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In the world of chemistry, oxides are a type of substance that is both ordinary and magical. They are not only simple combinations in the periodic table, but also important components ubiquitous in nature. This article will take you into the wonderful world of oxides, revealing their diversity and importance. Oxide refers to a compound composed of two elements, one of which must be oxygen. According to their different properties and structures, oxides can be classified into multiple types, each with its unique characteristics and applications. According to whether they contain metal elements, oxides can be divided into two categories: metal oxides and non-metal oxides. Metal oxides typically have high melting and boiling points, and can conduct electricity under certain conditions. For example, iron oxide (Fe ₂ O3) is a common metal oxide commonly used in the manufacture of pigments and magnetic materials. Non metallic oxides, on the other hand, are mostly molecular crystals that are generally non-conductive but may exhibit special physical or chemical properties in certain situations. Like carbon dioxide (CO ₂), it is a typical non-metallic oxide that plays an important role in the atmosphere. From the perspective of chemical reactions, oxides can also be divided into acidic oxides and alkaline oxides. Acidic oxides are oxides that react with bases to form salts and water. Acidic oxides can usually react with water to form acids, and sulfur dioxide (SO ₂) is a typical example. When it combines with water, it forms sulfurous acid (H ₂ SO3). Alkaline oxides are oxides that can react with acids, salts, and water. Sodium hydroxide (NaOH) is a representative of this type of oxide. It is worth noting that some oxides can react with both acids and bases to form salts and water, known as amphoteric oxides. Aluminum oxide - aluminum trioxide (Al ₂ O ∝) is a classic example.