small amount of water, sodium reacts directly with water, and if it is in a molten state, it can be replaced.

So copper sulfate, why can't it react with sodium?

Na is put into CuSO4 solution and reacted with water first. Because the activity of Na is too strong, the outer electrons are very easy to lose, because in the aqueous solution, no matter how high the concentration of CuSO4 is, it is far lower than the amount of water, and Na is put into the solution, because its density is lower than that of water, so Na floats on the water, before the water contact, there is no contact with Cu2+, the reaction generates NaOH, resulting in an increase in the concentration of OH, and it combines with Cu2+ to form a blue flocculent precipitate.

That's why.

It is difficult to explain this in middle school chemistry, in fact, the replacement of sodium with water and salt, and the reaction of direct current electrolysis of molten sodium salt are all redox reactions, and the oxidation of metal cations after potential sequence hydrogen is indeed stronger than that of hydrogen ions, but this is only for standard electrode potential. Whether the actual redox reaction can be carried out is closely related to the effective concentration and activity of each ion in the solution, and the electrode potential will also change accordingly. Under the action of sodium and salt solution at room temperature and pressure, the reaction trend of sodium and hydrogen ions and metal cations is very large, the presence of a large amount of solvent water makes sodium and hydrogen ions can be fully contacted and reduced, and the strong exothermic melting of sodium in the reaction makes the reaction speed with water further accelerated, and the metal cations are quickly precipitated by the caustic soda generated before they have time to be reduced to elemental matter.

However, due to the high temperature non-aqueous liquid phase of the melted sodium salt in DC electrolysis, the cathode is discharged and reduced in strict accordance with the order of the oxidation strength of each cation. Strictly speaking, the two reactions of sodium reduction of hydrogen ions and metal cations are competing reactions in aqueous solution, which are thermodynamically feasible, but in fact, more kinetic factors such as reaction rate and energy change effect determine the final product.

When sodium reacts with a salt solution, the reaction between sodium and water is earlier than the reaction between sodium and salt solution, therefore, sodium reacts with water to form sodium hydroxide and hydrogen. When sodium hydroxide reacts with salt solution, it needs to generate precipitate, water or gas, which belongs to metathesis, and there are only metal compounds after the reaction, and there is no way to replace the metal element.

You learn this part, sodium reacts with water because sodium is highly reducible, and it reacts when it comes into contact with water in solution, so it cannot replace metal. The electrons gained by metal ions are its oxidizing properties.

Because Na is the main group of alkali metal elements, it is more active.

It reacts easily with water.

Of course, this is only theoretical.

Chemistry is idealized in many cases.

In fact, in the real reaction, the displacement reaction also exists, but it is weak, and the idealized ideal is lost, you are talking about the discharge order, and it cannot be confused with redox ability, after all, many have special cases = =

If there's something wrong, don't spray me, wow, I'm only a sophomore in high school = = poof.

I don't think it has anything to do with the oxidation of metals here, and although it is true that the oxidation of hydrogen ions is weaker than the ions that follow hydrogen ions, water is a molecule and there are no hydrogen ions.

It is natural that sodium reacts with water first in a salt solution, but I don't know why.

Sodium is a very reactive metal that reacts with oxygen in the air to form sodium oxide; Under heating conditions, sodium peroxide will be formed with oxygen; When it reacts violently with water, sodium hydroxide and hydrogen gas are generated, and if copper sulfate is taken as an example, then the sodium hydroxide produced will react with copper sulfate to form copper hydroxide precipitate and sodium sulfate. In this process, the reaction of sodium and water will release a large amount of heat, and copper hydroxide may decompose into copper oxide and water when heated.

Hope it helps you!