Is it true that ionic compounds must be all strong electrolytes ?

Not all ionic compounds are strong electrolytes, this statement is not true. For example, lead acetate is an ionic compound, but it is a weak electrolyte.

Ionic compounds are compounds made up of cations and anions. When active metals (such as sodium, potassium, calcium, magnesium, etc.) and active nonmetals (such as fluorine, chlorine, oxygen, sulfur, etc.) are combined with each other, the active metals lose electrons to form positively charged cations (such as Na+, K+, Ca2+, Mg2+, etc.), and active nonmetals obtain electrons to form negatively charged anions (such as F-, Cl-, O2-, S2-, etc.), and cations and anions form ionic compounds by electrostatic action. For example, sodium chloride is an ionic compound composed of positively charged sodium ions (Na+) and negatively charged chloride ions (Cl-).

In ionic compounds, the total number of positive charges carried by cations is equal to the total number of negative charges carried by anions, and the whole compound is electrically neutral.

Electrolytes can generally be divided into strong electrolytes and weak electrolytes, and the conductivity of the two varies greatly. Strong electrolytes can be considered to exist entirely in the form of ions in solution, i.e. there are no "molecules" of the electrolyte (at least in the range of dilute solutions). As the concentration increases, the electrostatic force between the ions increases, causing the ion mobility to decrease, and the equivalent conductance also decreases.

For weak electrolytes, its main form of existence in solution is molecule, its ionization degree is very small, so the number of ions is very small, and the electrostatic effect is also very small, it can be considered that the ion mobility basically does not change with concentration, so the reason for the rapid decline of equivalent conductance with the increase of concentration is mainly the rapid decrease in ionization.

1.Not all ionic compounds are strong electrolytes, for example, lead acetate is an ionic compound, but it is a weak electrolyte.

Strong electrolytes are compounds that are completely ionized in an aqueous solution or in the molten state, while weak electrolytes are compounds that are not completely ionized. The strength of the electrolyte is independent of whether it is an ionic compound or not.

2.Ionic compounds can conduct electricity when melted, and they break ionic bonds, but not all of them, that is, they may not all be ionized, depending on the situation. In addition, there are ionic compounds that do not have a molten state, such as NaHCO3

When the ionic compound is dissolved, it is a strong electrolyte that is fully ionized.

3.A solution of a substance in ionization equilibrium, such as ammonia. Exist.

NH3·H2O <==> NH4+ +OH-, when diluted with water, the ionization equilibrium shifts to the right, and the number of NH4+, OH- in the solution increases, but the concentration decreases. This is the dilution effect of ionization equilibrium, which needs to be explained by the equilibrium constant. The limit method is available here.

There is a beaker of ammonia, there is ionization equilibrium, NH3·H2O is partially ionized, and it is now poured into a lake, then it can be considered that this ammonia water has been completely ionized (ionization balance is negligible).

The electrolyte is ionized by the action of water molecules in the solution, and the ions exist as hydrated ions, so it can also be considered that the addition of water increases the water and its force, which can be explained according to the principle of equilibrium movement.

False (CH3OO)2Pb is an ionic compound but whether a weak electrolyte ionic compound is a strong electrolyte or a weak electrolyte is related to the polarity of the anion.

High school exams, that's right. Just remember it.

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According to the query operation help, strong acids, strong bases, and most salts are strong electrolytes, while ionic compounds generally refer to substances containing active metal cations, and substances containing active metal cations are generally strong electrolytes.

Ionic compounds are compounds made up of cations and anions. When reactive metals (such as sodium, potassium, calcium, magnesium, etc.) and active nonmetals (such as fluorine, chlorine, oxygen, sulfur, etc.) are combined with each other, the active metals lose their acres and return to electrons to form positively charged cations (such as Na+, K+, Ca2+, Mg2+, etc.), and the active non-metals are electrons to form negatively charged anions (such as F-, Cl-, O2-, S2-, etc.), and cations and anions form ionic compounds by electrostatic action.

The ionic compound must be an electrolyte because the ionic compound conducts electricity in its molten state.

However, ionic compounds are not necessarily strong electrolytes, such as HGCL2 and (CH3COO)2PB are weak electrolytes.

Electrolytes are compounds that are dissolved in aqueous solution or can be trapped and conductive in a stupid molten state. According to the degree of ionization, it can be divided into strong electrolyte and weak electrolyte, almost all ionized is strong electrolyte, and only a small part of the row hood is ionized weak electrolyte.

A compound composed of an anion and an anion. When reactive metals (such as sodium, potassium, calcium, magnesium, etc.) and reactive nonmetals (such as fluorine, chlorine, oxygen, sulfur, etc.) are combined with each other, reactive metals lose electrons to form positively charged cations (such as Na+, K+, Ca2+, Mg2+, etc.), and reactive nonmetals obtain electrons to form anions with negative rolling and rapid charges, and cations and anions form ionic compounds by electrostatic action.

Electrolytes are compounds that are able to conduct electricity when dissolved in an aqueous solution or in a molten state. 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. Electrolytes are substances that are bound by ionic bonds or polar covalent bonds.

Strong electrolytes are not necessarily ionic compounds, weak electrolytes are all covalent compounds.

In the case of AlCl3, which is a strong electrolyte, it is also a special covalent compound. Therefore, strong electrolytes are not necessarily ionic compounds.

Weak electrolytes are all covalent compounds. Because ionic compounds are all strong electrolytes, weak electrolytes are all covalent compounds. However, covalent compounds are not necessarily weak electrolytes, but can also be strong electrolytes, such as HCl.

An electrolyte that completely ionizes ions in an aqueous solution or in a molten state is called a strong electrolyte. Degree of ionization: Complete ionization, no ionization equilibrium. Solute particles: only ions.

Examples: strong acids HCl, HNO3, H2SO4, HBR, Hi, HCO4, etc.; Strong alkalis KOH, NaOH, BA(OH)2, SR(OH)2, Ca(OH)2, etc.; Salt for the vast majority.

Weak electrolytes are compounds that can partially dissociate into ions. It usually contains four types of substances: weak acid, weak alkali, water and a few salts.

NH4OH is an ionic compound which is incorrect and is a covalent compound. Ionic compounds are strong electrolytes that have nothing to do with solubility, weak acids and bases.

H2O is a weak electrolyte.

Not necessarily, NH4OH is a weak electrolyte, but an ionic compound.

HCl is a covalent compound, but a strong electrolyte.

Not all of them, for example, sodium hydroxide is a strong electrolyte, and aluminum hydroxide is a weak electrolyte.