Metals and Non metals FULL CHAPTER | Class 10th Science | Chapter 3 | Udaan

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The lecture on metals and non-metals covers various elements, properties, and reactions, emphasizing the differences between metals and non-metals, their physical and chemical properties, and how they interact with other elements. It discusses the reactivity series, the formation of oxides, and how to extract and refine metals using different processes, focusing on techniques like roasting, calcination, and electrolyte refinement to obtain pure metals and prevent corrosion.

Insights

  • The lecture delves into the classification of elements into metals and non-metals, highlighting common examples like Lithium, Sodium, and Gold for metals, and Carbon and Hydrogen for non-metals.
  • Metalloids, also known as semi-metals, exhibit properties that share characteristics of both metals and non-metals, contributing to their unique classification.
  • The physical properties of metals, such as shine and malleability, contrast with non-metals, known for being brittle and easily breakable, except for exceptions like Iodine and Graphite.
  • Metals conduct electricity due to free electrons, while heat conduction in solids is attributed to atomic vibrations, with exceptions like Lead and Mercury.
  • The reactivity series aids in determining the order of reactivity of metals, showcasing a hierarchy from highly reactive metals like Potassium and Sodium to the least reactive ones like Silver, Gold, and Platinum.
  • Corrosion, a surface degradation process triggered by atmospheric gases, leads to the formation of stable oxide, sulphide, or carbonate layers on metals, with rusting being a notable concern due to its cyclic nature and impact on metal integrity.

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Recent questions

  • What are the physical properties of metals and non-metals?

    Metals exhibit shine and malleability, while non-metals are brittle and break easily. Metals are generally hard, while non-metals are soft, making them easy to wear but difficult to cut or rub. Exceptions include Lithium, Sodium, and Potassium, which can be easily cut with a knife and even touched with bare hands. Diamond, a form of carbon and a non-metal, is naturally hard and grows in nature, making it the hardest substance found in the earth's crust. Hardness is a property defined only for solids, not for liquids or gases, with Mercury being an exception as it is a liquid. Metals exhibit metallic luster, reflecting light to create a shiny surface, while non-metals are generally dull, with exceptions like Iodine and Graphite. Malleability is the ability of metals to be converted into thin sheets under compressive forces, with Mercury and Zinc being exceptions at room temperature. Ductility refers to the ability of metals to be converted into thin wires under tensile forces, with Carbon Fiber being an exception among non-metals. Sonority is the ability of metals to produce sound when struck hard, with metals being sonorous and non-metals being non-sonorous.

  • How do metals react with oxygen?

    Metals like Magnesium, Aluminum, Zinc, Iron, and Lead react with oxygen to form their respective oxides at room temperature or low heating, without producing flames or light energy. Zinc reacts moderately with oxygen to form zinc oxide, burning with a light blue flame. Iron reacts slowly with oxygen to form iron oxide, producing sparks but no flames. Lead and Copper are less reactive, forming lead oxide and copper oxide without generating flames or light energy. Potassium and Sodium react with oxygen at room temperature to form potassium oxide and sodium oxide, burning with orange or golden yellow flames. Calcium, Magnesium, Aluminum, Zinc, Iron, and Lead form their respective oxides at room temperature or low heating, without producing flames or light energy. These reactions showcase the varying reactivity levels of metals when exposed to oxygen.

  • What is the reactivity series of metals?

    The reactivity series helps in determining the order of reactivity of metals. Potassium and Sodium are the most reactive metals, while Silver, Gold, and Platinum are the least reactive. Aluminum, Zinc, and Iron are more reactive than Lead and Copper, with Zinc and Iron producing flames and light energy. The reactivity series order is Potassium, Sodium, Calcium, Magnesium, Aluminum, Zinc, Iron, Lead, Copper, Mercury, Silver, Gold, and Platinum. This series provides a structured way to understand how metals interact with other elements and compounds based on their reactivity levels.

  • How are metals extracted from ores?

    The process of extracting metals from ores involves several steps. Initially, the material is crushed and ground to convert it into a powdered form. Concentration, dressing, or benefaction is crucial for removing impurities and increasing the material's concentration. Gangue and matrix, which are earthy and rocky impurities associated with minerals, need to be removed before extracting the metal. Separating impurities based on physical and chemical properties is essential, using techniques like magnetic separation. The process involves converting carbonate and sulfide ores into oxides before reducing them to obtain the metal. Roasting the metal sulfide in the presence of oxygen helps in converting it into metal oxide. Reduction involves removing oxygen from the metal oxide to obtain the metal, a process known as auto-reduction. The final steps include refining the metal and repeating the process of converting sulfide into oxide for extraction. These steps outline the systematic approach to extracting metals from ores efficiently.

  • How does the process of electrolyte refinement work?

    Electrolyte refinement is a method used to remove impurities from metals through electrolysis. The process involves connecting a thick copper block to the positive terminal as an anode and a thin strip of pure copper to the negative terminal as a cathode. The electrolyte dissociates into copper and sulfate ions, with copper ions gaining electrons at the cathode and forming pure copper, while the anode loses electrons, gradually becoming thinner. Two types of impurities in copper are soluble and insoluble, with soluble impurities like iron becoming Fe2+ in solution by losing electrons, and insoluble impurities like silver and gold not dissolving in the electrolyte. This method allows for the purification of metals by selectively removing impurities through controlled electrolysis, resulting in refined and high-quality metal products.

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Summary

00:00

"Metals, Non-Metals, and Metalloids Explained"

  • The recipe involves attending a high-level academy for content and concept clarity, followed by creativity and experimentation.
  • The lecture focuses on the chapter "Metals and Non-Metals," covering elements, physical properties, reactivity series, chemical properties, ionic compounds, and corrosion.
  • Elements are categorized into metals (dhatu) and non-metals, with common metals like Lithium, Sodium, and Gold, and non-metals like Carbon and Hydrogen.
  • Non-metals include Carbon, Phosphorus, and Sulfur in solid states, while Hydrogen, Nitrogen, and Chlorine are in gaseous states.
  • Bromine is a non-metal found in liquid state, while Mercury is the only metal in liquid state at room temperature.
  • Metalloids, or semi-metals, have properties showing characteristics of both metals and non-metals.
  • Metal properties include shine and malleability, while non-metals are brittle and break easily.
  • Six commonly recognized metalloids are Antimony, Arsenic, Germanium, Silicon, Tellurium, and Polonium.
  • Noble gases, previously called inert gases, are unreactive compared to other elements, with a mnemonic to remember their names.
  • Physical properties of metals and non-metals are studied based on their outer appearance and behavior, with mercury being the only metal in liquid state and bromine the only non-metal in liquid state at room temperature.

19:34

Metals vs Non-Metals: Properties and Exceptions

  • Metals are generally hard, while non-metals are generally soft, making them easy to wear but difficult to cut or rub.
  • Exceptions to this rule include Lithium, Sodium, and Potassium, which can be easily cut with a knife and even touched with bare hands.
  • Diamond, a form of carbon and a non-metal, is naturally hard and grows in nature, making it the hardest substance found in the earth's crust.
  • Hardness is a property defined only for solids, not for liquids or gases, with Mercury being an exception as it is a liquid.
  • Metals exhibit metallic luster, reflecting light to create a shiny surface, while non-metals are generally dull, with exceptions like Iodine and Graphite.
  • Malleability is the ability of metals to be converted into thin sheets under compressive forces, with Mercury and Zinc being exceptions at room temperature.
  • Ductility refers to the ability of metals to be converted into thin wires under tensile forces, with Carbon Fiber being an exception among non-metals.
  • Sonority is the ability of metals to produce sound when struck hard, with metals being sonorous and non-metals being non-sonorous.
  • Metals conduct electricity due to the presence of free electrons, while heat conduction in solids occurs due to atomic vibrations, with exceptions like Lead and Mercury.
  • The melting point of metals is generally high, with exceptions like Cesium having very low melting points, causing them to melt on human palms at room temperature.

37:17

Metal wire properties and conductivity testing results.

  • Heat the wire near the clamp with a spirit lamp candle and a burner.
  • Observe the wire after heating and note any changes.
  • The metal wire will fall down after heating near the clamp.
  • The heat flows through the wire and melts the wax, causing the pin to fall.
  • The wire does not melt even after prolonged heating, indicating high melting points of metals.
  • Gold is the most malleable metal, while platinum is the most ductile.
  • Silver is the best conductor of heat among metals, followed by copper.
  • Diamond is the best conductor of heat overall.
  • Silver is the best conductor of electricity among metals, followed by copper and gold.
  • Silver and gold wires are not commonly made due to their rarity and high cost.

54:28

Metal Oxides: Reactions and Properties

  • Magnesium reacts with oxygen in the air to form a white layer of magnesium oxide.
  • Before burning magnesium, it needs to be sanded with paper to remove the magnesium oxide layer.
  • Heating magnesium strongly in the presence of oxygen produces white powder, magnesium oxide, along with heat and light energy.
  • Potassium and sodium react with oxygen at room temperature to form potassium oxide and sodium oxide, burning with orange or golden yellow flames.
  • Calcium, magnesium, aluminum, zinc, iron, and lead form their respective oxides at room temperature or low heating, without producing flames or light energy.
  • Zinc reacts moderately with oxygen to form zinc oxide, burning with a light blue flame.
  • Iron reacts slowly with oxygen to form iron oxide, producing sparks but no flames.
  • Lead and copper are less reactive, forming lead oxide and copper oxide without generating flames or light energy.
  • Potassium and sodium are the most reactive metals, while silver, gold, and platinum are the least reactive.
  • Aluminum, zinc, and iron are more reactive than lead and copper, with zinc and iron producing flames and light energy.

01:11:58

Metal Oxides: Acid-Base Behavior and Reactions

  • An amphoteric oxide behaves as both an acid and a base, exemplifying a neutralization reaction.
  • Metal oxides and hydroxides can be amphoteric, basic, or acidic.
  • When metals react with water, they form oxides and release hydrogen gas.
  • Reactivity determines the displacement reaction between metals and non-metals.
  • Displacement reactions often involve redox reactions.
  • Heat released during reactions can cause hydrogen gas to catch fire.
  • Soluble oxides form hydroxides when reacting with water.
  • Potassium reacts more rapidly with water than sodium due to higher reactivity.
  • Calcium reacts with water, displacing hydrogen and forming oxides.
  • Metals like potassium, sodium, and calcium react with cold water, releasing hydrogen gas and forming oxides.

01:29:22

Metal Reactivity and Acid Reactions Explained

  • Potassium, sodium, and calcium are highly reactive metals.
  • To determine the reactivity order, observe the amount of bubbles produced when reacting with dilute acid.
  • Sodium and potassium are stored in kerosene or mineral oil to prevent contact with air and moisture, which can cause them to catch fire.
  • Aluminum is used for utensils due to its high heat conductivity, melting point, and self-protective nature.
  • Reactivity of metals with dilute acids can be determined by observing the rate of effusion of hydrogen gas.
  • Magnesium, aluminum, zinc, iron, and lead react with dilute hydrochloric acid in decreasing order of reactivity.
  • The reaction of metals with dilute nitric acid results in the formation of salt and hydrogen gas, with magnesium and manganese showing exceptions.
  • Aqua Regia is a mixture of concentrated nitric acid and hydrochloric acid in a 1:3 ratio, used to dissolve gold and platinum due to its corrosive nature.

01:46:44

"Reactivity Series Determines Metal Reactivity Order"

  • Aqua regia is used to dissolve gold, creating a shining surface.
  • Chemical reactions help in obtaining gold back after it has dissolved.
  • Reactivity series helps in determining the order of reactivity of metals.
  • Displacement reactions show which metal is more reactive than the other.
  • Lead is proven to be more reactive than copper through reactions.
  • Copper is more reactive than silver, which is more reactive than gold.
  • Silver is found in both free and combined states, while gold is always in the free state.
  • The reactivity series order is potassium, sodium, calcium, magnesium, aluminum, zinc, iron, lead, copper, mercury, silver, gold, platinum.
  • Platinum is placed after hydrogen due to its behavior as a metal.
  • Non-metal oxides can be acidic or neutral, like CO2, SO2, SO3, CO, H2O, N2O.

02:03:54

Formation and Properties of Ionic Compounds

  • Sodium chloride is formed by sodium losing an electron and chlorine gaining an electron to become stable.
  • Magnesium chloride is created by magnesium losing two electrons and chlorine gaining one electron for stability.
  • Lewis electron dot or cross symbol is used to represent the structure of compounds like mgcl2.
  • Ionic compounds are brittle solids that break under pressure due to repulsion between like charges.
  • Ionic compounds have high melting and boiling points due to strong electrostatic forces between opposite charges.
  • Ionic compounds are generally soluble in water, except for exceptions like baso4, pb2, and caco3.
  • Ionic compounds conduct electricity in molten or aquas form due to free movement of ions.
  • Solid ionic compounds do not conduct electricity as ions are immobile, unlike in molten or aquas form.
  • Metallurgy is the branch of science focused on economically extracting metals from compounds.
  • Metals obtained from sea water are in the form of water-soluble salts, which are ionic compounds.

02:21:15

Metals in Earth's Crust and Sea Water

  • Metals can be found in free state or combined state in the crust of the earth.
  • Some metals like sodium and potassium form soluble salts found in sea water.
  • Metals can be found in free state (elemental form) or combined form (compound form).
  • Metals are found in the crust of the earth and in sea water in the form of soluble salts.
  • Metals like potassium, sodium, calcium, magnesium, and aluminum are highly reactive and are found in combined form.
  • Metals like copper, mercury, and silver are of medium reactivity and can be found in both free and combined forms.
  • Gold and platinum, being the least reactive metals, are found in free state (elemental form).
  • Minerals occur naturally in the form of elements or compounds in the earth's crust and sea water.
  • Earthy and rocky impurities associated with minerals are called gang or matrix.
  • Minerals from which metals can be economically and conveniently extracted are called ores.

02:40:06

Metal Extraction Process for Low Reactivity Metals

  • The first step is crushing the material, followed by grinding it to convert it into a powdered form.
  • The process involves attrition to break the material into smaller pieces before turning it into powder.
  • Concentration, dressing, or benefaction is crucial for removing impurities and increasing the material's concentration.
  • Gangue and matrix need to be removed before extracting the metal, emphasizing the importance of cleaning.
  • Separating impurities based on physical and chemical properties is essential, using techniques like magnetic separation.
  • The process involves converting carbonate and sulfide ores into oxides before reducing them to obtain the metal.
  • Roasting the metal sulfide in the presence of oxygen helps in converting it into metal oxide.
  • Reduction involves removing oxygen from the metal oxide to obtain the metal, a process known as auto-reduction.
  • The final steps include refining the metal and repeating the process of converting sulfide into oxide for extraction.
  • The process is detailed for low reactivity metals like copper and mercury, emphasizing the steps of crushing, grinding, roasting, and auto-reduction.

02:56:15

Metal Ore Processing Methods and Reduction Techniques

  • Found in oxide, sulphide, and carbonates formats
  • Crushing and grinding of sugar and concentration of ore are the initial steps
  • Crushing and grinding, followed by concentration, are common in both cases
  • Sulphide and carbonate will form oxide
  • Carbonates need to be removed first if present in excess
  • Roasting for sulphide and calcination for carbonate
  • Roasting for sulphide, calcination for carbonate
  • Metal sulphide undergoes roasting, while carbonate undergoes calcination
  • Reduction of metal oxide by carbon or coke in smelting
  • Aluminum used as a reducing agent in thermite process for metal oxide reduction

03:14:02

Metal Extraction and Refinement Techniques Explained

  • Metal displacement reactions involve redox reactions with assorted metals of medium reactivity.
  • Steps include crushing and grinding, concentration, roasting for sulphides, and calcination for carbonates to form metal oxides.
  • Reduction of metal oxides to metals can be done through smelting with coke or aluminothermy using aluminum.
  • High reactivity metals like potassium, sodium, calcium, magnesium, and aluminum require specific extraction methods.
  • Chlorides and oxides of highly reactive metals are stable and cannot be reduced by typical agents due to their affinity for oxygen or chlorine.
  • Electrolyte reduction involves giving electric shocks to separate metals like sodium and chlorine.
  • Refinement of metals involves removing impurities through electrolyte refinement processes.
  • Electrolyte refinement can be done using copper sulfate solution or acidified copper sulfate.
  • The process involves connecting a thick copper block to the positive terminal as an anode and a thin strip of pure copper to the negative terminal as a cathode.
  • The electrolyte dissociates into copper and sulfate ions, with copper ions gaining electrons at the cathode and forming pure copper, while the anode loses electrons, gradually becoming thinner.

03:34:23

"Metals, Impurities, and Corrosion: A Summary"

  • Two types of impurities in copper: soluble and insoluble
  • Copper accepts electrons and donates electrons in reactions
  • Anode in electrolysis process gets thinner and thicker due to errors
  • Soluble impurities like iron become Fe2+ in solution by losing electrons
  • Insoluble impurities like silver and gold do not dissolve in electrolyte
  • Process of refining low reactivity metals involves crushing, grinding, and roasting
  • Corrosion is a surface degradation process caused by atmospheric gases
  • Metals form stable oxide, sulphide, or carbonate layers due to electron exchange
  • Rusting of iron occurs due to reaction with oxygen and water, forming hydrated ferric oxide
  • Positive corrosion types like patina on copper and silver create protective layers, preventing further corrosion

03:53:08

Preventing Rust Formation with Protective Barriers

  • Rusting is a significant issue as it forms a crust on metal, exposing the metal underneath, leading to a cyclic process of rust formation due to lack of oxygen and moisture.
  • The process of rust peeling off occurs because it forms a non-sticky layer that falls off, exposing fresh iron to oxygen and moisture, leading to a continuous weakening of the metal.
  • To prevent rusting, three types of barriers can be used: barrier protection, sacrificial protection, and alloy protection, with barrier protection involving introducing a layer between iron and factors causing rusting, like paint or grease.
  • Sacrificial protection involves placing a layer of more reactive metal over less reactive metal, preventing oxygen and water from reaching the iron, thus protecting it from corrosion.
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