Since the ionic equation is detached from the chemical equation, isn t the ionic equation redundant?

Chemical equations are relatively intuitive. Let you beginners recognize the reaction substance.

And the ion equation is based on the essence. Describe the ions that react in the reaction. These ions do not coexist.

Everything else coexists. Unchanged ions.

Embodies the essence of the chemical reaction.

Because in solution, some substances do not react, such as Na+ and Cl-, they do react in the chemical equation, but in fact they are only ions, they are not combined, and only after combining to become gases, precipitates or weak electrolytes will they separate from the solute in solution.

If you have any questions, just ask them as soon as possible.

The ionic equation expresses all the chemical reactions of the same class, while the chemical equation can only represent a certain chemical reaction, and the ionic reaction reflects the essence of some chemical reactions.

The ion equation reflects the essence of the chemical reaction, and those ions and acids that do not react do not change in the solution and do not need to be written. Writing ion equations is simple, easy to understand, convenient, and can reflect the essence. In addition, the same ion equation can represent different reactions, which is convenient for studying similar reactions and finding patterns.

Hope it helps.

No, the ion equation provides a clearer picture of the reactions between ions, changes in valency, and oxides and reductants. There are functions that ordinary reflection equations do not have.

The ionic equation reflects the essence of chemical change.

Shenma effect?! When you take the exam, if you can not write chemical equations, you will not write chemical equations, and if you use ion equations to calculate or something, chemical equations will be troublesome.

Regularity features. 1.Weak electrolytes cannot be disassembled. For example: water,Acetic acid, etc. (weak acid, weak base).

2.Oxides are basically not disassembled, and CO2 is not an ionic compound.

Iron oxide is insoluble and precipitates, so it can't be disassembled, in short, you remember, when you see oxide, it's best not to dismantle it.

3.Gases, elemental matter, you're right, don't think about dismantling these things when you see them, because they are all molecular structures or atomic structures.

Since it is to write ionic compounds, only soluble ions that can move freely in solution can be dismantled, typical of which are chlorination and nitric acid.

Wait. Weak electrolytes can not be disassembled, such as: water, acetic acid, etc. (weak acid, weak alkali), oxides can not be disassembled, CO2, iron oxide can not be disassembled, gas, elemental substances can not be disassembled, precipitation can not be disassembled, detachable has strong electrolytes that are easily soluble in water, such as strong acids and strong alkalis can be dissolved in water salts.

Absolutely not disassembled: water precipitation, gas oxides, elemental complexes such as ferric thiocyanide, lead acetate, non-electrolytes (such as ethyl alcohol), weak electrolytes (such as acetate ammonia monohydrate).

To be dismantled: Soluble salts other than ferric thiocyanide and lead acetate, dilute sulfuric acid, nitric acid, hydrobromide, hydroiodic acid, hydrobromide, iodic acid, alkali formed by alkali metals below sodium on the periodic table, clear lime water.

Concentrated sulfuric acid does not dismantle hydrofluoric acid, does not dismantle lime milk, and weak alkali does not dismantle (but sometimes depending on the situation, for example, the sodium bicarbonate in Hou-style alkali is not dismantled, because it is a precipitation).

1.Weak electrolytes cannot be disassembled, such as: water, acetic acid, etc. (weak acid, weak base).

2.Oxide basically can't be disassembled, CO2 is not an ionic compound, iron oxide is insoluble, precipitate one, so it can't be disassembled, in short, you remember, when you see oxide, it's best not to dismantle it

3.Gas, elemental, you're right, don't think about dismantling these things when you see them, because they are all molecular or atomic structures, since you want to write ionic compounds, only soluble ions that can move freely in solution can be dismantled. Typical ones are sodium chloride, nitric acid, and so on.

Weak electrolytes, precipitation, gases cannot be disassembled (excluding insoluble electrolytes dissolved equilibrium).

Weak electrolytes are substances that cannot be completely ionized in water, such as weak acids, weak bases, etc.

Precipitates such as calcium carbonate, barium sulfate. Weak acid and weak alkali. The claw machine can't write equations and wants to cry.

Detachable:

1) Strong acids, such as hydrochloric acid, sulfuric acid, nitric acid, perchloric acid, hydrobromic acid, hydroiodic acid, chloric acid, etc. 2) Strong alkalis, such as koh, naoh, ba(oh)2, and ca(oh)2 can be removed when clarifying lime water, and lime milk cannot be detached.

3) Most soluble salts, except for Hg2Cl2, PB(CH3CoO)2 are non-electrolytes and cannot be dismantled.

Non-detachable: 1) Elemental.

2) Non-electrolytes, such as gaseous compounds.

3) Weak electrolytes, such as water, weak alkali, weak acid.

4) Insoluble substances, such as insoluble salts and metal oxides.

1.weak acid, medium strong acid as reactants; Weak bases appear in ionic equations and are always written as chemical formulas.

2.Substances that are insoluble in water, water, gases, and elemental substances that appear in the ionic equation are all written as chemical formulas.

3.If the microlyble is used as a reactant, emphasize its dissolved side, treat it as a soluble, and write it as an ion symbol (pay attention to the size of the concentration, if the solid or suspension participates in the reaction, it will be written as a chemical formula); If it is used as a product, emphasize its insoluble side and write it as a chemical formula.

4.Reactions between solids (non-molten state), reactions between concentrated sulfuric acid and solids, do not write ion equations, and use ordinary chemical reaction equations to express the reactions.

Ions that do not actually participate in the reaction are removed.

For example, HCl+NaOH=NaCl+H20

Na[+] and Cl[-] do not participate in the reaction and still exist in ionic form.

So delete it and write it as h[+]oh[-]h2o

Another example is kclo3+6HCl=KCL+3Cl2+3H2O, where k[+] does not participate in the reaction, and 1 Cl[-] does not participate in the reaction.

Therefore, delete and write as clo3[-]6h[+]5cl[-]3cl2+3h20

Write out the chemical equation first, and then dismantle everything that can be dismantled into ions, including soluble strong electrolytes (strong acids, strong bases, soluble salts), all of which are represented by ions, like insoluble substances (including weak electrolytes), gases, water, do not disassemble, retain! , and slightly soluble, depending on the situation.

Again, remember, if an ion has on both sides of the equal sign, it is considered an ion that does not participate in the reaction, and it should be deleted, (if it is on both sides, it should be deleted), and then check whether the mass is conserved, whether the charge is conserved, and it's OK!

Like the first equation, manganese ions are produced by manganese dioxide, manganese dioxide is insoluble and does not dismantle, and it is soluble after generating manganese chloride, so it should be dismantled, but manganese exists in the form of manganese dioxide before the reaction, there are no ions, and ions are produced after the reaction.

The same is true for the others, if the following ions are removed, the mass is not conserved.

The metathesis reaction is essentially the process of combining barium ions and sulfate ions to form barium sulfate precipitate, which has nothing to do with copper ions and chloride ions, you just replace the reaction with sodium sulfate and barium nitrate, and the ion equation is the same.

Mn2+ is not a precipitation, but MnO2 is, you can't let the mn in MnO2 disappear after the reaction, in the reaction of CuSO4 + BACl2 = CuCl2 + BaSO4, CuSO4 and BACL2 are ionized into Cu2+ and SO42- and Ba2+ and Cl-, and then Ba2+ and SO42- react into BaSO4 precipitation, and Cu2+ and Cl-, are still in an ionic state, and they are still floating in water. So they don't participate in the ionic reaction.

Chemical equations for sodium bicarbonate and sodium hydroxide.

NaHCO3 + NaOH = Na2CO3 + H2O sodium bicarbonate and sodium hydroxide ion equations.

hco3-oh-co3

h2o here.

It doesn't matter if there is an excess of sodium bicarbonate or an excess of sodium hydroxide, the equation is the same.

Basic steps.

Write clearly the chemical equation about the reaction.

Soluble strong electrolytes (strong acids, strong bases, soluble salts) are all represented by ion symbols, and other insoluble substances. Substances that are difficult to ionize, gases, oxides, water, etc., are still expressed by chemical formulas.

For slightly soluble substances, they usually exist in ionic form (in solution) in ionic reactions, but if they are in turbid liquids, the complete chemical formula needs to be written, for example, calcium hydroxide in lime water is written as an ion symbol, and calcium hydroxide in lime milk is expressed as a chemical formula. Due to the presence of mainly sulfuric acid molecules, the chemical formula is also written. Concentrated nitric acid and hydrochloric acid are completely ionized, so they are written as ionic.

Remove the same ions and molecules on both sides of the equation.

Check whether the number of atoms and the number of charges on both sides of the formula are equal and whether they are balanced, and whether the stoichiometric number of the obtained formula is the simplest integer ratio, if not, it should be reduced to the simplest integer ratio.

Strong acid, strong alkali, soluble salt, detachable. Others cannot be dismantled.

Complete dissolution of completely ionized written ions, precipitation, weak electrolyte, gas written chemical formula.

Strong electrolytes should be disassembled, and weak electrolytes should not be dismantled.