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< Back Previous Next 🎇🎆🚀 Welcome to Electrifying World of Electrolysis and Conductivity! 🎇🎆🚀 Have you ever wondered how a piece of metal conducts electricity, but your rubber shoes don't? Or what magic makes your salty water conduct electricity? Well, buckle up for an electrifying journey! Today, we're diving into the mysterious and fascinating world of conductors, non-conductors, semi-conductors, electrolytes, non-electrolytes and even the incredible process of electrolysis ! ⚡⚗🔬 ⭐💫✨ Conductors, Non-conductors and Semi-Conductors ✨💫⭐ Let's begin with a quick rundown on these three: 1️⃣ Conductors 👨🔬: These are the 'social butterflies' of the material world! They LOVE to share their electrons and allow electricity to flow through them. All metals, like the aluminium and steel in overhead cables or the copper in your electric wires, are fabulous conductors! Why? It's all thanks to their free-moving delocalized electrons. 🚃💨 2️⃣ **Non-conductors (Insulators)**🧤: Now these are the 'hermits'. They do NOT like to share their electrons. Non-metals like plastic, glass, wood, and rubber fall into this category. Exception alert! 🚨 Graphite, a non-metal, is actually a good conductor because it has free electrons. 🎭 3️⃣ Semi-conductors 🌗: As the name suggests, these materials are in-betweeners. They're the 'casual friends' who only let a very small electric current pass through them. Silicon is a prime example. 🌉 💧🔋🚰 Electrolytes and Non-Electrolytes 🚰🔋💧 Next up, let's splash into the world of liquids that conduct electricity: 🔹 Electrolytes 💡: These are the 'party starters' in liquid form! They contain ions that are free to move, and hence, they conduct electricity. Examples include aqueous ionic compounds (like salts dissolved in water), molten ionic compounds, and solutions of acids or alkalis. If it's an electrolyte, it makes the bulb glow!💡🎉 🔸 Non-electrolytes 💤: On the other hand, we have these 'party poopers'. They're liquids that do NOT conduct electricity. Examples are pure water, ethanol, sugar solution, oil, benzene. If it's a non-electrolyte, the bulb stays off.😴 Now, what if we told you that you can break down certain substances using electricity? Enter the process of electrolysis! ⚡⚗🎆 ⚡🧪🔥 Electrolysis - The Electro-Magic 🔥🧪⚡ Electrolysis is the magical process where a substance is decomposed (broken down) by the passage of electricity. It's a stunning electro-dance where ions migrate towards the opposite electrodes (remember, opposites attract!). 🕺💃🎊 👉 The cathode is the -ve electrode, and it attracts +ve cations. Here, these cations gain electrons and turn into atoms or molecules. (Remember: Cathode attracts Cations!) 👉 The anode is the +ve electrode, and it attracts -ve anions. Here, these anions lose electrons and turn into atoms or molecules. (Remember: Anode attracts Anions!) For the energy enthusiasts, it's important to know that electrolysis is an endothermic process , absorbing energy and converting electrical energy to chemical energy (opposite to cells!). In the following parts, we'll explore the exciting process of electrolysis of molten ionic compounds and the extraction of aluminium ! Stay tuned! 📺🔍⏳ The whole lesson can be summarized by a simple yet effective mnemonic: OILRIG - Oxidation Is Loss of electrons; Reduction Is Gain of electrons . So, ready for more electric magic? Let's carry on and stay charged! ⚡🔋🔆 Fantastic! You're keeping up really well! Let's continue our electrifying journey and dive deep into the world of Electrolysis ! ⚡🔬 ⚡⚗🔥 Electrolysis of Molten Ionic Compounds 🔥⚗⚡ When an ionic compound melts, it's like a dance party - ions are free to move around! That's when electrolysis enters the dance floor! Here's what happens when molten lead bromide, for instance, gets electrolyzed: 👉 At the Cathode (-ve electrode) : Pb2+(l) + 2e- → Pb(l). The silvery shiny metal lead forms! This is a reduction process (Remember: Red uction happens at the Red Cathode!). 🕺 👉 At the Anode (+ve electrode) : 2Br-1(l) - 2e- → Br2(g). Red-brown bromine vapour bubbles off! This is an oxidation process (Remember: Ox idation happens at the A node!). 💃 Our mnemonic friend OILRIG will help you remember this! In general, with electrolysis: 1️⃣ Metal is deposited at the cathode (it's all shiny and new!). 2️⃣ Non-metal is deposited at the anode. As for the colors at the electrodes, most metals are silvery grey (except gold, which is yellow, and copper, which is red-brown). Non-metals can be a bit more colorful – sulfur is a yellow solid, halogens can range from pale-yellow gas (fluorine) to grey solid/purple gas (iodine), and others are colorless gases. 🌐🛠🔩 Extraction of Aluminium 🔩🛠🌐 Aluminium extraction is a perfect example of electrolysis in action in the industry. Bauxite, the primary aluminium ore, is transformed into aluminium through a process that involves electrolysis. Remember that reactive metals like Al can only be extracted by electrolysis. So, here's what happens: 👉 At the Cathode (-ve electrode) : Al3+(l) + 3e- → Al(l). Aluminium sinks to the bottom - it's born anew! It's another case of reduction. 🎈 👉 At the Anode (+ve electrode) : 2O-2(l) - 4e- → O2(g). Oxygen gas bubbles off and also reacts with the graphite electrode to produce CO2 and CO. It's oxidation at work here. 🎉 👉 Fluorine gas is also formed at the anode (originating from the cryolite). So that's it! We've now taken a journey through conductors, non-conductors, semi-conductors, electrolytes, non-electrolytes and even the incredible process of electrolysis! And there you have it, another amazing adventure in the world of chemistry. Stay curious and keep exploring! 🎆🎇🚀 Go To lesson 2 Electricity and Chemistry Lesson 1 Next Topic

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< Back Previous Next ecessary to know the bonds present in both the reactants and products How to complete bond energy calculations Write a balanced equation if none is present already Optional - draw the displayed formula in order to identify the type and number of bonds more easily Add together all the bond energies for all the bonds in the reactants – this is the ‘energy in’ Add together the bond energies for all the bonds in the products – this is the ‘energy out’ Calculate the enthalpy change: Enthalpy change (Δ H ) = Energy taken in - Energy given out Worked Example Hydrogen and chlorine react to form hydrogen chloride gas: H2 + Cl2 ⟶ 2HCl The bond energies are given in the table below. Bond Energy (kJ) H–H 436 Cl–Cl 242 H–Cl 431 Calculate the overall energy change for this reaction and use this value to explain whether the reaction is exothermic or endothermic. Answer: Calculate the energy in 436 + 242 = 678 (kJ) Calculate the energy out 2 x 431 = 862 (kJ) Calculate the energy change 678 - 862 = –184 (kJ) Since the energy change is a negative number, energy is being released (to the surroundings) Therefore, the reaction is exothermic Examiner Tips and Tricks When calculating enthalpy change using bond energies, it is helpful to write down a displayed formula equation for the reaction before identifying the type and number of bonds, to avoid making mistakes. So, the reaction for the above worked example is: H-H + Cl-Cl → H-Cl + H-Cl Worked Example Hydrogen reacts with iodine to form hydrogen iodide. H2 + I2 ⟶ 2HI The relevant bond energies are shown in the table below. Bond Energy (kJ) H–I 295 H–H 436 I–I 151 Calculate the overall energy change for this reaction and use this value to explain why the reaction is exothermic. Answer: Calculate the energy in 436 + 151 = 587 (kJ) Calculate the energy out 2 x 295 = 590 (kJ) Calculate the energy change 587 - 590 = -3 (kJ) The reaction is exothermic because: More energy is released than taken in Worked Example Hydrogen bromide decomposes to form hydrogen and bromine: 2HBr ⟶ H2 + Br2 The overall energy change for this reaction is +103 kJ. The relevant bond energies are shown in the table below. Bond Energy (kJ) H–Br 366 Br–Br H–H 436 Calculate the bond energy of the Br–Br bond. Answer: Calculate the energy in 2 x 366 = 732 (kJ) State the energy out 436 + Br–Br Overall energy change = energy in - energy out +103 = 732 - (436 + Br–Br) +103 = 732 - 436 - Br–Br Calculate the bond energy of the Br–Br bond Br–Br = 732 - 436 - 103 Br–Br = + 193 (kJ) Chemical energetics Next Topic

< Back Previous Next 🎯 Solubility of Ionic Compounds 🎯 The solubility of ionic compounds can be predicted with some general rules, which you already listed. These rules are not absolute, but they offer a good starting point for understanding solubility. You'll be able to predict whether certain compounds will dissolve in water and under what conditions. 🌊💡🔋 Electrolysis of Aqueous Solutions 🔋💡🌊 An aqueous solution contains dissolved ions and also ions from the water itself. When it comes to electrolysis: 👉 At the cathode: The less reactive cation (positive ion) will be discharged. In general, this is often a metal ion or a hydrogen ion (H+). 👉 At the anode: The less reactive anion (negative ion) will be discharged. Usually, this is the hydroxide ion (OH-) or a halide ion if the solution is concentrated. 🎨🌈 pH Scale and Indicators 🌈🎨 The pH scale ranges from 0 (strongly acidic) to 14 (strongly basic). A pH of 7 is neutral. Indicators are chemicals that change color based on the pH of the solution. Common indicators include: Litmus: Red in acid, blue in base. Methyl orange: Red in acid, yellow in base. Thymolphthalein: Colourless in acid, blue in base. Universal indicator: Displays a range of colors across the pH scale. 💡⚡ Electrolysis Examples ⚡💡 You've provided multiple examples for the electrolysis of different substances, including: Copper sulfate (CuSO4) : Copper is deposited at the cathode, and oxygen is released at the anode. Sulfuric acid (H2SO4) : Hydrogen is released at the cathode, and oxygen at the anode. Dilute NaCl : Hydrogen is released at the cathode, and oxygen at the anode. Concentrated HCl : Hydrogen is released at the cathode, and chlorine at the anode. Concentrated NaCl (brine) : Hydrogen is released at the cathode, and chlorine at the anode. Note that in all these reactions, the less reactive ions are the ones getting discharged at the electrodes. In each case, the electrolyte concentration changes during the electrolysis process, often getting more concentrated. 🏭🔋 Applications of Electrolysis 🔋🏭 Electrolysis has many important industrial applications, including the production of chlorine, hydrogen, and sodium hydroxide from brine. These products have a wide range of uses, such as in the production of plastics, fuels, soaps, detergents, and more. And there you have it! A journey through the intricate world of solubility, pH, electrolysis, and their applications. Remember, the more you understand these processes, the easier it becomes to understand how the world of chemistry works around us. Keep exploring! 🧪🎆🚀 Go To lesson 3 Electricity Lesson 2 Next Topic

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