1. Common properties and uses of metals. 2. Corrosion and rusting. 3. The reactions of metals with water. 4. The reactions of metals with acids. 5. The properties of alloys and their use.
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Alloys -> Mixture of two or more metals
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Increased Strength: Alloys are usually stronger than pure metals, making them suitable for construction and manufacturing.
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Improved Resistance to Corrosion: Many alloys, like stainless steel, resist rust and corrosion better than the base metal.
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Enhanced Hardness: Alloys are often harder than the metals they are made from, which helps in making cutting tools and machinery.
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Tailored Magnetic or Lightweight Properties: Certain alloys are used for their magnetic properties (like alnico) or light weight (like aluminum alloys in aircraft).
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Better Heat and Electrical Properties: Some alloys are designed to have specific heat or electrical conductivity, like nichrome for heating elements.
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Metal + Water -> Metal Hydroxide + Hydrogen
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Mg(s) + 2H2O(I) -> Mg(OH)2 (aq*) + H2 (g)
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Metal + Oxygen -> Metal Oxide
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2Mg(s) + O2 (g) -> 2MgO(S)
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Conductors of heat and electricity (copper, electrical wiring)
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Malleable and Ductile (aluminum, airplanes and cans)
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High melting points and are solid at room temperature, except mercury (iron, cooking pans)
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Shiny (gold and silvers, jewelry and electronics)
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Strong and Durable (iron and steel, buildings and machines)
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Rusting -> chemical reaction where iron reacts with oxygen and water to form a reddish-brown substance called rust. Occurs because of oxidation.
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Corrosion -> Formation of compounds of metals due to oxidation reaction.
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Prevent -> Painting/coating, Galvanization, Stainless steel, Powder coating
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Factors Influencing -> High temperature, acidic PH, oxygen, high flow velocity
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Aluminum & Titanium -> Form an oxide layer to be stronger (Does not weaken the iron structure)
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Metal + Acid -> Salt + Hydrogen gas
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Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g)
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Hydrochloric Acid
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Chloride
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Sulfuric Acid
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Sulfate
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Nitric Acid
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Nitrate
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