How to distinguish between electrolytes and non electrolytes, please thank you

It is not necessarily the electrolyte that can conduct electricity to judge whether a compound is an electrolyte, and it is not only based on whether it conducts electricity in aqueous solution, but also needs to further investigate its crystal structure and the nature of chemical bonds. For example, to determine whether barium sulfate, calcium carbonate, and iron hydroxide are electrolytes. Barium sulfate is insoluble in water, the ion concentration in the solution is very small, and its aqueous solution is not conductive and appears to be a non-electrolyte.

However, molten barium sulfate can conduct electricity. 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- has covalent properties, and its solubility is smaller than that of barium sulfate; A small part of the water-soluble part 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 [1] ; 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 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.

What is the way to distinguish between electrolytes and non-electrolytes?

As all metals are neither electrolytes nor non-electrolytes. Because they are not chemical compounds, they do not meet the definition of electrolytes. Here's how to judge:

1. Whether it can be ionized (essential difference): Electrolyte is a compound that can be ionized under certain conditions, while non-electrolyte cannot be ionized.

2. Common substance categories: electrolytes are generally acids, alkalis, salts, typical metal oxides and some non-metal hydrides. Non-electrolytes are typically non-metallic oxides, some nonmetallic hydrides, and most organic compounds.

3. Compound category: The electrolyte is ionic compounds and some covalent compounds, and the non-electrolytes are all covalent compounds.

Thing or teasing. 1. Distinguish according to the concept:

Electrolyte: A compound that conducts electricity in an aqueous solution or in a molten state.

Non-electrolyte: Compounds that do not conduct electricity in both aqueous solution and in the molten state.

Note: 1) Both electrolytes and non-electrolyte groups must be compounds.

2) Both electrolytes and non-electrolytes must be pure.

3) The conductivity of the electrolyte solution must be self-ionized, producing free-moving ions.

4) There is no definite relationship between electrolyte and conductivity.

2. Judge according to the type of substance.

1.Substances that belong to electrolytes.

1) acids, such as HCl, H2SO4, HNO3, CH3COOH, H2CO3, etc.;

2) Alkalis, such as NaOH, Ba(OH)2, NH3·H2O, etc.;

3) Most salts, such as NaCl, Na2SO4, BaSO4, etc.;

4) oxides of active metals, such as Na2O, Al2O3, etc.;

5) Water. 2.Substances that are non-electrolytes.

1) Non-metallic oxides, such as CO2, SO2, SO3, etc.;

2) Cover most of the organic matter, such as ethanol, sucrose, CH4, etc.;

3) A few non-metallic hydrides, such as NH3.

1. Electrolytes:

1) Definition: A compound that conducts electricity in an aqueous solution or in a molten state. (2) Range: acids, alkalis, salts, water, active metal oxides. Precautions.

The electrolyte must be a chemical compound. (Must be pure first) Compounds are not necessarily electrolytes.

The electrolyte must be conductive: in aqueous solution or in a molten state. The electrolyte must be a compound capable of ionizing on its own.

2. Non-electrolytes:

Compounds that do not conduct electricity in aqueous solution or in the molten state. (2) Scope: non-metallic oxides (such as: CO2, SO2), some non-metallic hydrides (such as: NH3), most organic compounds (such as alcohol, sucrose), etc

1) Electrolytes, non-electrolytes should be compounds. (First of all, purity) (2) Elemental and mixtures are neither electrolytes nor non-electrolytes.

Classification of electrolytes and non-electrolytes:

Both electrolytes and non-electrolytes are subordinate compounds, and the difference is whether they are conductive or non-conductive in an aqueous solution or in a molten state.

Common electrolytes are: acids, alkalis, salts, active metal oxides, etc.;

Common non-electrolytes are: non-metallic oxides and most organic compounds.

Strong electrolytes: 1. Strong acids: HCl

H2SO4 sulfuric acid.

HNO3 nitric acid.

HBR hydrobromic acid.

HI hydroiodic acid.

HCO4 is high in envy chloric acid.

2. Strong alkali: NaOH

KOHBA(OH)2 barium hydroxide.

Ca(OH)2 calcium hydroxide.

3. Most salt: The salt you see in high school is all strong electrolytes.

Metal compounds: a

Oxide: calcium oxide cao

Sodium oxide Na2O

Magnesium oxide MGO

Oxidation of Al2O3

Zinc oxide. zno

Oxide iron Feo

Iron oxide Fe2O3

Copper oxide cuo

Mercury oxide HGO

Silver oxide AG2O

B. Peroxide compound: sodium peroxide Na2O2

c. Metal carbide: calcium carbide CaC2

d. Metal sulfides: calcium sulfide Cas2

Ferrous sulfide FeS2

Weak electrolyte: 1. Weak acid: H2CO3 carbonate

Sulfite H2SO3

Acetate CH3COOH

H2S hydrosulfate

Hydrofluoric acid HF silicic acid H2SiO3

Orthosilicate H3SiO4

All organic acids.

2. Weak alkali: ammonia monohydrate.

All metal hydroxide r(OH) except for strong alkalis

3. Water H2O is also a weak electrolyte.

Non-electrolyte: 1. Non-metallic oxide: carbon dioxide.

Sulfur dioxide. Carbon monoxide.

Sulfur trioxide cracking.

Nitrogen dioxide. Nitric oxide.

2. Most organic matter: methane.

Ethanol. Cane sugar.

Except for organic acids and organic salts).

3. Non-metallic compounds: ammonia.

Judgment method: 1. Electrolyte is a compound that can be ionized under certain conditions, while non-electrolyte cannot be ionized.

2. Common substance categories: electrolytes are generally acids, alkalis, salts, typical metal oxides and some non-metal hydrides. Non-electrolytes are typically non-metallic oxides, some non-metallic hydrogen-positives, and the vast majority of organic compounds.

Some covalent compounds can also conduct electricity in aqueous solutions, but there are also solid electrolytes that are conductive** related to the migration of ions in the crystal lattice.

According to the degree of ionization, it can be divided into strong electrolyte and weak electrolyte, almost all of which are ionized by strong electrolytes, and only a small part of which are ionized by weak electrolytes.