Before we talk about concepts, let's look at the following two examples:
2NaOH+COtwo=NatwoCOthree+HtwoO
Ca(OH)two+SOthree=CaSOfour+HtwoO
The above reaction shows that:carbon dioxideThe nature of sulfur trioxide is similar to that of acid. Therefore, people call carbon dioxide and sulfur trioxide, which can react with alkali to form only salt and water oxidesAcid oxide。
However, acid oxides are not necessarily non-metallic oxides.
React with water
Most acid oxides can directly combine with water to form acids.
COtwo+HtwoO=HtwoCOthree
SOthree+HtwoO=HtwoSOfour
SiOtwoCan not react directly with water to generate HtwoSiOthree。
Unstable acid can also be generated by thermal decompositionAcid oxide。
HtwoCOthree=(Heating) CO2↑+HtwoO
HtwoSOfour=SOthree↑+HtwoO
ad locumcarbon dioxideSulfur trioxide can be regarded as the product of dehydration of carbonic acid and sulfuric acid, calledAcid anhydride。
It can be said that all acid oxides are anhydride.
Reaction with alkali
Acid oxides can react with alkali to form salt and water.
2NaOH+COtwo=NatwoCOthree+HtwoO
Ca(OH)two+SOthree=CaSOfour+HtwoO
And alkaline oxides
Under certain conditions,Alkaline oxideReact with acid oxides to form salts.
CaO+COtwo=CaCOthree
CaO+SiOtwo=(High temperature) CaSiOthree[2]
Alkaline oxide
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For the same introduction, let's look at the following two examples:
2HCl+CuO=CuCltwo+H2O
3HtwoSOfour+FetwoOthree=Fetwo(SOfour)three+3HtwoO
The above reaction shows that the properties of copper oxide, iron oxide and alkali are similar.Therefore, people call copper oxide and iron oxide, which can react with acid to form only salt and water oxidesAlkaline oxide。(SiOtwoIt can react with HF, but SiOtwoyesAcid oxide(SiOtwoCan react with HF is SiOtwoIs independent of whether it is alkaline oxide or acidic oxide)metallic oxideAnd other low valent oxides of metals, such as NatwoO. CaO, BaO, CrO, MnO, etc.)
Most metal oxides areAlkaline oxide, but there are some other types, with the exception of MntwoOseven(Acid oxide),AltwoOthree(Amphoteric oxide), ZnO (amphoteric oxide), MnOtwo(amphoteric oxide), etc.
Although acid oxides are not necessarilyNonmetallic oxide(e.g. MntwoOseven)However, we can say that the alkaline oxide must be a metal oxide.
React with water
The corresponding hydrate of alkaline oxide is alkali, and the corresponding alkali isSoluble alkaliThe alkaline oxide of C can be directly combined with water to form a base.
KtwoO+HtwoO=2KOH
NatwoO+HtwoO=2NaOH
BaO+HtwoO=Ba(OH)two
CaO+HtwoO=Ca(OH)two
Theoretically,Alkaline oxideIt can be regarded as the product of corresponding alkali dehydration.
Insoluble alkali can be decomposed by heat to produce corresponding alkaline oxide and water.
Cu(OH)two=(Heating) CuO+HtwoO
React with acid
Alkaline oxides can react with acids to form salts and water.
Because it is a critical elementMetallicity, there are certainNonmetallic, while being able toStrong acid and strong baseThe reaction is called amphoteric, and the corresponding hydrates are alsoAmphoteric hydroxide。
As AltwoOthree, ZnO, etc.
With AltwoOthreeFor example:
AltwoOthree+ 6HCl= 2AlClthree+ 3HtwoO
AltwoOthree+ 2NaOH = 2NaAlOtwo+ HtwoO[2]
MnOtwoSameAmphoteric oxide。Moderate oxidation in acid medium, 2MnOtwo+2HtwoSOfour=2MnSOfour+Otwo+2HtwoO。It has medium strength reducibility in strong alkali and can be oxidized by oxygen in air to produce MnOfour。
MntwoOseven>MnOthree>MnOtwo>MnO
Acidic Acidic Amphoteric Alkaline
Neutral oxide
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Oxides that cannot react with acid to form salt and water and cannot react with alkali to form salt and water are calledNeutral oxideperhapsUnsalted oxide。
Nitrogen dioxideIt is an unsalted oxide because the valence in the oxyacid of nitrogen is not+4.(The oxide corresponding to nitrate isNitrogen pentoxideIt is not nitrogen dioxide, or the anhydride of nitric acid is nitrogen pentoxide instead of nitrogen dioxide.)
It should be noted here that some non salt forming oxides can "form salt" under certain conditions.
althoughcarbon monoxideCan followsodium hydroxideReact to form sodium salt of formic acid.However, no water is generated when salt is generated, so carbon monoxide still belongs to non salt oxide.[2]
peroxide
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Sodium peroxideperoxide, because the molecule containsPeroxy grouporPeroxy ionAnd get its name.In addition, it has extremely weak acidichydrogen peroxidePeroxides can also be formed by reacting with alkali.Therefore, peroxide can also be regarded as a salt of hydrogen peroxide.Metal that can generate peroxide, mainly alkali metal andalkaline-earth metal。
Sodium peroxideSodium peroxide is one of the products of sodium combustion in oxygen or air. Pure sodium peroxide is white, but generally seen sodium peroxide is light yellow, because a small amount of sodium peroxide is generated during the reactionSodium Superoxide。Sodium peroxide is easy toDeliquescence, Yescorrosive, should be sealed for storage;With strongOxidizability, can be used tobleachTextile articles, straw, feathers, etc.[3]
8 Electronic housing, oxide of highly charged ions
MntwoOseven[4]
chemical property
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Acid-base property
According to the acid-base characteristics, oxides can be divided into four categories: acidic, alkaline, amphoteric and neutral.
(1)Acid oxide。Oxides that dissolve in water as acid solutions or occur with the same alkali are acid oxides.For example:
PfourOten+6HtwoO→4HthreePOfour
SbtwoOfive+2NaOH+5HtwoO→2Na[Sb(OH)six]
Most non-metallic covalent oxides and some highly oxidized metal oxides with weak electropositivity are acidic.
(2)Alkaline oxide。The oxides dissolved in water as alkaline solution or occurring with acid are alkaline oxides.For example:
CaO+HtwoO→Ca(OH)two
FetwoOthree+6HCl→2FeClthree+3HtwoO
The oxides of most electropositive elements are alkaline.
(3)Amphoteric oxide。The oxides that are alkaline and acidic with strong acid are amphoteric oxides.For example:
ZnO+2HCl→ZnCltwo+H2O
ZnO+2NaOH+HtwoO→Natwo[Zn(OH)four]
The oxides of some metal elements close to the non-metallic region in the long-period table are easy to show hermaphroditism.
(4)Neutral oxide。Oxides that do not react with acids or bases are called neutral oxides.E.g. CO and NtwoO。
See:Acidity and alkalinity of oxides。
thermal stability
Most oxides have highthermal stability, especially oxides and Li of IIA and IVB group elementstwoO、NatwoO、BtwoOthree、AltwoO3、SiOtwoLess oxide with thermal instability, such ashalogenOxide, NtwoOfive、Ag2O. HgO, etc.Short period elementOxidestabilityDecreasing from left to right, alkali only metal element oxides are more stablealkaline-earth metalFor poor, when we consider M+The repulsion between ions makes MtwoWhen the lattice energy of O is low, it is not difficult to understand this "abnormal" phenomenon;In the same family, especiallySubfamily elements, thermal stability is enhanced from top to bottom, this is because, althoughcationAnd the sum of anion radiusLattice energy, but withAtomic radiusThe effect of increasing the ionization energy is more significant, especially when the cationRadius ratioThis is especially true when the radius of the oxygen ion is small.
② It can be divided into ionic oxide and covalent oxide according to bonding type or constituent particle type
Ionic oxide: oxides formed by some active metal elements, such as Na2O, CaO, etc
Covalent oxides: oxides of some metallic elements and all non-metallic elements, such as MnO2, HgO, SO2, ClO2, etc
③ According to the oxidation state of oxygen, it can be divided into ordinary oxides (the oxidation state of oxygen is - 2), peroxides (the oxidation state of oxygen is - 1)Superoxide(The oxidation state of oxygen is - 1/2) and ozone (the oxidation state of oxygen is - 1/3)
④ According to the acidity and alkalinity, whether it forms salt with water, and the salt content generatedAcid oxide, alkaline oxides and amphoteric oxidesNeutral oxide、Complex oxide。