Properties of oxides
Oxides are complex chemical substances that are chemical compounds simple elements with oxygen. They are salt-forming And non-salt forming. In this case, there are 3 types of salt-forming agents: main(from the word "foundation"), acidic And amphoteric.
An example of oxides that do not form salts are: NO (nitric oxide) - is a colorless, odorless gas. It is formed during a thunderstorm in the atmosphere. CO (carbon monoxide) is an odorless gas produced by the combustion of coal. It is usually called carbon monoxide. There are other oxides that do not form salts. Now let's take a closer look at each type of salt-forming oxides.
Basic oxides
Basic oxides- these are complex chemical substances related to oxides that form salts when chemical reaction with acids or acidic oxides and do not react with bases or basic oxides. For example, the main ones include the following:
K 2 O (potassium oxide), CaO (calcium oxide), FeO (ferrous oxide).
Let's consider Chemical properties oxides with examples
1. Interaction with water:
- interaction with water to form a base (or alkali)
CaO+H 2 O → Ca(OH) 2 (known lime slaking reaction, which releases large quantities warmth!)
2. Interaction with acids:
- interaction with acid to form salt and water (salt solution in water)
CaO+H 2 SO 4 → CaSO 4 + H 2 O (Crystals of this substance CaSO 4 are known to everyone under the name “gypsum”).
3. Interaction with acid oxides: salt formation
CaO+CO 2 → CaCO 3 (Everyone knows this substance - ordinary chalk!)
Acidic oxides- these are complex chemical substances related to oxides that form salts upon chemical interaction with bases or basic oxides and do not interact with acidic oxides.
Examples of acidic oxides can be:
CO 2 (well-known carbon dioxide), P 2 O 5 - phosphorus oxide (formed by the combustion of white phosphorus in air), SO 3 - sulfur trioxide - this substance is used to produce sulfuric acid.
Chemical reaction with water
CO 2 +H 2 O → H 2 CO 3 - this substance is carbonic acid - one of the weak acids, it is added to carbonated water to create gas “bubbles”. With increasing temperature, the solubility of gas in water decreases, and its excess comes out in the form of bubbles.
Reaction with alkalis (bases):
CO 2 +2NaOH→ Na 2 CO 3 +H 2 O- the resulting substance (salt) is widely used in the household. Its name is soda ash or washing soda, - excellent detergent for burnt pans, fat, burnt marks. I do not recommend working with bare hands!
Reaction with basic oxides:
CO 2 +MgO→ MgCO 3 - the resulting salt is magnesium carbonate - also called “bitter salt”.
Amphoteric oxides
Amphoteric oxides- these are complex chemical substances, also related to oxides, which form salts during chemical interaction with acids (or acid oxides) and grounds (or basic oxides). The most common use of the word "amphoteric" in our case refers to metal oxides.
Example amphoteric oxides can be:
ZnO - zinc oxide (white powder, often used in medicine for making masks and creams), Al 2 O 3 - aluminum oxide (also called “alumina”).
The chemical properties of amphoteric oxides are unique in that they can enter into chemical reactions with both bases and acids. For example:
Reaction with acid oxide:
ZnO+H 2 CO 3 → ZnCO 3 + H 2 O - The resulting substance is a solution of the salt “zinc carbonate” in water.
Reaction with bases:
ZnO+2NaOH→ Na 2 ZnO 2 +H 2 O - the resulting substance is a double salt of sodium and zinc.
Obtaining oxides
Obtaining oxides produce different ways. This can happen physically and by chemical means. The most in a simple way is the chemical interaction of simple elements with oxygen. For example, the result of the combustion process or one of the products of this chemical reaction are oxides. For example, if a hot iron rod, and not only iron (you can take zinc Zn, tin Sn, lead Pb, copper Cu - basically whatever is at hand) is placed in a flask with oxygen, then a chemical reaction of iron oxidation will occur, which accompanied by a bright flash and sparks. The reaction product will be black iron oxide powder FeO:
2Fe+O 2 → 2FeO
Chemical reactions with other metals and non-metals are completely similar. Zinc burns in oxygen to form zinc oxide
2Zn+O 2 → 2ZnO
Coal combustion is accompanied by the formation of two oxides at once: carbon monoxide and carbon dioxide.
2C+O 2 → 2CO - formation of carbon monoxide.
C+O 2 → CO 2 - formation of carbon dioxide. This gas is formed if there is more than enough oxygen, that is, in any case, the reaction first occurs with the formation of carbon monoxide, and then the carbon monoxide is oxidized, turning into carbon dioxide.
Obtaining oxides can be done in another way - through a chemical decomposition reaction. For example, to obtain iron oxide or aluminum oxide, it is necessary to calcinate the corresponding bases of these metals over a fire:
Fe(OH) 2 → FeO+H 2 O
Solid aluminum oxide - mineral corundum 
Iron(III) oxide. The surface of the planet Mars is reddish-orange in color due to the presence of iron (III) oxide in the soil. Solid aluminum oxide - corundum 
2Al(OH) 3 → Al 2 O 3 +3H 2 O,
as well as during the decomposition of individual acids:
H 2 CO 3 → H 2 O+CO 2 - decomposition of carbonic acid
H 2 SO 3 → H 2 O+SO 2 - decomposition of sulfurous acid
Obtaining oxides can be made from metal salts with strong heating:
CaCO 3 → CaO+CO 2 - calcination of chalk produces calcium oxide (or quicklime) and carbon dioxide.
2Cu(NO 3) 2 → 2CuO + 4NO 2 + O 2 - in this decomposition reaction two oxides are obtained at once: copper CuO (black) and nitrogen NO 2 (it is also called brown gas because of its really brown color).
Another way in which oxides can be produced is through redox reactions.
Cu + 4HNO 3 (conc.) → Cu(NO 3) 2 + 2NO 2 + 2H 2 O
S + 2H 2 SO 4 (conc.) → 3SO 2 + 2H 2 O
Chlorine oxides
ClO2 molecule 
Cl 2 O 7 molecule 
Nitrous oxide N2O 
Nitrogenous anhydride N 2 O 3 
Nitric anhydride N 2 O 5 
Brown gas NO 2 The following are known chlorine oxides: Cl 2 O, ClO 2, Cl 2 O 6, Cl 2 O 7. All of them, with the exception of Cl 2 O 7, are yellow or orange in color and are not stable, especially ClO 2, Cl 2 O 6. All chlorine oxides are explosive and are very strong oxidizing agents.
Reacting with water, they form the corresponding oxygen-containing and chlorine-containing acids:
So, Cl 2 O - acid chlorine oxide hypochlorous acid.
Cl 2 O + H 2 O → 2HClO - Hypochlorous acid
ClO2 - acid chlorine oxide hypochlorous and hypochlorous acid, since during a chemical reaction with water it forms two of these acids at once:
ClO 2 + H 2 O→ HClO 2 + HClO 3
Cl 2 O 6 - too acid chlorine oxide perchloric and perchloric acids:
Cl 2 O 6 + H 2 O → HClO 3 + HClO 4
And finally, Cl 2 O 7 - a colorless liquid - acid chlorine oxide perchloric acid:
Cl 2 O 7 + H 2 O → 2HClO 4
Nitrogen oxides
Nitrogen is a gas that forms 5 different compounds with oxygen - 5 nitrogen oxides. Namely:
N2O- nitric oxide. Its other name is known in medicine as laughing gas or nitrous oxide- It is colorless, sweetish and pleasant to the taste of gas.
- NO - nitrogen monoxide- a colorless, odorless, tasteless gas.
- N 2 O 3 - nitrous anhydride- colorless crystalline substance
- NO 2 - nitrogen dioxide. Its other name is brown gas- the gas really has a brownish-brown color
- N 2 O 5 - nitric anhydride- blue liquid, boiling at a temperature of 3.5 0 C
Of all these listed nitrogen compounds, NO - nitrogen monoxide and NO 2 - nitrogen dioxide are of greatest interest in industry. Nitrogen monoxide(NO) and nitrous oxide N 2 O does not react with water or alkalis. (N 2 O 3) when reacting with water forms a weak and unstable nitrous acid HNO 2, which in air gradually turns into a more stable Chemical substance nitric acid Let's look at some chemical properties of nitrogen oxides:
Reaction with water:
2NO 2 + H 2 O → HNO 3 + HNO 2 - 2 acids are formed at once: nitric acid HNO 3 and nitrous acid.
Reaction with alkali:
2NO 2 + 2NaOH → NaNO 3 + NaNO 2 + H 2 O - two salts are formed: sodium nitrate NaNO 3 (or sodium nitrate) and sodium nitrite (a salt of nitrous acid).
Reaction with salts:
2NO 2 + Na 2 CO 3 → NaNO 3 + NaNO 2 + CO 2 - two salts are formed: sodium nitrate and sodium nitrite, and carbon dioxide is released.
Nitrogen dioxide (NO 2) is obtained from nitrogen monoxide (NO) using a chemical reaction of combining with oxygen:
2NO + O 2 → 2NO 2
Iron oxides
Iron forms two oxide:FeO- iron oxide(2-valent) - black powder, which is obtained by reduction iron oxide(3-valent) carbon monoxide by the following chemical reaction:
Fe 2 O 3 +CO→ 2FeO+CO 2
This is a basic oxide that reacts easily with acids. It has reducing properties and quickly oxidizes into iron oxide(3-valent).
4FeO +O 2 → 2Fe 2 O 3
Iron oxide(3-valent) - red-brown powder (hematite), which has amphoteric properties (can interact with both acids and alkalis). But the acidic properties of this oxide are so weakly expressed that it is most often used as basic oxide.
There are also so-called mixed iron oxide Fe 3 O 4 . It is formed when iron burns and conducts well electricity and has magnetic properties(it is called magnetic iron ore or magnetite). If iron burns, then as a result of the combustion reaction, scale is formed, consisting of two oxides: iron oxide(III) and (II) valence.
Sulfur oxide
Sulphur dioxide SO 2 Sulfur oxide SO 2 - or sulphur dioxide refers to acid oxides, but does not form acid, although it is perfectly soluble in water - 40 liters of sulfur oxide in 1 liter of water (for the convenience of drawing up chemical equations, such a solution is called sulfurous acid).
Under normal circumstances, it is a colorless gas with a pungent and suffocating odor of burnt sulfur. At a temperature of only -10 0 C it can be converted into a liquid state.
In the presence of a catalyst - vanadium oxide (V 2 O 5) sulfur oxide attaches oxygen and turns into sulfur trioxide
2SO 2 +O 2 → 2SO 3
Dissolved in water sulphur dioxide- sulfur oxide SO2 - oxidizes very slowly, as a result of which the solution itself turns into sulfuric acid
If sulphur dioxide pass an alkali, for example, sodium hydroxide, through a solution, then sodium sulfite is formed (or hydrosulfite - depending on how much alkali and sulfur dioxide you take)
NaOH + SO 2 → NaHSO 3 - sulphur dioxide taken in excess
2NaOH + SO 2 → Na 2 SO 3 + H 2 O
If sulfur dioxide does not react with water, then why does its aqueous solution give an acidic reaction?! Yes, it does not react, but it itself oxidizes in water, adding oxygen to itself. And it turns out that free hydrogen atoms accumulate in water, which give an acidic reaction (you can check with some indicator!)
In lesson 32 " Chemical properties of oxides" from the course " Chemistry for dummies“We will learn about all the chemical properties of acidic and basic oxides, consider what they react with and what is formed.
Because chemical composition Acid and basic oxides are different; they differ in their chemical properties.
1. Chemical properties of acid oxides
a) Interaction with water
You already know that the products of the interaction of oxides with water are called “hydroxides”:
Since the oxides that enter into this reaction are divided into acidic and basic, the hydroxides formed from them are also divided into acidic and basic. Thus, acidic oxides (except SiO2) react with water to form acidic hydroxides, which are oxygen-containing acids:
Each acidic oxide corresponds to an oxygen-containing acid, which is classified as acidic hydroxides. Despite the fact that silicon oxide SiO 2 does not react with water, the acid H 2 SiO 3 also corresponds to it, but it is obtained by other methods.
b) Interaction with alkalis
All acid oxides react with alkalis according to the general scheme:
In the resulting salt, the valency of the metal atoms is the same as in the original alkali. Besides, the salt contains the remainder of the acid that corresponds to the given acid oxide.
For example, if the acidic oxide CO 2 reacts, which corresponds to the acid H 2 CO3 CO3, whose valence, as you already know, is II:
If the acidic oxide N 2 O 5 enters into the reaction, which corresponds to the acid H NO 3(indicated in square brackets), then the resulting salt will contain the remainder of this acid - NO 3 with valency equal to I:
Since all acidic oxides react with alkalis to form salts and water, these oxides can be given another definition.
Acidic are called oxides that react with alkalis to form salts and water.
c) Reactions with basic oxides
Acidic oxides react with basic oxides to form salts according to the general scheme:
In the resulting salt, the valency of the metal atoms is the same as in the original basic oxide. It should be remembered that the salt contains the remainder of the acid that corresponds to the acid oxide that enters into the reaction. For example, if the acidic oxide SO 3 reacts, which corresponds to the acid H 2 SO 4(indicated in square brackets), then the salt will include the remainder of this acid - SO 4, whose valency is II:
If the acidic oxide P 2 O 5 enters into the reaction, which corresponds to the acid H 3 RO 4, then the resulting salt will contain the remainder of this acid - PO 4 with a valence of III.
2. Chemical properties of basic oxides
a) Interaction with water
You already know that as a result of the interaction of basic oxides with water, basic hydroxides are formed, which are otherwise called bases:
These basic oxides include the following oxides: Li 2 O, Na 2 O, K 2 O, CaO, BaO.
When writing equations for the corresponding reactions, it should be remembered that the valence of metal atoms in the resulting base is equal to its valence in the original oxide.
Basic oxides formed by metals such as Cu, Fe, Cr do not react with water. The corresponding bases are obtained in other ways.
b) Interaction with acids
Almost all basic oxides react with acids to form salts according to the general scheme:
It should be remembered that in the resulting salt, the valency of the metal atoms is the same as in the original oxide, and the valency acid residue the same as in the original acid.
Since all basic oxides react with acids to form salts and water, these oxides can be given another definition.
Main are called oxides that react with acids to form salts and water.
c) Interaction with acid oxides
Basic oxides react with acidic oxides to form salts according to the general scheme:
In the resulting salt, the valency of the metal atoms is the same as in the original basic oxide. In addition, you should remember that the salt contains the remainder of the acid that corresponds to the acid oxide that reacts. For example, if the acidic oxide N2O5 reacts, which corresponds to the acid H NO 3, then the salt will contain the remainder of this acid - NO 3, whose valency, as you already know, is I.
Since the acidic and basic oxides we have considered form salts as a result of various reactions, they are called salt-forming. There is, however, no large group oxides that do not form salts in similar reactions, which is why they are called non-salt-forming.
Brief conclusions of the lesson:
- All acidic oxides react with alkalis to form salts and water.
- All basic oxides react with acids to form salts and water.
- Acidic and basic oxides are salt-forming. Non-salt-forming oxides - CO, N 2 O, NO.
- Bases and oxygen-containing acids are hydroxides.
Hope lesson 32" Chemical properties of oxides"was clear and informative. If you have any questions, write them in the comments.
Modern encyclopedia
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Oxides are called complex substances whose molecules include oxygen atoms in oxidation state - 2 and some other element.
can be obtained through the direct interaction of oxygen with another element, or indirectly (for example, during the decomposition of salts, bases, acids). Under normal conditions, oxides come in solid, liquid and gaseous states; this type of compound is very common in nature. Oxides are contained in Earth's crust. Rust, sand, water, carbon dioxide are oxides.
They are either salt-forming or non-salt-forming.
Salt-forming oxides- These are oxides that form salts as a result of chemical reactions. These are oxides of metals and non-metals, which, when interacting with water, form the corresponding acids, and when interacting with bases, the corresponding acidic and normal salts. For example, copper oxide (CuO) is a salt-forming oxide because, for example, when it interacts with hydrochloric acid(HCl) salt is formed:
CuO + 2HCl → CuCl 2 + H 2 O.
As a result of chemical reactions, other salts can be obtained:
CuO + SO 3 → CuSO 4.
Non-salt-forming oxides These are oxides that do not form salts. Examples include CO, N 2 O, NO.
Salt-forming oxides, in turn, are of 3 types: basic (from the word «
base »
), acidic and amphoteric.
Basic oxides These metal oxides are called those that correspond to hydroxides belonging to the class of bases. Basic oxides include, for example, Na 2 O, K 2 O, MgO, CaO, etc.
Chemical properties of basic oxides
1. Water-soluble basic oxides react with water to form bases:
Na 2 O + H 2 O → 2NaOH.
2. React with acid oxides, forming the corresponding salts
Na 2 O + SO 3 → Na 2 SO 4.
3. React with acids to form salt and water:
CuO + H 2 SO 4 → CuSO 4 + H 2 O.
4. React with amphoteric oxides:
Li 2 O + Al 2 O 3 → 2LiAlO 2.
If the composition of the oxides contains a non-metal or a metal exhibiting the highest valence (usually from IV to VII) as the second element, then such oxides will be acidic. Acidic oxides (acid anhydrides) are those oxides that correspond to hydroxides belonging to the class of acids. These are, for example, CO 2, SO 3, P 2 O 5, N 2 O 3, Cl 2 O 5, Mn 2 O 7, etc. Acidic oxides dissolve in water and alkalis, forming salt and water.
Chemical properties of acid oxides
1. React with water to form an acid:
SO 3 + H 2 O → H 2 SO 4.
But not all acidic oxides react directly with water (SiO 2, etc.).
2. React with based oxides to form a salt:
CO 2 + CaO → CaCO 3
3. React with alkalis, forming salt and water:
CO 2 + Ba(OH) 2 → BaCO 3 + H 2 O.
Part amphoteric oxide includes an element that has amphoteric properties. Amphotericity refers to the ability of compounds to exhibit acidic and basic properties depending on conditions. For example, zinc oxide ZnO can be either a base or an acid (Zn(OH) 2 and H 2 ZnO 2). Amphotericity is expressed in the fact that, depending on the conditions, amphoteric oxides exhibit either basic or acidic properties.
Chemical properties of amphoteric oxides
1. React with acids to form salt and water:
ZnO + 2HCl → ZnCl 2 + H 2 O.
2. React with solid alkalis (during fusion), forming as a result of the reaction salt - sodium zincate and water:
ZnO + 2NaOH → Na 2 ZnO 2 + H 2 O.
When zinc oxide interacts with an alkali solution (the same NaOH), another reaction occurs:
ZnO + 2 NaOH + H 2 O => Na 2.
Coordination number is a characteristic that determines the number of nearby particles: atoms or ions in a molecule or crystal. Each amphoteric metal has its own coordination number. For Be and Zn it is 4; For and Al it is 4 or 6; For and Cr it is 6 or (very rarely) 4;
Amphoteric oxides are usually insoluble in water and do not react with it.
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Oxides, their classification and properties are the basis of such an important science as chemistry. They begin to be studied in the first year of studying chemistry. In such exact sciences as mathematics, physics and chemistry, all the material is interconnected, which is why failure to master the material entails a lack of understanding of new topics. Therefore, it is very important to understand the topic of oxides and fully understand it. We will try to talk about this in more detail today.
What are oxides?
Oxides, their classification and properties are what needs to be understood first. So, what are oxides? Do you remember this from school?
Oxides (or oxides) are binary compounds that contain atoms of an electronegative element (less electronegative than oxygen) and oxygen with an oxidation state of -2.
Oxides are incredibly common substances on our planet. Examples of oxide compounds include water, rust, some dyes, sand, and even carbon dioxide.
Formation of oxides
Oxides can be obtained in a variety of ways. The formation of oxides is also studied by such a science as chemistry. Oxides, their classification and properties - this is what scientists need to know in order to understand how this or that oxide was formed. For example, they can be obtained by direct connection oxygen atom (or atoms) with chemical element is the interaction of chemical elements. However, there is also indirect formation of oxides, this is when oxides are formed by the decomposition of acids, salts or bases.
Oxides classification
Oxides and their classification depend on how they are formed. According to their classification, oxides are divided into only two groups, the first of which is salt-forming, and the second is non-salt-forming. So, let's take a closer look at both groups.
Salt-forming oxides are a fairly large group, which is divided into amphoteric, acidic and basic oxides. As a result of any chemical reaction, salt-forming oxides form salts. As a rule, the composition of salt-forming oxides includes elements of metals and non-metals, which form acids as a result of a chemical reaction with water, but when interacting with bases they form the corresponding acids and salts.
Non-salt-forming oxides are those oxides that do not form salts as a result of a chemical reaction. Examples of such oxides include carbon.
Amphoteric oxides
Oxides, their classification and properties are very important concepts in chemistry. The composition of salt-forming compounds includes amphoteric oxides.
Amphoteric oxides are oxides that can exhibit basic or acidic properties, depending on the conditions of chemical reactions (they exhibit amphotericity). Such oxides are formed by transition metals (copper, silver, gold, iron, ruthenium, tungsten, rutherfordium, titanium, yttrium and many others). Amphoteric oxides react with strong acids, and as a result of a chemical reaction they form salts of these acids.
Acidic oxides
Or anhydrides are oxides that exhibit and also form oxygen-containing acids in chemical reactions. Anhydrides are always formed by typical nonmetals, as well as by some transition chemical elements.
Oxides, their classification and chemical properties are important concepts. For example, acidic oxides have completely different chemical properties from amphoteric oxides. For example, when an anhydride reacts with water, a corresponding acid is formed (the exception is SiO2 - Anhydrides react with alkalis, and as a result of such reactions water and soda are released. When reacting with, a salt is formed.
Basic oxides
Basic (from the word "base") oxides are oxides of chemical elements of metals with oxidation states +1 or +2. These include alkali and alkaline earth metals, as well as the chemical element magnesium. Basic oxides differ from others in that they are the ones that are able to react with acids.
Basic oxides interact with acids, unlike acidic oxides, as well as with alkalis, water, and other oxides. As a result of these reactions, salts are usually formed.
Properties of oxides
If you carefully study the reactions of various oxides, you can independently draw conclusions about what chemical properties the oxides are endowed with. The common chemical property of absolutely all oxides is the redox process.
But nevertheless, all oxides are different from each other. The classification and properties of oxides are two interrelated topics.
Non-salt-forming oxides and their chemical properties
Non-salt-forming oxides are a group of oxides that exhibit neither acidic, basic, nor amphoteric properties. As a result of chemical reactions with non-salt-forming oxides, no salts are formed. Previously, such oxides were not called non-salt-forming, but indifferent and indifferent, but such names do not correspond to the properties of non-salt-forming oxides. According to their properties, these oxides are quite capable of chemical reactions. But there are very few non-salt-forming oxides; they are formed by monovalent and divalent nonmetals.
From non-salt-forming oxides, salt-forming oxides can be obtained as a result of a chemical reaction.
Nomenclature
Almost all oxides are usually called this way: the word “oxide”, followed by the name of the chemical element in the genitive case. For example, Al2O3 is aluminum oxide. In chemical language, this oxide reads like this: aluminum 2 o 3. Some chemical elements, such as copper, can have several degrees of oxidation; accordingly, the oxides will also be different. Then CuO oxide is copper (two) oxide, that is, with an oxidation degree of 2, and Cu2O oxide is copper (three) oxide, which has an oxidation degree of 3.
But there are other names for oxides, which are distinguished by the number of oxygen atoms in the compound. Monoxides or monoxides are those oxides that contain only one oxygen atom. Dioxides are those oxides that contain two oxygen atoms, which are indicated by the prefix “di”. Trioxides are those oxides that already contain three oxygen atoms. Names such as monoxide, dioxide and trioxide are already outdated, but are often found in textbooks, books and other aids.
There are also so-called trivial names for oxides, that is, those that have developed historically. For example, CO is the oxide or monoxide of carbon, but even chemists most often call this substance carbon monoxide.
So, an oxide is a compound of oxygen with a chemical element. The main science that studies their formation and interactions is chemistry. Oxides, their classification and properties are a few important topics in science there is chemistry, without understanding which it is impossible to understand everything else. Oxides are gases, minerals, and powders. Some oxides are worth knowing in detail not only for scientists, but also ordinary people, because they can even be dangerous to life on this earth. Oxides are a very interesting and quite easy topic. Oxide compounds are very common in everyday life.