High School Chemistry Oxidation, Reductiveness, Acidity and Alkalinity Sorting?

I'm a chemistry teacher, and I'll tell you how to look at it, and I'll know it when I open your periodic table.

In the same period, from left to right, the elemental oxidation gradually increases, corresponding to the most ** oxide and hydride acidity increases, (except for HF acid, because F is the strongest oxidizing element).

In the same main group, from top to bottom, the elemental reducibility is gradually enhanced, the alkalinity of metal elements corresponding to oxides is enhanced, and the acidity of non-metallic elements is enhanced. The acidity of non-metallic element hydrides is enhanced (metal element hydrides are not examined).

In the periodic table, from left to right, the oxidation is enhanced, the reduction is weakened, and the hydrate corresponding to the most ** oxide is more acidic and the alkalinity is weakened. The elemental element at the leftmost end is the weakest, the most reducible, the most alkaline, and the weakest acidic. There is a verbal decision:

**Reduction of low-price oxidation, intermediate valence on both sides". For what you are talking about, it is necessary to refer to the specific reaction, sometimes acting as an oxidizing agent, sometimes acting as a reducing agent, which can be judged by the transfer of electrons. If you still don't understand, I'll tell you.

The higher the valence, the stronger the oxidation and the higher the acidity, so the oxidation of sulfur trioxide is higher than that of sulfur dioxide, and the acidity of sulfuric acid is stronger than that of sulfurous acid.

The lower the valence, the stronger the reduction and the weaker the acidity.

The most advanced state of sulfur can only be reduced, so it can only oxidize another substance, and the lowest valence state can only rise, so it can only reduce another substance, and the intermediate valence state depends on the strength of the oxidation and reduction of the reacting substance

It seems that there are summaries in the current reference books.

One. Non-metallic elemental oxidation: In general, the strong non-metallic nature of the element corresponds to the strong elemental oxidation.

For example: non-metallic F>Cl>Br>i>Sthen oxidizing F2>Cl2>Br2>I2>S

1.The non-metallic properties of the elements in the same period (horizontal, from left to right) increase, and the elemental oxidation increases.

Second Cycle: (Elemental Oxidation) N2S>Se>Te; (elemental non-metallic) o>s>se>te

Seventh main group: (elemental oxidizing) F2>Cl2> Br2>i2; (elemental non-metallic) f>cl>br>i

In addition, it should be noted that the non-metallic properties of oxygen are slightly stronger than those of chlorine; However, the oxidation of elemental matter is the opposite, oxidation (Cl2>O2), that is, chlorine is slightly more oxidizing than oxygen; However, ozone O3 is much more oxidizing than Cl2.

Two. Oxidation of metal cations:

The more oxidizing the metal is at the bottom of the order of activity.

Oxidizing strong) Ag > Hg2 > Cu2 >H > Pb2 > Sn2 >Fe2 >Zn2 >Al3 ...The oxidation is very weak).

The oxidation of Fe3 is between Hg2 and Cu2: Hg2 >Fe3 >Cu2

Three. The oxidation of the compound (you must look at the pH of the solution, the oxidation of the compound has a great relationship with the pH):

In general:

F2>>O3>> kmNO4 (H)>Cl2>K2Cr2O7(H)> mNO2>HNO3> concentrated H2SO4>H2O2>O2>Br2> AG>Fe3 >I2>Cu2 >H

The principle that the oxidation of the oxidant is stronger than the oxidation of the oxygen source product: nitric acid can oxidize ferric iron to ferric iron - the oxidation of nitric acid is greater than that of ferric; Chlorine can oxidize ferric to ferric - chlorine is more oxidizing than ferric; According to the periodic law, the oxidation (non-metallicness) of the element closer to the upper right corner is stronger, so the oxidation of chlorine is greater than that of nitric acid; Potassium permanganate and hydrogen peroxide can also oxidize ferric iron to ferric, so ferric is the weakest oxidizing; Because potassium permanganate has strong oxidizing properties, and can oxidize hydrogen peroxide, which in turn can oxidize chlorine; So to sum up, the oxidation is arranged from large to small:

Potassium permanganate, hydrogen peroxide, chlorine, nitric acid, and ferric iron. For all the elements, their reducibility is arranged from large to small as potassium, calcium, sodium, magnesium, aluminum, zinc, iron, tin, lead, (hydrogen) copper, mercury, silver, platinum, gold, ......The formal arrangement of the ions of these elements is the order of oxidation from small to large. That's my opinion, thank you!

There are several ways to compare the strength of oxidation.

Potassium permonate to nitric acid to chlorine to hydrogen peroxide to iron ions.

The oxidation of high school chemistry is not self-sufficient for these substances.

Nature sorted! Because to grasp the strength of the properties is nothing more than to judge the direction of the chemical reaction and the sequence of reactions, and for the oxidation of the above-mentioned oxidants, they are all highly oxidizing substances. Naturally, they can usually participate in redox reactions.

There are two orders that need to be mastered, namely: F2>O2>Cl2>Br2>Fe3+>I2>SO2>SAG+>Fe3+>Cu2+>H+>Fe2+>Zn2+>Al3+>Mg2+>Na+>Ca2+>K+

Potassium permanganate is the most ruthless, tribai valence iron is the most rubbish, and then nitric acid is more than chlorine (you can follow it.

The difficulty of the reaction between the two and the copper is judged by the final chlorine gas is greater than hydrogen peroxide. Let me tell you that the oxidation of matter cannot be arranged according to the oxidation of element atoms, because these elements present different valence states in matter, for example: oxygen is more oxidizing than chlorine, but water is not oxidizing!

On the contrary, chlorine is highly oxidizing! Therefore, the specific oxidation line of the discharged substance depends on the specific reaction, remember that the oxidation of the oxidant in the reaction is greater than the oxidation product! For example, in the landlord's question, chlorine is greater than ferric, because chlorine and ferric react to form ferric, of which chlorine is the oxidant ferric is the oxidation product, so chlorine is greater than ferric iron ......

Mainly according to the distribution of the periodic table.

From top to bottom, the reducibility is gradually enhanced, and the oxidation is gradually enhanced, and the internal general metal is strongly reducible, and the non-gold capacity is explicit oxidation.

However, the strength is not determined by the number of electrons gained and lost, but the difficulty of gaining and losing electrons has a law: potassium, calcium, sodium, magnesium, aluminum, zinc, iron, tin, lead, hydrogen, copper, mercury, silver, platinum, The reduction is weakened in turn, and the oxidation is increased in turn.

There are also more common tests for alkali metals and halogens.

Mainly according to the periodic law.

The most ** cation of the metal has no reducing property and the lowest price anion of the metal has no oxidizing property and has strong oxidizing properties, such as acidic potassium permanganate, hydrogen peroxide, chlorine, etc., which have strong reducing properties, such as (SO3)2- I- etc., I hope it will help you!

Common oxidation is more common.

f2>cl2>br2>fe3+>i2>s >so2kmno4>kclo3>mno2

Fe3+>Cu2+>H+>Fe2+>Zn2+concentrated HNo3> dilute Hno3

cl2>o2>s

Oxidation: K ca na mg al zn fe pb h cu fe ag ; Reducibility: S so i fe + br cl f.

Some common oxidants such as: KMNO4 (sulfuric acid acidification), potassium dichromate, ozone, chlorine, potassium chlorate, potassium hypochlorite, nitric acid, concentrated sulfuric acid, hydrogen peroxide, sodium peroxide, manganese dioxide, lead dioxide. Non-metallic elemental oxidation:

In general, the elements with strong non-metallic properties correspond to strong elemental oxidation. For example: non-metallic F>Cl>Br>i>S

then oxidizing F2>Cl2>Br2>I2>S1.

Common ionreducibility: S so i Fe + br Cl F.

Common ionic oxidation: k ca na mg al zn fe pb h cu fe ag .

Substances in the ** state are generally oxidizing, such as some non-metallic elemental O, Cl; Part** Metals, FE, MNO, etc. Substances in the low-valence state are generally reducible, such as some non-metallic anions Br, I, etc. Substances in the intermediate valence state are generally both reducing and oxidizing, such as tetravalent sulfur.

Common oxidants are substances that are easily reduced in chemical reactions.

1) Typical non-metallic elements such as F2, O2, Cl2, Br2, I2, S, etc. (their oxidation is basically the same as that of non-metallic activity).

2) ** compounds containing valence elements, such as KMNO4, KCLO3, H2SO4, HNO3, Mno2, etc.

3) Metal cations such as: Fe3+, Cu2+, (H+) (in the displacement reaction of metal with acid and salt solution, such as the reaction Fe CuSO4=Feso4 Cu, it is essentially Cu2+ ions oxidizing Fe atoms, Cu2+ as oxidizing agent, and Fe as reducing agent).

A common reducing agent is a substance in which volatile electrons are oxidized in a chemical reaction.

1) Typical metal elements such as: K, Ca, Na, MG, etc. (their reducibility is basically the same as that of metal activity).

2) Certain non-metallic elements and their compounds, such as: H2, C, CO.

3) The lowest valence compounds with valence elements, such as H2S, Hi, HBR, and HC

4) Non-metallic anions such as: S2-, I-, Br-, Cl-

1. From the order of metal activity: reducing K>GA>NA>MG>Al>ZN>Fe>SN>PB>(H)>Cu>Hg>AG>PT>Au [elemental, H is H2] Oxidation from strong to weak (large to small): Au>pt>Ag>Hg>Cu>(h)>Pb>SN>fezn>Al>mg>Na>Ga>K [ion] (Add the ion symbol to the above in reverse, note that the ion symbol is not good to input I didn't add, Be sure to add) 2, reductive:

Cl>br>Fe ion (+2 valence)> i [Except for Fe, the rest are elemental] Oxidation: Cl

Oxidation products, reducibility: reducing agent" reducing products such as, oxidation: Fe3+>Fe2+>Fe, reducibility:

The stronger the non-metallic property, the weaker the elemental reducibility. [There are also special circumstances, pay attention to summarizing and inductive memory] 5. Generally, acidic KMno4 and acidic K2CR2O7 are both strong oxidizing (much stronger than other substances), the former and the latter. 6. There will be hints or information in some questions, pay attention to reading the questions.

This is my small experience in high school for three years, I hope it will help you.

Volatile: hydrochloric acid, phosour sulfuric acid, hydrogen peroxide insoluble who: silicon dioxide, calcium carbonate, silver chloride.

In high school chemistry, oxidation is usually sorted according to the affinity of a substance for electrons in other substances. Here are some common substances sorted by oxidation:

1.Strong Oxidizing Agents: These substances are highly oxidizing and can easily get electrons. Typical strong oxidizing agents include:

Oxygen (O2).

Oxidants such as high concentration of hydrogen peroxide (H2O2), high concentration of perchloric acid (HCO4), etc.

2.Stronger oxidizing agents: These substances have high oxidizing properties but relatively high requirements for electrons. Typical of the stronger oxidant packet is missing:

Chlorine dioxide (CLO2).

High concentration of acidic potassium permanganate (KMNO4).

High concentration of perchlorous acid (HCOs).

High concentration of periodic acid (HIO4).

3.Medium Oxidants: These substances are moderately oxidizing and require a certain amount of energy to get electrons. Typical medium oxidants include:

Nitric oxide (NO).

Nitrous oxide (N2O4).

High concentration of nitric acid (HNO3).

4.Weak oxidants: These substances have low oxidation and require higher energy to obtain electrons. Typical weak oxidants include:

Sodium oxide (Na2O).

Calcium oxide (CAO).

Zinc oxide (ZNO).

It should be noted that this is only a general concept of oxidation ranking, and the actual situation will be affected by other factors.

I hope mine can help you and have a great day!

High and high oxidation strength sequential sorting formula: common ion reduction: S2-SO3(2-) I-Fe2+ br- Cl- F-; Common ionic oxidation:

k+ ＜ca2+ ＜na+ ＜mg2+ ＜al3+＜ zn2+＜ fe2+ ＜pb2+＜h+＜cu2+ ＜fe3+ ＜ag+；Strength and weakness law: oxidation, oxidation products; In reduction, reducing products; Valence law: the element is in the most advanced state and only has oxidation; The element is in the lowest valence state and is only reductive; It is in the intermediate valence state, which is both oxidizing and reducing; Law of Conservation:

The number of electrons gained by the oxidizing agent is equal to the number of electrons lost by the reducing agent. Strength and weakness law: oxidation, oxidation products; In reduction, reducing products; Valence Law:

The element is in the most ** state so that the hail limb is only oxidized; The element is in the lowest valence state and is only reductive; It is in the intermediate valence state, which is both oxygen-repentant and reductive; Conservation law: Oxidizing agents get electrons'The number is equal to the number of electrons lost by the reducing agent.