Can t you write ionization equations for non electrolytes?

The answer is yes: no.

Compounds that do not conduct electricity in either the molten state or in aqueous solution. This concept is relative to electrolytes. Non-electrolytes are compounds that are typically covalently bonded and do not ionize in aqueous solutions.

With the exception of carboxylic acids and their salts, phenols, and amines, most organic compounds are non-electrolytes, such as sucrose, glycerol, ethanol, etc. Among inorganic compounds, only some non-metallic halides and all non-metallic oxides are non-electrolytes.

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.

To use an analogy; In the normal state, it is the yin and yang fish of Tai Chi that are together.

When the electrolyte is in the water, the yin and yang fish are separated, and they can move regularly under the action of electric current.

Non-electrolytes are yin and yang fish that do not separate in the water, and the current does not work for them.

Is there a white spot?

Non-electrolytes cannot be ionized, and of course the ionization equation cannot be written.

Yes, non-electrolytes are compounds that are typically covalently bonded and do not ionize in aqueous solutions. (Quoted from Encyclopedia).

NaCl Anode 2Cl- -2E-==Cl2 Cathode 2H+ +2E-==H2 Total Reaction Formula: 2NaCl+2H2O= Energized = 2NaOH+Cl2 +H2 CuSO4 Anode: 2H2O -4E-==4H+ +O2 Cathode:

Cu2+ +2E-==Cu Total Reaction Formula: 2CuSO4+2H2O= Energized = 2Cu+O2 +2H2SO4 CuCl2 Anode: 2Cl- -2E-==Cl2 Cathode:

Cu2+ +2E-==Cu Total Reaction Formula: CuCl2=Energized=Cu+Cl2 HCl Anode: 2Cl- -2E-==Cl2 Cathode:

2H+ +2E-==H2 Total Reaction Formula: 2HCl=Energized=H2 +Cl2 Na2SO4 Anode: 4OH- -4E-=2H2O+O2 Cathode:

2H+ +2E-=H2 Total Reaction Formula: 2H2O=Energized=2H2 +O2 AgnO3 Anode: 2H2O-4E-===4H+ +O2 Cathode:

AG+ +E-==AG Total Reaction Formula: 4AGnO3+2H2O=Energized = 4AG+4HNO3+O2 KBR Anode: 2BR- -2E-==BR Cathode:

2H+ +2E-==H2 Total Reaction Formula: 2KBR+2H2O=Energized=BR2 +H2 +2KOH H2SO4 Anode: 4OH- -4E-=2H2O+O2 Cathode:

2H+ +2E-=H2 Total Reaction Formula: 2H2O=Energized=2H2 +O2 NaOH Anode: 4OH- -4E- =2H2O+ O2 Cathode:

2H+ +2E- =H2 Total Reaction Formula: 2H2O=Energized=2H2 +O2 Note: The electrolysis reaction does not play the precipitation symbol, because the electrolysis is an adsorption type!

Note: Rough as pure hand-hitting! No copy!

The total ion reaction equation is simpler than the total chemical equation of Yanqi, so the total chemical equation is played. (The ion equation is to use the anode equation + cathode equation) if necessary, please hi me.

C(H+)=C(OH-)+C(NH3·H2O) The H+ in the solution comes from two parts, one is the ionization of water, and the concentration is equal to the concentration of OH-.

The other part is the hydrolysis of NH4+, and the concentration is equal to the concentration of NH3·H2O.

NH4+ +H2O= Reversible=NH3·H2O+H+ Charge Conservation: The positive charge of all cation bands in the solution is equal to the negative charge of all anion bands.

Conservation of materials: Some ions in the solution can be hydrolyzed or ionized, and the total number of some atoms in these particles does not change, and the ratio of the number of certain atoms does not change.

Conservation of protons: The amount of H+ and Oh- substances ionized by water is equal.

The ionization equation is: NaCl=Na++Cl-, CH3CoonH4=CH3COO-+NH4+.

The strong electrolyte is completely ionized in aqueous solution, and the ionization equation is written with the symbol "=" when writing the ionization equation for poorly soluble cherry cavity and slightly soluble strong electrolyte"="Some electrolytes are written differently depending on the conditions.

1. The strong electrolyte is completely ionized in the aqueous solution, and the symbol "=" is used when writing the ionization equation, for example: NaCl=Na++Cl-, CH3CoonH4=CH3COO-+NH4+.

2. Use the symbol "=" when writing the ionization equation of poorly soluble and slightly soluble strong electrolytes "" "For example:

baso4=ba2++so42-，ca（oh）2=ca2++2oh-，baso4（s）⇌ba2+（aq）+so42-（aq），ca（oh）2（s）⇌ca2+（aq）+2oh-（aq）。

3. Some electrolytes are written differently due to different conditions. For example, when melting, khso4=k++hso4-; In aqueous solution: KhSO4=K++H++SO42-.

4. The weak electrolyte is partially ionized in aqueous solution, and the ionization equation is written with the symbol " "For example, CH3COOH CH3COO-+H+, NH3·H2O NH4++OH-.

5. The ionization of multiple weak acids in aqueous solution is carried out step by step, and it is required to write the ionization equation step by step, and there are several levels of ionization equation for several yuan acids. For example, H2CO3 H++HCO3-, HCO3- H++CO32-.

The ionization of multiple weak bases in aqueous solution is more complicated, so the ionization equation of multiple weak bases is generally written in one step, but still the spine hail shirt is still marked with the symbol " "For example, Cu(OH)2 Cu2++2OH-.

6. The acid salt of weak acid is a strong electrolyte, and the first step in water is to completely ionize cations and acid ions of weak acid, and the acid ions of weak acid can be ionized, and it is a reversible process. For example, the ionization equation for NaHCO3 in aqueous solution is: NaHCO3=Na++HCO3-, HCO3- H++CO32-.

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.

1. All you mean "ion equation", right?

People use the ion equation to represent the ionic reactions that take place in an aqueous solution, and only those strongly soluble electrolytes can be broken down into ions.

For oxides, most of the non-metallic oxides are non-electrolytes, so they are not dismantled; Metal oxides, such as some Cuo, Fe2O3, etc., are insoluble in water, so they are not disassembled, or they are put into water and immediately react with water to form corresponding bases such as Na2O, CaO, etc., without the process of ionization (in aqueous solution, O2- ions cannot exist stably), so they cannot be disassembled.

In fact, what needs to be disassembled into ions, that is, soluble strong electrolytes, only includes strong acids, strong bases and soluble salts, and the rest are not disassembled.

A: Not necessarily.

Sensitive:

1) Ionic compounds are all electrolytes.

including insoluble ionic compounds such as caCO3 and so on).

2) Covalent compounds.

Some are electrolytic bridge sedans, such as HCl, H2S, H2O, CH3COOH and so on.

Some are non-electrolytes, such as CO2, SO2, SO3, NO2, NO4, CH4, and so on.

The ionic compound must be an electrolyte. Early conversely, electrolytes are not necessarily ionic compounds, such as HCl. The previous one is wrong, and it is suspected that Cu(OH)2 should belong to the alkali of insoluble celery, which also belongs to strong electrolytes.