How to turn chemical equations into ionic equations

Chemical equationsWrittenIonic equationsProcess:

Of course, after familiarity, you can directly write the ion equation Cu2+ +Fe — Fe2+ Cu, and then trim

The front is the method, and the back is the example. Once you are familiar with it, you can write it out at a glance, and it is recommended to do more questions.

How do you write the ionic equation between sodium sulfate solution and sodium chloride solution?

An ionic equation, i.e., a formula that represents an ionic reaction with the symbol of the ions that actually participate in the reaction.

Refers to the reaction in which soluble substances are detachable. The ionic equation not only represents a certain reaction between certain substances, but also represents the same type of ionic reaction.

For example, H++OH-=H2O can represent the neutralization of many strong acids and bases.

Whether a variety of ions can coexist in the same solution in large quantities can be summed up as: one color, two sexes, three special, and four reactions. To write an ionic equation, you must first determine whether the reaction is an ionic reaction or not.

For example, the reaction of acetic acid with sodium carbonate is an ionic reaction, and the reaction of acetic acid with ethanol to produce ethyl acetate and water is not an ionic reaction.

Iron oxide + 6 hydrogen ions 2 iron ions + 3 water molecules.

All three do not react.

Iron is already the highest valence, but it is specifically oxidized, and oxygen in the air does not react.

If this aspect is weak, you can practice more, generally just start to learn is a little unaccustomed, but you can first write out the chemical equation, and then split it into ion equations, but also pay attention to some substances can not be disassembled (such as elemental, weak acid, weak alkali, insoluble salt), and then check the trim is OK, if you want to learn the ion equation well, you must learn the chemical equation, this is the foundation, learn it well, chemistry is not difficult, come on.

Elemental substances do not need to be dismantled Strong acids and strong bases should be dismantled into ionic form, weak acids and weak bases should not be dismantled, soluble salts should be dismantled, insoluble should not be dismantled, and oxides should not be dismantled.

It's all about feeling and it's just a matter of practice.

Elemental quality is left alone.

Strong acids and alkalis must be dismantled into the form of ion collapse.

Weak acids and weak alkalis are not dismantled.

The soluble salt of the shirt should be dismantled.

The insoluble ones are not dismantled.

Oxide is not disassembled.

Step 1: Dismantle the substances that are easily soluble in water and easy to ionize into ionic form Step 2: Delete the ions on both sides of the equation that do not participate in the reaction Step 3:

Check that the elements and charges on both sides of the equation are conserved and "split" is key. Insoluble substances, oxides, weak acids, weak bases, volatile gases and other substances cannot be disassembled when writing ion equations, and chemical formulas must be written.

1.Disassemble what can be disassembled, and keep what cannot be disassembled.

2.About going to things that are on the left and right.

Write the notes of the teacher's lecture clearly! Don't get distracted in class...

Write equations.

Disassemble into ions. The same ions before and after are deleted.

All that's left is the ionic equation.

Write only the reactions of the ions.

As long as there is an ionization equilibrium in the product, it is written as reversible. Otherwise, write equally.

Only reactants that are weak electrolytes are not disassembled. Only those products that are weaker than the reactants should not be dismantled (including insoluble substances), because the metathesis reaction needs to produce gas, produce substances that are difficult to ionize, or produce substances that are difficult to dissolve in water, and if they are disassembled, it means that the reaction has not been carried out.

By the way, water is generally seen as non-ionizing, so there is no need to write reversible.

First, write the correct chemical equation, disassemble the ions that can be divided into ions, and delete the same ions or substances on both sides of the equal sign.

This should have a specific topic. You have to remember some atomic clusters.

Basic steps. 1.Write.

Clearly write out the chemical equation about the reaction.

2.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.

Slightly soluble strong electrolytes should be seen to see if they exist mainly in the form of free ions, for example, calcium hydroxide in lime water is written as an ion symbol, and calcium hydroxide in lime milk is expressed by 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.

3.Delete Remove ions on both sides of the equation that do not participate in the reaction.

4.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.

For example: CaCO3+2HCl=CaCl2+H2O+CO2 CaCO3+2H+=Ca2++H2O+CO2

The ionic equation is a reaction equation described by the ionic symbol plus the chemical formula.

In the reaction in solution, the strong electrolyte should be written in the form of ions, for example, CaCl2 should be written as Ca2+ and 2Cl-, beginners can write the chemical equation first, and then dismantle the strong electrolyte, and turn the chemical equation into an ion equation (note that the weak electrolyte and precipitation should never be disassembled).Take the reaction of calcium chloride and silver nitrate as an example:

The chemical equation CaCl2 + 2agNO3 ==== 2AGCl +CA(NO3)2, disassemble CA2+ +2Cl- +2AG+ +2NO3- ***** 2AGCl +Ca2+ +2NO3-, the same ions on both sides are about to be removed, and then the coefficient before throwing away the remaining three substances is AG + Cl- ==== AGCL, and it is completed.

sodium sulfate and barium chloride; so4(2-) ba2+ ==== baso4 ↓

Hydrochloric acid and sodium hydroxide: H+ +OH- === H2O