Chemistry, how do you distinguish electrolytes from non electrolytes? Thank you

Electrolytes and non-electrolytes:

Difference: Whether it conducts electricity in an aqueous solution or in a molten state.

Identification: Most acids and alkalis are electrolytes, and non-electrolytes are commonly alcohol, sucrose, carbon dioxide, sulfur dioxide and other non-metallic oxides.

Note: Both electrolytes and non-electrolytes are chemical compounds, such as chlorine, which can conduct electricity when dissolved in water, and Cu, which can also conduct electricity, but neither of them are electrolytes nor non-electrolytes.

Strong electrolytes: strong acids, strong bases, most salts (except lead acetate) Strong acids: 6 types: hydrochloric acid (mixture) sulfuric acid.

Nitric acid. Phosphoric acid (moderately strong acid) hydrobromic acid.

Hydroiodic acid. Perchloric acid.

Strong alkali: potassium hydroxide, barium hydroxide, sodium hydroxide, calcium hydroxide (medium and strong alkali), weak electrolyte: weak acid, weak alkali, a few salts.

Weak acids: hydrofluoric acid, acetic acid.

Wait. Weak bases: except for hydroxide (potassium, sodium.

Calcium. barium) and of course ammonia.

1. Electrolytes and non-electrolytes.

Electrolytes – aqueous solutions or compounds that conduct electricity in the melted state.

Non-electrolytes – compounds that do not conduct electricity, either in aqueous solution or in the melted state.

Discussion: Which of the following are electrolytes? Copper, sodium chloride solids, potassium nitrate solids, calcium carbonate solids, carbon dioxide.

Note: 1) Acids and bases are electrolytes.

2) Most metal oxides are electrolytes.

3) Water is an electrolyte.

4) Most non-metallic oxides are non-electrolytes.

5) Most of the organic matter is non-electrolyte.

Electrolytes vs. non-electrolytes.

The distinction between electrolytes and non-electrolytes is as follows:

Compounds that are capable of conducting electricity in an aqueous solution or in a molten state are called electrolytes. Compounds that are not capable of conducting electricity in both aqueous solution and in the molten state are called non-electrolytes.

1. Metals can conduct electricity, but they are not compounds, so metals are neither electrolytes nor non-electrolytes.

2. SO2 and NH3 are soluble in water and can conduct electricity, and conductive ions are ionized by H2SO3 and NH3·H2O, so SO2 and NH3 are not electrolytes. HCl, H2SO4, etc. are soluble in water and can conduct electricity, and conductive ions are ionized by themselves, so they are electrolytes. Acids, bases, and salts are electrolytes, and non-metal oxides are not electrolytes.

3. Active metal oxides, such as Na2O, Al2O3, etc., can conduct electricity in the molten state because they can ionize ions themselves, Al2O3 (melting) = 2Al3++3O2, which is an electrolyte.

4. The conductivity of the aqueous solution of refractory substances (such as caCO3, etc.) is very weak, but the molten state can conduct electricity, which is an electrolyte.

5. Most organic substances such as alcohol and sucrose are non-electrolytes.

6. Electrolytes do not necessarily conduct electricity. Strong alkali and salt plasma compounds cannot conduct electricity because they cannot move freely in the solid state, so they cannot conduct electricity, but they can conduct electricity in the molten state or when dissolved in water.

Acids in the solid or liquid state (molten state) have only molecules, no free-moving ions, so they do not conduct electricity, and in aqueous solutions, they are ionized by water molecules to produce free-moving ions, and can conduct electricity.

7. Non-conductive substances are not necessarily non-electrolytes, and substances that can conduct electricity are not necessarily electrolytes. Electrolytes, non-electrolytes refer to chemical compounds. O2 does not conduct electricity, iron and aluminum can conduct electricity, but they are neither electrolytes nor non-electrolytes.

8. The conductivity of the electrolyte solution is related to the concentration of ions in the solution and the amount of charge carried by the ions.

9. To judge whether the electrolyte is conductive, the key is to see whether the electrolyte is ionized, which produces free-moving ions, and also depends on the concentration of ions produced by ionization. For example, the solubility of CaCO3 in water is very small, and the ion concentration produced by ionization in water is very small, so its aqueous solution is considered to be non-conductive.

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.

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.

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.

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.