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When most people hear the word “oxide,” they think of metal. But did you know that there are also non-metallic oxides? In this blog post, we will discuss the properties, uses, and formation of metallic and non-metallic oxides. We will also take a look at some examples of each type of oxide. So whether you’re a student studying for a chemistry test or just interested in learning more about these materials,
What are Oxides?
An oxide is a chemical compound that contains at least one oxygen atom and one other element. When combined, these two elements form an ionic bond, meaning they share electrons. There are two types of oxides: metallic and non-metallic. The main difference between the two is in their properties and uses. Metallic oxides tend to be hard, insoluble in water, and have a high melting point. They are used for things like jewellery and metal production. Non-metallic oxides, on the other hand, are usually soft, soluble in water, and have a low melting point. They are often used in chemical reactions or as abrasives.
What are Metallic Oxides
Metallic oxides are compounds that contain at least one metal and one oxygen atom. They can be either ionic or covalent, but most are ionic. Metallic oxides are generally insoluble in water, but some (like aluminium oxide) are soluble. Many metallic oxides are basic, meaning they react with acids to form salt and water.
Uses of Metallic Oxides
Metallic oxides have a variety of uses. Some, like iron oxide, are used as pigments in paints and plastics. Others, like titanium oxide, are used as catalysts or for their photo catalytic properties. Still others, like aluminium oxide, are used in abrasives and refractory materials.
Formation of Metallic Oxides
Metallic oxides can be formed in several ways. The most common is the reaction of a metal with oxygen, but they can also be formed by the decomposition of metal salts or by the reaction of a metal with acid. Some metallic oxides, like chromium oxide, can even be formed by the oxidation of the metal itself.
Reduction of Metallic Oxides
Metallic oxides can be reduced to metal by heating in the presence of a reducing agent. The most common reducing agents are carbon (in the form of coal or coke) and hydrogen. Other reducing agents include metals like magnesium or calcium.
FeO + C → Fe + CO
In this reaction, the carbon reduces the iron oxide to iron. Carbon dioxide is a by-product of the reaction.
What are Non-metallic Oxides
Non-metallic oxides are compounds that contain at least one non-metal and one oxygen atom. They can be either ionic or covalent, but most are covalent. Non-metallic oxides are generally soluble in water, but some (like carbon dioxide) are insoluble. Many non-metallic oxides are acidic, meaning they react with bases to form salt and water.
Uses of Non-metallic Oxides
Non-metallic oxides have a variety of uses. Some, like carbon dioxide, are used as gases in food and beverage packaging. Others, like silicon dioxide, are used as abrasives or for their photo catalytic properties. Still others, like sulphuric acid, are used in batteries or as electrolytes.
Formation of Non-metallic Oxides
Non-metallic oxides can be formed in several ways. The most common is the reaction of a non-metal with oxygen, but they can also be formed by the decomposition of metal salts or by the reaction of a non-metal with acid. Some non-metallic oxides, like nitrogen oxide, can even be formed by the oxidation of the non-metal itself.
Reduction of Non-metallic Oxides
Non-metallic oxides can be reduced to non-metal by heating in the presence of a reducing agent. The most common reducing agents are carbon (in the form of coal or coke) and hydrogen. Other reducing agents include metals like magnesium or calcium.
NO + C → N + CO
In this reaction, the carbon reduces the nitrogen oxide to nitrogen. Carbon dioxide is a by-product of the reaction.
Difference Between Metallic and Non-metallic Oxides
Metallic oxides are those that contain metal in their chemical structure, while non-metallic oxides do not. The key difference between metallic and non-metallic oxides is that the metallic oxides conduct electricity, whereas the non-metallic oxides do not. This is because metals have free electrons in their outermost orbital, whereas non-metals do not. This means that when metallic oxides are heated, they become good electrical conductors. Non-metallic oxides, on the other hand, remain poor electrical conductors, even when heated.
Conclusion
In conclusion, metallic and non-metallic oxides play an important role in the world around us. They can be found naturally or produced artificially, and have a variety of uses depending on their properties. Some oxides are toxic, while others are essential for life. Understanding the formation and properties of these compounds is key to understanding their role in the world. Oxides are a fascinating class of compounds with a wide range of properties and uses. By understanding these molecules, we can better understand the world around us.
