Chemistry
30 flashcards
~15 min
Chemistry of Metals and Alloys
This deck explores the properties and behavior of metals: how metallic bonding gives rise to conductivity and malleability, how metals are extracted from their ores using methods matched to their reactivity, why metals corrode and how corrosion is prevented, a...
About this deck
This deck explores the properties and behavior of metals: how metallic bonding gives rise to conductivity and malleability, how metals are extracted from their ores using methods matched to their reactivity, why metals corrode and how corrosion is prevented, and how alloys like steel, brass, and bronze are engineered for specific properties. A practical companion to periodic table and reactivity-series topics for GCSE, A-Level, and general chemistry learners.
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A type of bonding where positive metal ions are held together in a lattice by a "sea" of delocalized electrons that are free to move throughout the structure.
Because their delocalized electrons can move freely through the metal lattice, carrying electric charge.
Because the layers of metal ions can slide over one another without breaking the metallic bonds, allowing metals to be bent, hammered, or drawn into wires.
A ranking of metals by how readily they react (lose electrons to form positive ions), from most reactive (e.g., potassium) to least reactive (e.g., gold).
Highly reactive metals require electrolysis; moderately reactive metals are extracted by reduction with carbon; unreactive metals occur naturally and need little processing.
Because these metals are too reactive to be reduced by carbon, so molten ionic compounds must be broken down using electrical energy instead.
Carbon is more reactive than iron so it can reduce iron oxide, but carbon is less reactive than aluminum so it cannot reduce aluminum oxide.
Unreactive metals such as gold and platinum that are found in the Earth's crust in their pure elemental form, requiring no chemical extraction.
Iron ore, coke, and limestone are heated; carbon monoxide reduces iron oxide to molten iron, while limestone removes acidic impurities as slag.
A highly exothermic reaction between aluminum powder and iron oxide, producing molten iron and aluminum oxide; used for welding railway tracks.
The gradual destruction of a metal through chemical reaction with substances in its environment, most commonly oxygen and water.
The corrosion of iron, forming hydrated iron(III) oxide, which requires both oxygen and water to occur.
Coating iron or steel with a layer of zinc to prevent rusting; the zinc acts as a barrier and, if scratched, corrodes preferentially to protect the iron.
Attaching a more reactive metal (like zinc or magnesium) to a less reactive metal so the more reactive metal corrodes first, protecting the main structure.
A mixture of a metal with one or more other elements (often other metals or carbon), designed to have improved properties compared to the pure metal.
Because atoms of different sizes disrupt the regular lattice structure, preventing layers of atoms from sliding smoothly over each other.
An alloy of iron with a small percentage of carbon (and sometimes other elements), making it stronger and harder than pure iron.
An alloy of iron, carbon, and chromium (often with nickel); chromium forms a thin, unreactive oxide layer that protects the steel from corrosion.
An alloy of copper and zinc, valued for its machinability and golden appearance, commonly used in fittings and musical instruments.
An alloy of copper and tin, known for its hardness and resistance to corrosion, historically used for tools and statues.
A lightweight, strong alloy of aluminum, copper, and other elements, used extensively in aircraft manufacturing.
A naturally occurring rock or mineral from which a metal can be economically extracted.
Using an electric current to deposit a thin layer of one metal onto the surface of another, often for decoration or corrosion resistance.
An alloy of mercury with another metal, historically used in dentistry for fillings.
An industrial method for extracting titanium by reacting titanium tetrachloride with magnesium in an inert atmosphere.
Because in aqueous solution, water can be preferentially reduced/oxidized at the electrodes instead of the metal ion, so molten (solvent-free) electrolytes are needed.
It decomposes to calcium oxide, which reacts with silica impurities to form molten slag, removing them from the molten iron.
It requires large amounts of electrical energy to melt the aluminum oxide (mixed with cryolite to lower its melting point) and drive the electrolysis.
The formation of a thin, adherent oxide layer on a metal's surface (e.g., aluminum oxide) that protects the underlying metal from further corrosion.
Because varying the carbon content and added elements changes the balance of hardness, strength, and flexibility to suit different applications.