A compound is soluble in water, but its aqueous solution does not conduct electricity, then the comp

Electrolyte. Electrolytes are compounds that are capable of conducting electricity in an aqueous solution or in a molten state, such as acids, bases, and salts. Compounds that cannot conduct electricity under the above circumstances are called non-electrolytes, such as sucrose, alcohol, etc.

To determine whether a compound is an electrolyte, it is not only based on whether it conducts electricity in aqueous solution, but also needs to further investigate its crystal structure and the properties of chemical bonds. For example, to determine whether barium sulfate, calcium carbonate, and iron hydroxide are electrolytes. Barium sulfate is poorly soluble in water (solubility in water at 20 is g), the ion concentration in the solution is small, its aqueous solution is not conductive, and appears to be a non-electrolyte.

However, the small fraction of barium sulfate dissolved in water is almost completely ionized (20 The degree of ionization of the barium sulfate saturated solution is. Thus, barium sulfate is an electrolyte. Calcium carbonate and barium sulfate have a similar situation and are also electrolytes.

From a structural point of view, for other insoluble salts, as long as they are ionic compounds or strong polar covalent compounds, although they are insoluble, they are also electrolytes.

The case of iron hydroxide is more complicated, the chemical bond between Fe3+ and OH- is covalent, and its solubility is smaller than that of barium sulfate (solubility in water at 20 is g); A small part of the part that falls on water may form colloids, and the rest can also be ionized into ions. But iron hydroxide is also an electrolyte.

To determine whether the oxide is an electrolyte, a specific analysis should also be made. Non-metallic oxides such as SO2, SO3, P2O5, CO2, etc., which are covalent compounds that do not conduct electricity in liquid state, are not electrolytes. Some oxides are not electrolytes even if they conduct electricity in aqueous solutions.

Because these oxides react with water to form new substances that can conduct electricity, what conducts electricity in the solution is not the original oxide, such as SO2 itself cannot be ionized, but it reacts with water to form sulfurous acid, which is the electrolyte. Metal oxides such as Na2O, MGO, CaO, Al2O3, etc., are ionic compounds that are capable of conducting electricity in the molten state and are therefore electrolytes.

It can be seen that electrolytes include ionic or strongly polar covalent compounds; Non-electrolytes include weakly polar or non-polar covalent compounds. The aqueous solution of electrolytes conducts electricity because the electrolyte can be dissociated into ions. As for whether a substance can be ionized in water, it is determined by its structure.

Therefore, the identification of electrolytes from non-electrolytes by the structure of matter is the essence of the problem.

In addition, some substances that can conduct electricity, such as copper and aluminum, are not electrolytes. Because they are not electrically conductive compounds, they are elemental and do not meet the definition of electrolyte.

Electrolytes are defined as compounds that conduct electricity in a water-soluble or molten state; Compounds that do not conduct electricity when dissolved in water or in a molten state.

Sucrose is soluble in water, but the aqueous solution does not conduct electricity, so it is not an electrolyte.

Carbon dioxide is soluble in water, and the aqueous solution conducts electricity, but it is not carbon dioxide that conducts electricity, so it is a non-electrolyte.

Chlorine is soluble in water and conducts electricity, but it is elemental and is neither an electrolyte nor a non-electrolyte.

If the compound is dissolved in the solution and only dissolves and conducts electricity without chemical change, then it is an electrolyte, but if it is due to a chemical change, such as carbon dioxide dissolved in water to produce carbonic acid to conduct electricity, the electrolyte is carbonic acid, not carbon dioxide, and carbon dioxide is a non-electrolyte.

In addition, when describing electrolytes, it is important to say that compounds, such as salt water conducts electricity, and the electrolyte is sodium chloride instead of salt water, which is a mixture, which is neither an electrolyte nor a non-electrolyte. Elemental substances, like mixtures, are neither electrolytes nor non-electrolytes.

Counter-example: Carbon dioxide dissolves in water to conduct electricity, but carbon dioxide is not an electrolyte.

So a certain compound could be carbon dioxide

It should be noted that gases that are generally soluble in water and can conduct electricity cannot be regarded as electrolytes, because it is not the gas that can conduct electricity in the end, but the gas has a chemical reaction with hydrogen ions in the water to make the aqueous solution conductive

Therefore, this kind of compound that can conduct electricity after being dissolved in water is actually not the compound itself in water, such as carbon dioxide, when it is dissolved in water, it is combined with hydrogen ions to become carbonic acid It is actually carbonic acid that conducts electricity, not carbon dioxide

Hydraphytes are compounds that can conduct electricity in a molten state or in an aqueous solution.

Key point analysis: 1 The word "or" means that as long as it meets one (or two), it can be.

2. Electrically disturbing the positive desolation must be a chemical repentance.

The non-electrolyte is not conductive in both melted and dissolved in water.

It is only certain that the aqueous solution does not conduct electricity, and it cannot be determined that it does not conduct electricity when melted.

Like AGCL, it has very little solubility in water and does not conduct electricity, but it is an electrolyte.

A certain compound is easily soluble in water, but its bridge aqueous solution does not conduct electricity", so this compound is solid or gaseous.

Solid compounds that are easily soluble in water, but their aqueous solutions are not conductive, and they are generally organic crystals, which cannot be salts.

Solid compounds that are easily soluble in water, but their aqueous solutions do not conduct electricity are generally NH3SO3, etc. So the answer is definitely non-electrolyte.

The example you gave "as long as it conducts electricity in its molten state" does not fit the question, can you give a specific example that meets the requirements of "a compound that is easily soluble in water, but its aqueous solution does not conduct electricity"?

The idea of answering the question is very important.

The examination of the question should not be messy.

Be clear-minded.

The counter-examples given should be within the scope of the question.

1) When melted or dissolved, the compound that can conduct electricity is called an electrolyte--- which is called an electrolyte!

2) Compounds that do not conduct electricity when melted or dissolved --- called non-noisy electrolytes--- correct!