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Oxides are binary compounds of oxygen with another element (E–O), where oxygen is typically in the −2 oxidation state. They range from ionic solids to covalent molecules and are fundamental in minerals, materials, and redox chemistry.
Aluminium Oxide - Aluminium (III) Oxide - Al2O3 - Aloxide - Aloxite - Alumina Powder - 1000g
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Aluminium Oxide - Aluminium (III) Oxide - Al2O3 - Aloxide - Aloxite - Alumina Powder - 100g
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Aluminium Oxide - Aluminium (III) Oxide - Al2O3 - Aloxide - Aloxite - Alumina Powder - 25 000g
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Aluminium Oxide - Aluminium (III) Oxide - Al2O3 - Aloxide - Aloxite - Alumina Powder - 5000g
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Aluminium Oxide - Aluminium (III) Oxide - Al2O3 - Aloxide - Aloxite - Alumina Powder - 500g
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Antymonu (III) Tlenek Antimony Trioxide Pure 25g
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Chromium (III) Oxide Cr2O3 Chromium Green Pigment - 1000g
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Colloidal Silica Aerosil 200 Original for Catalysts, Resins - 1000g = 20L
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Oxides are broadly categorized by bonding, composition, and acid–base behavior:
Bonding/structure types.
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Ionic oxides form with electropositive metals (e.g., Na₂O, CaO). They consist of O²⁻ and metal cations in extended lattices, often high-melting and basic.
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Covalent oxides form with nonmetals or high-oxidation-state metals (e.g., CO₂, SO₃, SiO₂). These feature directional E–O bonds and may exist as discrete molecules (CO₂) or giant networks (SiO₂).
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Mixed/metallic oxides of transition metals often have partial covalency and variable stoichiometry (e.g., Fe₃O₄, TiO₂), enabling rich electronic and catalytic properties.
Acid–base classification.
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Basic oxides (mostly metal oxides) react with acids to form salts and water; in water they generate hydroxides (CaO → Ca(OH)₂).
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Acidic oxides (mostly nonmetal oxides) are anhydrides of oxoacids and react with bases (SO₃ → H₂SO₄; CO₂ → H₂CO₃).
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Amphoteric oxides (e.g., Al₂O₃, ZnO, SnO₂) react with both acids and strong bases, reflecting intermediate metal–oxygen bonding and Lewis acidity/basicity.
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Neutral oxides (e.g., CO, N₂O) show little acid–base character.
Oxidation states and nonstoichiometry.
While oxygen is usually −2, exceptions occur in peroxides (O₂²⁻, −1 each O), superoxides (O₂⁻, −½ each O), and ozonides (O₃⁻). Many transition-metal oxides are nonstoichiometric due to oxygen vacancies or mixed valence (e.g., Fe²⁺/Fe³⁺ in Fe₃O₄), which strongly affects conductivity and magnetism.
Formation and reactivity.
Oxides form via direct oxidation of elements, thermal decomposition of hydroxides/carbonates, or controlled redox routes. Their reactivity includes:
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Redox behavior in metallurgy and energy materials (e.g., Fe₂O₃ reduced to Fe in blast furnaces).
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Surface chemistry and catalysis, especially for transition-metal oxides that adsorb/reactivate small molecules (CO oxidation on MnOₓ, TiO₂ photocatalysis).
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Hydration and carbonation (CaO + H₂O → Ca(OH)₂; CaO + CO₂ → CaCO₃), crucial in cement chemistry and carbon sequestration.
Properties and applications.
Oxides underpin ceramics, glasses, semiconductors (SiO₂, TiO₂, ZnO), battery electrodes (LiCoO₂, MnO₂), pigments, and protective passivation layers (Al₂O₃, Cr₂O₃). Their mechanical hardness, thermal stability, electronic band structures, and ionic transport make them central to both geology and modern technology.