Are there any conditions for metals non metals to react with oxygen

1.(1) Chemical reaction. The reaction produces a salt or alkali.

If the corresponding alkali is soluble in water, it can react with water, and if the corresponding alkali is insoluble in water, it does not react with water. For example: Na2O + H2O == 2NaOH

k2o + h2o == 2koh ,cao + h2o = ca(oh)2 ,bao + h2o == ba(oh)2

It can't react with water.

Metal oxides react with non-metal oxides to form salts.

For example: Na2O + CO2 == Na2CO3CAoAo + SiO2 === Casio3 (condition is high temperature) 2), reduction reaction: CO+CuO=Cu+CO2 (condition is heating) 2, the property of a substance (molecule, atom, ion) can be used as an oxidant (electrons are obtained in the reaction, the valency is reduced, that is, the oxidant) or as an electron acquirer is called oxidation.

Strong oxidizing agents have strong oxidizing properties. Under normal conditions, several common oxidants are composed of strong and weak order, such as F2, KMNO4 (acidic condition), HClLo (when coexisting with strong acid), HNO3, Fe3+, Cu2+, etc. The oxidation of the same oxidant is condition-dependent.

When the temperature is high, it is stronger than when the temperature is low; When it is thick, it is stronger than when it is thin; It is stronger in acidic media than in neutral media. Oxygen is oxidizing, and oxygen is a commonly used oxidizing agent.

Some reactions can occur at room temperature, such as aluminum can react with oxygen at room temperature to form alumina, some reactions need to be heated or high temperature, and some are difficult to occur even at high temperatures.

Oxygen limb slip + carbon ignites the life calendar into carbon dioxide (C + O2 ignites to generate CO2), which is fully combusted.

Oxygen + carbon ignition to form carbon monoxide (2C + O2 ignition to produce 2CO) This one is inadequate combustion.

Oxygen + ethanol (alcohol) ignites to form carbon dioxide + water (C2H5OH+3O2 ignition to generate 2CO2+3H2O).

I'm typing very hard,

First, the reducibility of elemental metals is higher than that of metal components in oxides. In other words, the metal activity of elemental metals is higher than that of metals in oxides.

Second, the reaction temperature is reached. The reaction of this metal element with metal oxides needs to be endothermic.

Third, oxygen or other oxides are isolated, otherwise the metal will react with the oxide first.

Metal-to-metal oxide reaction conditions.

1.Elemental metals are more reactive than metals in oxides.

2.The conditions are usually heating or high temperatures.

For example: 2Al+Fe2O3=High temperature Al2O3+2Fe Mg+CuO=Heating=MGO+Cu

Generally in the case of pure oxygen, ignition.

Some of the metal elements that are listed at the top of the metal activity order table can be displaced. But some don't.

Metathesis: The valence state of the metal oxide can be stable in the solution after the reaction, for example, the metathesis reaction between Mno2 and concentrated hydrochloric acid cannot occur, and the redox can only be stabilized by redox into Mn2+: the oxidation of the acid should be large enough, and it can be after the metal valence, for example, the reaction between Cuo and dilute sulfuric acid is a simple metathesis reaction, because Cu2+ can be stable in the aqueous solution, and Cu2O (cuprous oxide) reacts with dilute sulfuric acid, that is, an oxidation reaction must occur to make Cu+(unstable in aqueous solution) becomes Cu2+

It is the reaction of an acid with a basic oxide, and it does not require conditions, and it can be reacted.

For example, cuo+2HCl==Cucl2+H2O

cao+2hcl==cacl2+h2o

I don't know how to ask. 3fe+4h2o=fe3o4+4h2

Some can, some can't, and it has to do with the liveliness of metal! The less reactive the metal, the easier it is for its oxides to react with carbon, which is essentially a reduction reaction!

Metathesis reactions between precursor ions.

Then there is the non-redox reaction.

Finally, there is the redox reaction.

This has to do with the speed of reaction.

Bases can also react with bases, and acids and acids also react.

Both substances that produce more difficult ionization and substances that produce water can react.

It reacts with acid to form salt and water, reacts with water to form alkali, reacts with reducing agent to form metal, and heats with weak chemical properties to form metal and oxygen.

Metal oxides.

It refers to a binary compound composed of oxygen and another metal chemical element, such as iron oxide (Fe2O3), sodium oxide (Na2O), etc.

Metal oxides are widely used in daily life. Quicklime is a commonly used desiccant that can also be used for disinfection; Iron oxide (Fe2O3) is commonly known as iron red and can be used as a red pigment; Catalysts used in some industrial processes are also metal oxides. Metal oxides are compounds formed by the combination of metal elements and oxygen elements.

All metals, including platinum and gold, have corresponding metal oxides. There are generally a variety of oxides in variable metals, for example, iron has two oxides, ferrous oxide (FeO) and iron oxide (Fe3O4 is ferrous ferrite, which belongs to the salt class).

Calcium oxide reacts with silica, calcium oxide is a metal oxide, and silica is a non-metal oxide.

The reaction equation is:

cao+sio₂ =casio₃

Calcium oxide is a basic oxide that is sensitive to moisture. It easily absorbs carbon dioxide and moisture from the air. It reacts with water to form calcium hydroxide and produces a lot of heat, which is corrosive.

Sodium peroxide reacts with carbon dioxide, which is a metal oxide and carbon dioxide is a non-metal oxide.

The reaction equation is:

Sodium peroxide is not a basic oxide, it is a peroxide, which can react with carbon dioxide (which does not react with dry carbon dioxide) or acid, and oxygen is released during the reaction.

In addition to carbon dioxide, sodium peroxide can also react with nitric oxide (NO) and nitrogen dioxide.

Sodium peroxide is an ionic compound, in which the oxygen element is -1 valence, and the sodium element is +1 valence, which can dissolve sodium peroxide in sulfuric acid at low temperature, and then distilled under reduced pressure to obtain hydrogen peroxide.

1. Most metal oxides are alkaline, such as sodium oxide, calcium oxide, magnesium oxide, etc. 2. Most non-metallic oxides are acidic, such as carbon dioxide, silicon dioxide, sulfur trioxide, etc. 3. Basic metal oxides react with acidic non-metallic oxides to generate salts such as Na2O+CO3=Na2CO3; cao+sio2=casio3；mgo+so3=mgso4

Non-metals react with oxygen, because oxygen is generally more oxidizing than other non-metallic elements (except F2), so non-metals are generally oxidized, for example: S+O2=SO2.

Non-metals are gases or brittle solids or liquids without metallic properties under normal conditions, such as the 15 elements in the upper right part of the periodic table and hydrogen, the elemental elements of group zero. Most non-metallic atoms have more valence shell S and P electrons, which can form a diatomic molecular gas or a crystal structure of skeleton-like, chain-like or layered macromolecules.

Most non-metallic atoms have more valence shell S and P electrons, which can form a diatomic molecular gas or a crystal structure of skeleton-like, chain-like or layered macromolecules.

Between metals and non-metals, there are arsenic, antimony, silicon, germanium, etc., which are known as metaloids.

When conditions such as temperature or pressure change, metals or non-metals may be transformed. For example, metal tin can be turned into non-metallic gray tin at low temperatures.

Periodic table.

For the main group of elements, with the increase of atomic number, the number of nuclear charges of the atom gradually increases, but the number of electron layers does not change, so the gravitational attraction of the nucleus to the electrons outside the nucleus gradually increases, and the electron loss ability of the atom gradually decreases with the decrease of the atomic radius, and the metallicity of the element gradually decreases. The ability of atoms to gain electrons gradually increases, and the non-metallic properties of elements gradually increase. For example: for the metal Na>mg of the third period element.

With the increase of the atomic number, the electron shell gradually increases, the atomic radius increases significantly, the gravitational force of the atomic nucleus on the outermost electron gradually decreases, the atomic electron loss of the element gradually increases, and the electron-gaining ability gradually decreases, so the metallicity of the element gradually increases, and the non-metallicity weakens. For example: metallicity HCl>Br>I of the first main group element.

Combining the above two cases, a concise conclusion can be made: in the periodic table, the further to the left and below, the stronger the metallicity of the element, and the metal with the strongest metallicity is CS; The further to the right and up, the stronger the non-metallic of the element, and the strongest non-metallic element is f. For example:

Metallic K>Na>mg, non-metallic O>S>P.

Due to the complex bonding mode of non-metallic elements, almost all compounds contain non-metallic elements.

If non-metallic elements and metallic elements form inorganic compounds together, anoxic salts, oxygenates and complexes can be formed. If only inorganics are formed from non-metallic elements, a series of covalent compounds such as acids and others can be formed.

The non-metallic element carbon is the basis of organic compounds.

(1) Most metals can react with oxygen, but the difficulty and intensity of the reaction are different; Magnesium and aluminum can react with oxygen at room temperature; Iron and copper cannot react with oxygen at room temperature, but can react with oxygen at high temperature; Gold cannot react with oxygen even at high temperatures Activity: magnesium, aluminum, iron, copper, gold.

2) Aluminum reacts with oxygen in the air at room temperature to form a dense alumina film on its surface, which plays a protective role

Therefore, the answer is: (1) most metals; magnesium, aluminum; iron, copper; Gold; Real gold is not afraid of fire refining (2) dense alumina film; Plays a protective role.