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8432b7e1-ac6c-4c78-873d-3e271275e97a Heating Stage Summary The portion of the curve where the substance is being heated, resulting in an increase in temperature and average kinetic energy of the particles.

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Cancellation policy We understand very well how precious is your time , that is why we try to be always punctual and on it. That is why we are expecting the same from you , Start Lesson on time and not be late so that you do not miss anything. Still we understand circumstances happens that is why sometimes you come late or you are not able to show up. You are allowed 1 time cancellation on same day with valid reasons , 2 times cancellations at least 24 hours before lesson with valid reasons. Lessons cancellation beyond these 3 times are not allowed and Session will be considered as done , Please note that not providing valid reasons also for cancellation will result in session considered given. FAQ

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Expert SABIS Grade 12 Chemistry tuition in UAE and online . Weekly live sessions. Boost grades with a top private tutor. Register today at K-Chemistry.com

506be088-1a1d-45fa-9694-de33a6b8d504 Chemical Change Summary Always produces a new kind of matter, is generally not easily reversible, is usually accompanied by considerable heat change, produces no observable change in mass

Lesson 34 Chapter 6 SABIS Grade 10 Part 4 Lesson 34 261. Demonstration: Sublimation: Examples of solids that can sublime at room temperature: 1) Solid iodine, I2 (s) 2) Dry ice or solid carbon dioxide CO2 (s) 3) Any ammonium compound as ammonium chloride, NH4Cl and ammonium bromide, NH4Br 262. Demonstration: Simple Distillation 263. Demonstration: Fractional distillation. Discuss briefly: fractional distillation of liquefied air and fractional distillation of crude oil. 264. Demonstration: Separating funnel 265. Adsorption: means sticking to the surface. 266. Adsorption: sticking of the particles of one material on the surface of another. Examples of adsorbing substances: Silica gel: adsorbs water vapor, Charcoal: adsorbs gases with strong odor and removes colored impurities from a solution 267. Demonstration: Chromatography. It is the technique used to separate different compounds, especially those that can be easily destroyed by heat or chemicals. It can be used to separate colored components as: 1) Green liquid obtained by squashing green leaves. 2) Black ink. The property that carries the liquid up the paper is capillary action. 268. Demonstration: Crystallization 269. Alcohol is flammable, therefore it cannot be heated directly. To heat alcohol, we should use a steam bath or an electric heater. 270. If you need to collect sugar from sugar alcohol solution heat the solution using an electric heater to crystallization point. Leave the solution to cool and crystals to form. Filter off the crystals. 271. Vapor pressure and temperature are proportional NOT directly proportional. At the same temperature, the vapor pressure is the SAME. For the same liquid, the only factor affecting the pressure of the liquid is the temperature. 272. Minimum conditions for liquid molecules to vaporize: 1) Molecules are supposed to be on the surface. 2) Molecules are supposed to have an average kinetic energy greater than the energy keeping the molecules in the liquid state. 273. Water has a vapor pressure of 17.5 mmHg at 20oC. Which of the following will increase the vapor pressure of water? a) Transferring water to a larger container. b) Cooling water to 10oC c) Taking the container to the top of the mountain. d) Heating the water to 32oC 274. Boiling point: is the temperature at which the liquid vaporizes anywhere in the solution. 275. At the boiling point: a. Vapor pressure is equal to the surrounding pressure. b. Bubbles of vapor can form anywhere within the liquid. c. Molecules escape from the surface of the liquid to enter the gas phase as vapor (this also happens at room temperature). d. With increasing altitude, atmospheric pressure decreases and so does boiling point. 276. Normal boiling point: is the temperature at which the vapor pressure is exactly 1 atm or 760 mmHg. 277. Molar heat of fusion: is the energy required to change one mole of a substance from solid to liquid at the same temperature and constant pressure. 278. General equation for Molar heat of vaporization: X (l) + heat ⇌ X (g) 279. General equation for Molar heat of condensation: X (g) ⇌ X (l) + heat 280. In general, a substance that has a higher boiling point is expected to have a 281. An aqueous solution is one in which the solvent is water. 282. Salt and water is an example of aqueous solutions where the solute is a solid. 283. Alcohol and water is an example of aqueous solutions where the solute is a liquid. 284. Ammonia and water is an example of aqueous solutions where the solute is a gas. 285. Concentration: relative amounts of solute and solvent. 286. Molar concentration (Molarity): is the number of moles of solute per liter (dm3) of solution. (the relative amounts of solute and solution) 287. Concentration of a given solution does not change if solution is split into fractions. 288. Relationships between n, V, C and m, M, V, C: n = CV, 𝐂 = 𝐦/𝐕, 𝐕 = 𝐦/𝐂, m = n × M, m = CVM, 𝐌 = 𝐦/𝐂𝐕 289. Preparing solutions with given concentrations. 290. A 2 L bottle of 0.35 M solution is split into ten containers of 100ml capacity. What is the concentration of the solution in each of the new containers? a) 0.75 M b) 0.0035 M c) 2.0 M d) 0.35 M e) 100 M 291. Demonstration: Sublimation: Examples of solids that can sublime at room temperature: 1) Solid iodine, I2 (s) 2) Dry ice or solid carbon dioxide CO2 (s) 3) Any ammonium compound as ammonium chloride, NH4Cl and ammonium bromide, NH4Br 292. Demonstration: Simple Distillation 293. Demonstration: Fractional distillation. Discuss briefly: fractional distillation of liquefied air and fractional distillation of crude oil. 294. Demonstration: Separating funnel 295. Adsorption: means sticking to the surface. 296. Adsorption: sticking of the particles of one material on the surface of another. Examples of adsorbing substances: Silica gel: adsorbs water vapor, Charcoal: adsorbs gases with strong odor and removes colored impurities from a solution 297. Demonstration: Chromatography. It is the technique used to separate different compounds, especially those that can be easily destroyed by heat or chemicals. It can be used to separate colored components as: 1) Green liquid obtained by squashing green leaves. 2) Black ink. The property that carries the liquid up the paper is capillary action. 298. Demonstration: Crystallization 299. Alcohol is flammable, therefore it cannot be heated directly. To heat alcohol, we should use a steam bath or an electric heater. 300. If you need to collect sugar from sugar alcohol solution heat the solution using an electric heater to crystallization point. Leave the solution to cool and crystals to form. Filter off the crystals.

Lesson 13 Chapter 4 SABIS Grade 11 Lesson 13 🎉 Welcome to the Fascinating World of Electrolysis! 🎉 ⚡ What is Electrolysis? ⚡ Electrolysis may sound like a term from a sci-fi movie, but guess what? It's happening around us every day! It's a process that breaks down ionic compounds into their individual ions using electricity. 🌩️ 👀 Electrolysis in Daily Life 👀 Did you know you encounter products of electrolysis every day? 😲 When you use aluminum foil 🍽️ for your yummy dinner, remember that electrolysis was used to extract aluminum from its ore. Or when you're admiring the gold plating 💍 on jewelry, that's also done by electrolysis! So next time you see these items, give a quick thanks to electrolysis! 😉 💡 Breaking Down Ionic Compounds 💡 But how does electrolysis work, you ask? Well, it starts with an ionic compound . This compound is made up of positively charged ions, called cations , and negatively charged ions, known as anions . They stick together because opposites attract, right? 💖 But when we add electricity into the mix, it's like a dance party, and all the ions want to dance with the electric current! 💃🕺🎶 🧲 Forming Ions from Ionic Compounds 🧲 So how do we get these ions? Let's take a look at Sodium Chloride (NaCl), a classic ionic compound. Sodium (Na), a metal, loses an electron to become a cation (Na+), and Chlorine (Cl), a non-metal, gains that electron to become an anion (Cl-). Together, they form Sodium Chloride (NaCl) through an ionic bond! But remember, this process can also go in reverse during electrolysis! When electricity is applied, NaCl breaks up into its individual ions again (Na+ and Cl-) ready to join the ion dance party! 🥳 🎯 Electrolysis Quiz 🎯 What does the process of electrolysis break down? a. Atoms b. Covalent compounds c. Ionic compoundsd. Molecules Which of the following is a product of electrolysis that you might use in daily life? a. Aluminum foil b. Wooden furniture c. Plastic bottled. Glass window What happens to an ionic compound during electrolysis? a. It becomes a covalent compound. b. It breaks down into individual atoms. c. It breaks down into individual ions. d. Nothing changes. In an ionic compound, what do you call the positively charged ion? a. Atom b. Anion c. Cation d. Molecule What happens to Sodium Chloride (NaCl) during electrolysis? a. Sodium and Chlorine atoms combine to form Sodium Chloride. b. Sodium Chloride is converted into a covalent compound. c. Sodium and Chlorine atoms are separated, and Sodium Chloride disappears. d. Sodium Chloride breaks down into Sodium ions (Na+) and Chloride ions (Cl-). results if failed question 1 Let's revisit electrolysis with a solution of Sodium Chloride (NaCl): Electrolysis of Sodium Chloride (NaCl) will result in: a. Sodium and Chlorine atoms combining to form Sodium Chloride. b. Sodium Chloride being converted into a covalent compound. c. Sodium and Chlorine atoms being separated, and Sodium Chloride disappearing. d. Sodium Chloride breaking down into Sodium ions (Na+) and Chloride ions (Cl If student failed question 2: What are the products of electrolysis of water (H2O)? a. Oxygen and Hydrogen atoms b. Hydrogen and Oxygen ions c. Hydrogen gas (H2) and Oxygen gas (O2) d. Water molecules (H2O) If student failed question 3: The electricity in electrolysis is used to: a. Create new compounds b. Cause a chemical reaction between elements c. Break down compounds into their constituent ions d. Heat the solution to boiling point If student failed question 4: In the electrolysis of Sodium Chloride, where do Sodium ions (Na+) migrate? a. They stay in the middle of the solution b. They move towards the anode (negative electrode) c. They move towards the cathode (positive electrode) d. They evaporate into the air If student failed question 5: What happens to the ions at the electrodes during electrolysis? a. They combine to form the original compound b. They lose or gain electrons to form neutral atoms or molecules c. They are destroyed in the process d. They convert the electrode into a new compound

f4dca41b-3c48-42a1-bb54-fa81f3ae5eec Surrounding Summary The environment around a system where a chemical reaction is taking place.

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