Redox Problems in the third year of high school A question about redox reactions

The oxidation and reduction properties between metals and non-metals are generally not compared.

However, there will still be strengths and weaknesses, such as: the mn element in potassium permanganate has stronger oxidation than oxygen (potassium permanganate produces oxygen, and the strength of Johnson and Johnson can be judged).

However, not all metal elements are more oxidized than non-metals, such as the oxidation of MN in potassium permanganate just now is not stronger than that of fluorine, and the oxidation and reduction of ionic substances will generally change due to the acidity and alkalinity in the solution, and there is really no certain law.

In general, you can cite a few reactions to make a judgment. For example, if the reducibility of ag and cl- in the question, you can consider whether the reaction 2ag + cl2 = 2agcl will occur to judge, this reaction seems to occur, then according to the principle of strong and weak, the reducibility of ag is stronger than that of cl-.

However, not all substances can be compared in this way, and this method has limitations, but generally speaking, those that cannot be compared by this method will not appear in the exam.

Hope mine is helpful to you.

This is generally not the case, and can only be compared in the same type of substance, such as the same metal or the same non-metal.

The reducibility of the same metal is in order from high to low:

k,ca,na,mg，al，zn，fe，se，pb，（h）,cu，hg，ag，pt，au

The oxidation of the same non-metals is in order from high to low:

f,o,cl，br，i，s,p,c,si，（h).

If we really want to compare the reducibility of ag and cl- in this way, we can only discuss it in the specific reaction equations.

It is judged by whether it can gain or lose electrons. The available electrons are reducible, and the opposite is oxidation. To give you a formula: high (increased valency) loss (loss of electrons) oxygen (oxidizing), low to return.

Reducibility refers to the increase in valency and the loss of electrons in itself, which is called a reducing agent.

In addition to the one with the metal active type on the back, you also have to look at the periodic table of the same period, the stronger the left, the weaker the right, and the stronger the down.

But I still look at the experience of doing the question, and if I do more, I can reflect it at a glance.

What is this, it is obvious that the reduction of Cl- is strong, Ag is quite stable, and the reduction is very weak, the so-called "2AG+Cl2=2AGCl" is an impossible reaction, and it must be based on facts. To judge its strength by reaction, we can take oxygen or potassium permanganate (or manganese dioxide) as an example, and it can be said that Cl- is oxidized to chlorine, but AG cannot be oxidized. Therefore, CL-reducibility is strong, I hope to understand.

ag, the reducibility of metals is not generally stronger than that of non-metals.

Just memorize it. I won't list them.

I think your chemical formula should be written incorrectly, it should be 6HCl (concentrated) + KCLO3=KCl+3Cl2 +3H2O

Non-crossing regularity:

When the redox reaction occurs between different valence states of the same element, ** should be reduced, and the low price should be increased, and they mostly become the same valence state, and it is impossible to cross the phenomenon. This law is often used to determine the relationship between quantities, indicating the direction and number of electron transfers, for example, 6HCl (concentrated) + KCLO3 = KCl + 3Cl2 + 3H2O

The first question is selected, because there is no change in the valence of any element before and after the reaction, which is the criterion for judging whether it is redox or not.

The second question is that water only acts as an oxidant (a), water only acts as a reducing agent (d), water acts as an oxidant and a reducing agent (c), and water is neither an oxidant nor a reducing agent (b). The method of judging this problem is that if the hydrogen ions become hydrogen atoms before and after the reaction, that is, the hydrogen ions are reduced (the valency of hydrogen is reduced), then water is an oxidant, and in the same way, if the oxygen atoms become oxygen atoms, that is, the oxygen ions are oxidized, then the water is the reducing agent.

The strength of the oxidizing ability is the strength of the ability to obtain e or the bias of the shared electron pair.

2Fe(3+)+2i(-)2Fe(2+)+I2Fe3+ is converted into Fe2+ I2 as an oxidation product, which is reducible.

2Fe(2+)+Cl2==2Fe(3+)+2Cl(-)Fe2+ loses e to Fe3+

Order of strength: Cl2>Fe3+>i2

cl2>fe3+>i2

The strength of oxidation ability is the strength of the ability to gain and lose electrons.