Rapid Revision-Metals and Non Metals PDF

- RAPID REVISION - Metals & Non Metals Rapid Revision  Elements Metals Non Metals Metalloids Noble Gas e.g. Gold (Au), Iron (Fe), e.g. Hydrogen (H...

- RAPID REVISION - Metals & Non Metals Rapid Revision  Elements Metals Non Metals Metalloids Noble Gas e.g. Gold (Au), Iron (Fe), e.g. Hydrogen (H), e.g. Boron (B), Silicon e.g. Helium (He), Zinc (Zn), Lead (Pb). Helium (He),Oxygen (O), (Si), Germanium (Ge), Neon (Ne), Argon Antimony (Sb) (Ar) Property Metals Non Metals Malleable (can be hammered). Ex: Aluminium, Iron Malleability Brittle (easily break). Ex: Sulphur, Phosphorus Exceptions : Zinc, Arsenic, Mercury Ductile (can be drawn into wires). Ex: Copper, Al Ductility Not ductile. Ex: Sulphur, Iodine Exceptions: Mercury, Zinc Mostly hard. Ex: Iron, Aluminium Hardness Soft (except diamond). Ecept - sodium and potassium  Property Metals Non Metals Sonorous (produces sound). Ex: Iron, Copper Sonority Non-sonorous. Exceptions: Mercury Lustre Lustrous (shiny). Ex: Gold, Aluminium Dull (except iodine). High. Ex: Tungsten, Gold Melting/Boiling Point Exceptions: Sodium, Potassium, Mercury, Gallium, Low (except diamond). Cesium Good conductor. Ex: Silver, Copper Electrical Conductivity Poor conductor (except graphite). Exceptions: Mercury, Lead Good conductor. Ex: Silver, Copper Heat Conductivity Poor conductor (except graphite). Exceptions: Mercury, Lead State Solid (except mercury). Can be solid, liquid, or gas. Density High density. Ex: Gold, Iron Low density. Ex: Hydrogen, Nitrogen Interesting Facts Mercury is liquid at room temp. Gallium melts in hand. Graphite conducts electricity. Diamond is hardest.  Reactions of Metals and Non Metals Reaction with Metals Non Metals Metal + Oxygen → Metal Oxide (Basic) Example: 2Mg + O₂ → 2MgO Amphoteric Metals: Beryllium (Be), Zinc (Zn), Tin (Sn), Lead (Pb), Aluminium Non-Metal + Oxygen → Non- (Al), (Antimony (Sb) Metal Oxide (Acidic/Neutral) Oxygen Aluminium with Oxygen: 4Al(s) + 3O₂(g) → 2Al₂O₃(s) Example: C + O₂ → CO₂ Zinc with Oxygen: 2Zn(s) + O₂(g) → 2ZnO(s) S + O₂ → SO₂ Aluminium Oxide Reactions: 1. Al₂O₃(s) + 6HCl(aq) → 2AlCl₃(aq) + 3H₂O(l) 2. Al₂O₃(s) + 2NaOH(aq) → 2NaAlO₂(aq) + H₂O(l) Metal + Water → Metal Hydroxide + H₂ Na₂O, K₂O, CaO, and MgO dissolve in water to form metal hydroxides Non metals don’t react with water Example: 2Na + 2H₂O → 2NaOH + H₂ Non-Metal Oxide + Water → Acid K, Na react violently with water; Ca reacts mildly; SO₂ + H₂O → H₂SO₃ Water Ca+2H2​O→Ca(OH)2​+H2​ SO₃ + H₂O → H₂SO₄ Mg reacts with hot water. Al, Fe, Zn react with steam; CO₂ + H₂O → H₂CO₃ 2Al+3H2​O (steam)→Al2​O3​+3H2​ NO₂ + H₂O → HNO₃ + HNO₂ 3Fe+4H2​O (steam)→Fe3​O4​+4H2 Pb, Cu, Ag, Au do not react with water.  Reaction with Metals Non Metals Metal + dil. Acid → Salt + H₂ Example: Zn + 2HCl → ZnCl₂ + H₂ Hydrogen gas isn't produced when metals react with HNO₃ because it oxidizes H₂ to water and reduces to nitrogen oxides. Only Mg and Mn with very dilute HNO₃ release H₂ gas. Metal (Mg and Mn) + Dilute nitric acid → Salt + Hydrogen gas Acids 2Mg + 4HNO₃ → 2Mg(NO₃)₂ + H₂ No Reaction Mn + 2HNO₃ → Mn(NO₃)₂ + H₂ Other Metals + Dilute nitric acid → Salt + Water + NO₂/N₂O/NO Aqua regia is a mix of concentrated hydrochloric and nitric acids in a 3:1 ratio. It’s highly corrosive and can dissolve gold and platinum. More reactive metals displace less reactive metals from their salt solutions (displacement reaction). Metal Salts No Reaction Metal A + Salt solution of B → Salt solution of A + Metal B Example: Pb + CuCl₂ → PbCl₂ + Cu Reactivity Series  Reactions of Metals + Non Metals When metals react with non-metals, electrons transfer from metals to non-metals, forming ions. The compound formed is ionic. Metal + Non-metal → Ionic compound Sodium loses 1 electron, forming Na+ cation. Chlorine gains that electron, forming Cl- anion. Opposite charges attract. Strong electrostatic forces hold them together. Ionic bond forms due to electrostatic attraction between the ions. Sodium chloride (NaCl) is formed.  Property Description Properties Physical nature Solid, hard, brittle due to strong ionic bonds. of Ionic Melting & Boiling points High, due to strong inter-ionic attractions requiring more energy to break. Compounds Solubility Soluble in water, insoluble in organic solvents like kerosene and petrol. Electrical conductivity Conducts in molten and aqueous states, not in solid due to immobile ions. Metallurgy: Science & tech of metals' properties, production, purification Minerals: Naturally occurring elements/compounds in Earth's crust Ores: Minerals from which metals can be extracted economically and conveniently Gangue Particles: Impurities in ores (sand, oil, etc.) Enrichment of Ore/Concentration: Process of removing gangue particles from ores  Minerals Ores Elements or compounds occurring naturally in Earth's Minerals with a high percentage of metal, profitable for extraction. crust. May or may not contain metals. Definitely contain metals. All minerals are not ores. All ores are minerals. Example: Salt, Clay, Marble Example: Bauxite, Hematite, Rock Salt K (Potassium) Na (Sodium) Highly reactive metals (K, Na, Ca, Mg, Ca (Calcium) Electrolysis Mg (Magnesium) Al) are extracted using electrolysis. Al (Aluminum) Zn (Zinc) Moderately reactive metals (Zn, Fe, Fe (Iron) Reduction using carbon Pb) are usually extracted through Pb (Lead) carbon reduction. Cu (Copper) Metals like gold and silver are Ag (Silver) Found in native state Au (Gold) found in a free state due to low reactivity.  Metallurgy Reactivity Metals Process Key Reactions 1. HgS + O₂ → HgO + SO₂ 2. HgO → Hg + O₂ Low Reactivity Mercury (Hg), Copper (Cu) Reduction by heating 3. Cu₂S + O₂ → CuO + SO₂ Cu₂O + Cu₂S → Cu + SO₂ Roasting (for sulphides), 1. ZnS + O₂ → ZnO + SO₂ Medium Zinc (Zn), Iron (Fe), Lead Calcination (for 2. ZnCO₃ → ZnO + CO₂ Reactivity (Pb) carbonates) 3. ZnO + C → Zn + CO Reduction using carbon MnO₂ + Al → Mn + Al₂O₃ or displacement Fe₂O₃ + Al → Fe + Al₂O₃ (Thermit reaction- highly exothermic) Sodium (Na), Magnesium 1. Na⁺ + e⁻ → Na High Reactivity (Mg), Calcium (Ca), Electrolytic reduction 2. 2Cl⁻ → Cl₂ + 2e⁻ Aluminium (Al) 3. Al₂O₃ (electrolysis) → Al Acche se dekhlena reactions!  Cathode : Na⁺ + e⁻ → Na Electrolytic Reduction Anode : 2Cl⁻ → Cl₂ + 2e⁻ Refining of Metals Electrolytic refining is widely used for impure metal is the anode purification. Metals like copper, zinc, tin, nickel, silver, gold are Electrolyte refined using this method. pure metal is the cathode Insoluble impurities form anode mud, while soluble ones stay in the solution.  Roasting Calcination Heating of a metal ore in the presence of excess air or oxygen. Heating of a metal ore in the presence of limited air or oxygen. Requires an excess amount of air or oxygen. Done with limited air or oxygen. Mainly done for sulphide ores. Done for carbonate ores. Releases toxic gases and substances (e.g., SO₂). Releases volatile compounds, often less toxic than in roasting. Corrosion Metal Reaction/Result Prevention Methods Chemical Reaction Turns black when exposed to air due to the Painting, oiling, greasing, galvanizing, Silver 4Ag + 2H₂S + O₂ → 2Ag₂S + 2H₂O formation of silver sulphide. chrome plating, anodizing, alloying Gains a green coat (copper carbonate) when Galvanization (coating with zinc), Cu + H₂O + O₂ + CO₂ → Copper reacting with moist carbon dioxide. Alloying (e.g., stainless steel) CuCO₃·Cu(OH)₂ (green) Forms a brown flaky substance (rust) when Galvanization, alloying, painting, oiling, Fe + O₂ + H₂O → Fe₂O₃·xH₂O Iron exposed to moist air. greasing (rust)  Alloying An alloy is a mixture of metals or a metal with a non-metal, altering properties like conductivity and melting point. Examples : Brass (Copper + Zinc) and Bronze (Copper + Tin) are poor conductors, unlike Copper, which powers electrical circuits. Solder (Lead + Tin) melts easily, making it perfect for welding electrical wires. Pure gold is soft, so it is alloyed with silver or copper to make jewelry, typically in 22 carat form in India. The Iron Pillar near Qutub Minar in Delhi, over 1600 years old, resists rust due to ancient Indian metallurgy techniques Class 10th Phodenge!