Class X Science: Metals and Non-metals PDF

# Class X - Science: Metals and Non-metals ## PK Hits - Chemical properties of metal - Reactivity series (give reasons type of questions) - Exceptional cases (***HNO***₃ reaction with metals) - Metallurgy - Calcination/Roasting - Electrolytic refining ## Properties of elements | Eleme...

# Class X - Science: Metals and Non-metals ## PK Hits - Chemical properties of metal - Reactivity series (give reasons type of questions) - Exceptional cases (***HNO***₃ reaction with metals) - Metallurgy - Calcination/Roasting - Electrolytic refining ## Properties of elements | Element type | Description | Examples | |---|---|---| | Metals | Elements that form positive ions by losing electrons | Sodium, Aluminum, Silver | | Non-metals | Elements that typically gain electrons to form negative ions or share electrons | Carbon, Sulfur, Oxygen, Nitrogen | | Metalloids | Elements with properties intermediate between metals and non-metals that can exhibit both behaviors | Silicon, Boron | | Inert elements | Elements with a stable electronic configuration, found in group 18 of the periodic table that rarely react | Helium, Neon, Argon | ### Visual representation of elements - **Gold** - A piece of gold with a golden color - **Copper** - A piece of copper with a reddish-brown color - **Diamond** - A diamond with a clear, crystalline structure - **Carbon** - A diagram of a carbon dioxide molecule (CO₂) - **Silicon** - A diagram of Silicon (Si) - **Boron** - A diagram of Boron - **Helium** - A diagram of a Helium atom (He) - **Argon** - A diagram of an Argon atom (Ar) ## Physical properties of metals and non-metals | Property | Metals | Non-metals | |---|---|---| | Hardness | Generally hard, except sodium and potassium | Generally soft, except diamond | | Lustre | Lustrous (shiny appearance) | Non-lustrous, except iodine | | Malleability | Malleable (can be beaten into sheets), except mercury | Non-malleable, brittle | | Ductility | Ductile (can be drawn into wires), except mercury | Non-ductile | | Sonority | Sonorous (produce sound when struck) | Non-sonorous | | Electrical conductivity | Good conductors of electricity | Poor conductors, except graphite | | Heat conduction | Good conductors of heat, except lead | Poor conductors of heat | | Melting Point | High melting point, except gallium | Low melting point | ## Facts and exceptions about metals - Metals are hard except alkali metals like sodium, potassium, lithium, which can be cut with a knife - **Gold** is the most malleable metal, while platinum is the most ductile metal (but costly) - Silver is the best conductor of electricity - The only metal found in liquid at room temperature is mercury (***Hg***) - used in thermometers - Gallium and Cesium have low melting points due to which they melt in the human palm ## Facts and exceptions about non-metals - The only non-metal found in liquid is bromine - Diamond is the hardest naturally occurring substance and it is the best conductor of heat. Non-metals also have very unique characteristics - Graphite and iodine are lustrous - Graphite is a good conductor of electricity ## Chemical properties of metals ### 1. Reaction with air (oxygen) Almost all metals combine with oxygen to form metal oxides. *Metal + Oxygen → Metal oxide* For example: *2Cu + O₂ → 2CuO* (black substance) Most other metal oxides are insoluble in water. Sodium and potassium oxides dissolve in water to form alkalis: *Base* *Na₂O + H₂O → 2NaOH* *K₂O + H₂O → 2KOH* ### 2. Reaction with water - Metals react with water and produce a metal oxide and hydrogen gas. - Metal oxides that are soluble in water dissolve in it to further form metal hydroxide. - However, all metals do not react with water. *Metal + Water → Metal oxide + Hydrogen* For example: *2Na (s) + 2H₂O (l) → 2NaOH (aq) + H₂ (g) + Heat* Oxides like Na₂O, K₂O, CaO, and MgO are soluble in water and form metal hydroxides. *Metal oxide + Water → Metal hydroxide* ### 3. Reaction with acids Metals react with acids to give a salt and hydrogen gas. *Metal + Dilute acid → Salt + Hydrogen* - Hydrogen gas (***H***₂) is not evolved when a metal reacts with nitric acid (***HNO***₃). This is because ***HNO***₃ is a strong oxidizing agent. It oxidizes the ***H***₂ produced to water and itself gets reduced to any of the nitrogen oxides (***N***₂***O***, ***NO***, ***NO***₂). - However, magnesium (***Mg***) and manganese (***Mn***) react with very dilute ***HNO***₃ to evolve ***H***₂ gas. - Copper (***Cu***) does not react with dilute hydrochloric acid (***HCl***). ### 4. Reaction of metals with other metal salts Reactive metals can displace less reactive metals from their compounds in solution or molten form. It is a displacement reaction. *Metal A + Salt solution of B → Salt solution of A + Metal B* ### Reactivity series This helps determine which metal will displace another. - ***K*** - Potassium (Most reactive) - -Sodium - -Calcium - -Magnesium - -Aluminium - -Zinc - -Iron - -Lead - -Copper - -Hydrogen] - -Mercury - -Silver - -Gold (Least reactive) ## Chemical properties of non-metals ### 1. Reaction with air (oxygen) When non-metals react with oxygen, they form non-metal oxides. *Non-metal + Oxygen → Non-metal oxide* For example: *C (s) + O₂ (g) → CO₂ (g)* (***Neutral***) *S (s) + O₂ (g) → SO₂ (g)* (***Acidic***) - Non-metallic oxides are acidic in nature: *CO₂, SO₂, SO₃* etc. - Non-metallic oxides can also be neutral in nature: *CO, H₂O, N₂O* etc. ### 2. Reaction of non-metal oxide with water Generally, non-metals do not react with water as they cannot displace hydrogen from water. *Non-metal oxide + water → Non-metal oxide* For example: *CO₂ (g) + H₂O (l) → H₂CO₃ (aq)* (***Carbonic Acid***) *SO₃ (g) + H₂O (l) → H₂SO₄ (aq)* *2NO₂ (g) + H₂O (l) → HNO₂ (aq)+ HNO₃ (aq)* ## Reaction of metal and non-metal (ionic compound) When metals react with non-metals, electrons are transferred from the metal atoms to the non-metal atoms, forming ions. The compound formed is called an **ionic compound**. *Metal + Non-metal → Ionic compound* **Example - Common salt (***NaCl***)** - **Sodium atom (***Na***)** - A diagram of a sodium atom with one electron in the outer shell - **Chlorine atom (***Cl***)** - A diagram of a chlorine atom with 7 electrons in the outer shell - **Sodium ion (***Na***⁺)** - A diagram of a sodium ion with a positive charge, having lost one electron - **Chlorine ion (***Cl***^-)** - A diagram of a chlorine ion with a negative charge, having gained one electron - **NaCl** - A diagram of sodium chloride with the sodium and chlorine ions bonded together ## Formation of ionic compound - **Sodium Chloride:** - **Na** - A diagram showing the electron configuration of sodium as *2,8,1* and *Na⁺ + e^-* with electron configuration *2,8* (sodium cation) - **Cl** - A diagram showing the electron configuration of chlorine as *2,8,7* and *Cl + e^-* with electron configuration *2,8,8* (chloride anion) - **Sodium chloride** - A diagram showing the formation of ionic sodium chloride as *Na* loses one electron to *Cl* forming *Na⁺* and *Cl^-* that are attracted to each other, resulting in *NaCl* - **Magnesium Chloride:** - **Mg** - A diagram showing the electron configuration of magnesium as *2,8* and *Mg²⁺ + 2e^-* with electron configuration *2,8* (magnesium cation) - **Cl** - A diagram showing the electron configuration of chlorine as *2,8,7* and *Cl + e^-* with electron configuration *2,8,8* (chloride anion) - **Magnesium chloride** - A diagram showing the formation of ionic magnesium chloride (**MgCl₂**) where *Mg* loses two electrons to two *Cl* atoms, forming *Mg²⁺* and two *Cl^-* ions that are attracted to each other. There is one magnesium ion and two chloride ions, forming *MgCl₂*. ## Ionic bond It is a type of linkage formed from the electrostatic attraction between oppositely charged ions in a chemical compound. ## Properties of ionic compounds - They are solid and hard, generally brittle - They have high melting and boiling points - They are generally soluble in water and insoluble in solvents such as kerosene, petrol, etc. - They conduct electricity in molten and solution form but not in solid state ## Abhay Premier League Abhay Premier League is a quiz-based competition on metals and non-metals. ### 2023 **Q: Aluminium is used for making cooking utensils. Which of the following properties of aluminium are responsible for the same?** (i) Good thermal conductivity (ii) Good electrical conductivity (iii) Ductility (iv) High melting point **Answer: (a) (i) and (ii)** ### 2019 **Q: A metal and a non-metal that exist in liquid state at the room temperature are respectively:** (a) Bromine and Mercury (b) Mercury and Iodine (c) Mercury and Bromine (d) Iodine and Mercury **Answer: (c) Mercury and Bromine** ### 2021 **Q: Which of the following pairs will give displacement reactions?** (a) FeSO₄ solution and Copper metal (b) AgNO₃ solution and Copper metal (c) CuSO4 solution and Silver metal (d) NaCl solution and Copper metal **Answer: (b) AgNO₃ solution and Copper metal** ### 2021 **Q: What is meant by amphoteric oxides? Choose the amphoteric oxides from the following: Na2O, ZnO, CO2, Al2O3, H2O** **Answer:** Amphoteric oxides are those oxides that exhibit both acidic and basic properties, i.e., they react with both acids and bases. From the given options, the amphoteric oxides are: ZnO and Al₂O₃ ### 2022 **Q: An element X is soft and can be cut with a knife. This is very reactive to air and cannot be kept open in air. It reacts vigorously with water. Identify the element from the following:** (a) Mg (b) Na (c) P (d) Ca **Answer: (b) Na** ### 2022 **Q: Aqua regia is a freshly prepared mixture of concentrated HNO₃ and concentrated HCl in the ratio of:** a) 1:3, respectively b) 2:3, respectively c) 3:1, respectively d) 3:2, respectively **Answer: (c) 3:1, respectively** ### 2022 **Q: Name a metal which:** (a) is the best conductor of heat. (b) has a very low melting point. (c) does not react with oxygen even at high temperature. (d) is most ductile. **Answer:** (a) Metal which is the best conductor of heat is silver. (b) Gallium has a very low melting point. (c) Silver and gold do not react with oxygen even at high temperature. (d) Gold is the most ductile metal. ### 2024 **Q: State reasons for the following:** (a) Zinc oxide is an amphoteric oxide. **Answer:** Zinc oxide reacts with both acids and bases to form salts and water, indicating it has both acidic and basic properties, making it amphoteric. **Q: State reasons for the following:** (b) Sodium metal is stored in a bottle filled with kerosene oil. **Answer:** Sodium is highly reactive with water and oxygen, which can cause it to ignite. Storing it in kerosene prevents it from coming into contact with moisture and air, thus preventing accidental ignition. **Q: State reasons for the following:** (c) In the reactions of nitric acid with metals, generally hydrogen gas is not evolved, **Answer:** Nitric acid is a strong oxidizing agent, which means that instead of hydrogen gas, nitrogen oxides are typically produced during the reaction with metals. ### 2024 **Q: (a) Why does calcium start floating when it reacts with water? Write the balanced chemical equation of the reaction.** **Q: (b) Name two metals which do not react with water.** **Answer: (a)** Calcium reacts with cold water to form calcium hydroxide and hydrogen gas. *Ca(s) + 2H₂O(l)^{Room temperature} → Ca(OH)₂(aq) + H₂(g)* The bubbles of hydrogen gas produced, stick to the surface of calcium and hence, it starts floating on the surface of water. **Answer: (b)** Gold and silver do not react with water. ### 2020 **Q: (a) (i) Write two properties of gold which make it the most suitable metal for ornaments.** **Q: (a) (ii) Name two metals which are the best conductors of heat.** **Q: (a) (iii) Name two metals which melt when you keep them on your palm.** **Q: (b) Explain the formation of ionic compound CaO with electron-dot structure.** *(Atomic numbers of calcium and oxygen are 20 and 8 respectively)* **Answer: (a)** **(i)** The malleability and ductility properties of gold make it suitable for ornaments. **(ii)** Silver and gold. **(iii)** Gallium and caesium have so low melting points that they melt even on keeping them on palm. **(b)** - **Calcium atom (Ca)** - A diagram of a calcium atom with a configuration of *2,8,8,2* - **Oxygen atom (O)** - A diagram of an oxygen atom with a configuration of *2,6* - **Calcium ion (Ca²⁺)** - A diagram of a calcium ion with a configuration of *2,8,8* - **Oxide ion (O^2-)** - A diagram of an oxygen ion with a configuration of *2,8* - **Calcium oxide** - A diagram of calcium oxide (CaO) A further diagram shows the transfer of two electrons from calcium to oxygen, resulting in the formation of an ionic compound, *Ca²⁺O^2-* ## Metallurgy The branch of science and technology concerned with the properties of metals and their production and purification. ### Minerals - Natural occurring chemical substances obtained by mining ### Ores - An ore is a mineral from which metal is obtained. ### Gangue - Ores mined from the earth are usually contaminated with large amounts of impurities such as soil, sand, etc. The impurities are called **gangue**. ### Ores of some important metals | Ore type | Metal | Mineral | Composition | |---|---|---|---| | Oxide Ores | Aluminium | Bauxite | Al₂O₃.2H₂O | | Oxide Ores | Copper | Cuprite | Cu₂O | | Oxide Ores | Iron | Magnetite | Fe₂O₄ | | Sulphide Ores | Copper | Copper pyrites | CuFeS2 | | Sulphide Ores | Zinc | Zinc blende | ZnS | | Sulphide Ores | Lead | Galena | PbS | | Carbonate Ores | Mercury | Cinnabar | HgS | | Carbonate Ores | Calcium | Limestone | CaCO₃ | | Halide Ores | Zinc | Calamine | ZnCO₃ | | Halide Ores | Sodium | Rock salt | NaCl | | Halide Ores | Magnesium | Carnallite | KCI MgCl2.6H2O | | Halide Ores | Calcium | Fluorspar | CaF2 | | Sulphate Ores | Silver | Horn Silver | AgCl | | Sulphate Ores | Calcium | Gypsum | CaSO4.2H2O | | Sulphate Ores | Magnesium | Epsom Salt | MgSO4.7H2O | | Sulphate Ores | Barium | Barytes | BaSO₄ | | Sulphate Ores | Lead | Anglesite | PbSO₄ | ### Metallurgy - A diagram of the Earth with an arrow pointing to the area where *gold* can be found. ### Metallurgy - *Step 1: Crushing and grinding of ore* - The ore is crushed into smaller pieces by putting impact forces through a hammer. It is converted to a powdered form through a grinder. - *Magnetic seperation* - An illustration of separating the ore from the gangue using magnetic separation with a diagram of a beaker containing froth bubbles carrying sulphide ore, a pipe containing water and oil, and a chamber with the sulphide ore particles and gangue at the bottom. ### Step 2: Concentration of ore - *Before extracting the metal, it is important to remove gangue or impurities.* ### Step 3: Extraction of metals - A diagram shows the steps involved in the extraction of metals from ores starting with ore and concentration, going through to refining. - The diagram also shows the different extraction methods depending on the reactivity of the metal. - *Metals of high reactivity* - Potassium, Sodium, Calcium, Magnesium, Aluminium, Zinc - are extracted using electrolysis. - *Metals of medium reactivity* - Iron, Lead and Copper - are extracted by reduction using carbon. - *Metals of low reactivity* - Gold and Silver - are found in native state This document is a comprehensive guide to the concepts of metals and non-metals, their properties and extraction. It also includes a section on Abhay Premier League, a quiz-based competition designed to assess students' understanding of the subject.