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Chapter 5 SABIS Grade 10 Lesson 2 Lesson 26 Chapter 5: Part 2 - Kinetic Theory of Gases Concept 1: The Basics of Kinetic Theory of Gases Temperature is a key player in how gas particles behave. Here's how it works: Average Kinetic Energy: The average kinetic energy of gas particles is directly related to the temperature. If you're at a party 🥳, think of the temperature as the volume of the music. The louder (hotter) the music, the more energy you have to dance 💃! As the temperature increases, particles move more rapidly. They also collide with the walls of the container more frequently and with more force. This leads to an increase in the pressure of the gas. It's like when you're making popcorn 🍿! The more heat, the faster the kernels pop and hit the inside of the popcorn maker, and the more popcorn you have in the end! Quick Understanding Check: If you have a gas inside a container and you increase the temperature, what happens to the gas particles? Answer: If the temperature increases, the gas particles move more rapidly and collide more frequently and strongly with the walls of the container. Test your understanding: What happens to the average kinetic energy of a gas when the temperature increases? A) It decreases B) It stays the same C) It increases D) It disappears What happens to the gas particles when the temperature increases? A) They move more slowly B) They collide less frequently with the container walls C) They move more rapidly and collide more frequently and strongly with the container walls D) They stop moving If you increase the temperature of a gas, what happens to the pressure it exerts on its container? A) It decreases B) It stays the same C) It increases D) It becomes zero If you compare a gas at a low temperature with a gas at a high temperature, which one has particles that move more rapidly? A) The gas at low temperature B) The gas at high temperature C) Both move at the same rate D) It depends on the type of gas If you decrease the temperature of a gas, what happens to the pressure it exerts on its container? A) It increases B) It stays the same C) It decreases D) It becomes zero Concept 2: Kinetic Energy and Temperature in Gases Now that we understand the basic idea of gas particle movement and pressure, let's look at how kinetic energy and temperature come into play. Kinetic Energy: The average kinetic energy of a gas - that's the energy it has due to its motion - is constant at a constant temperature. Just like when you keep pedaling a bike at a steady pace, your kinetic energy stays the same. Temperature and Energy: As temperature increases, the average kinetic energy of a gas increases. This is similar to how your body heats up when you exercise - as you work harder (increase your energy), your body temperature rises. Temperature and Pressure: As temperature increases, particles move more rapidly. They collide with the wall of the container more frequently and more strongly, so the pressure of the gas increases. This is like increasing the speed of a pinball machine. The ball (or particles) starts moving faster and hits the sides more often, which increases the pressure. 🏓💥 Concept 3: Ideal and Real Gases Gases can be categorized into two types: ideal and real. But what do these terms mean? Ideal Gas: An ideal gas always stays as a gas even when cooled. It perfectly follows the law PV = constant, where P is pressure and V is volume. It's called "ideal" because it's a model we use for calculations, but no real gas behaves ideally under all conditions. Imagine a unicorn - we have an idea of what it is, but it doesn't exist in real life. 🦄 Real Gas: Real gases can liquefy upon cooling. They follow the law PV = constant only approximately. They behave like ideal gases at high temperatures and low pressures. But as pressure increases and volume decreases, real gases can liquefy, and the PV = constant rule no longer applies. Imagine water vapor condensing into water; it goes from a gas to a liquid under certain conditions. 💨➡️💧 Quick Understanding Check: Why is an ideal gas called "ideal"? Answer: An ideal gas is called "ideal because it perfectly follows the law PV = constant and it doesn't change state upon cooling. It is a model used for calculations, but no real gas behaves ideally under all conditions.Test your understanding:What happens to an ideal gas when it is cooled? ❄️A) It liquefiesB) It remains a gasC) It becomes a solidD) It evaporates Answer: B) It remains a gas How does a real gas behave under high temperatures and low pressures? 🌡️⬆️ & ⬇️A) Like a liquidB) Like a solidC) Like an ideal gasD) It disappears Answer: C) Like an ideal gas Why doesn't PV = constant apply to real gases under all conditions? ❓A) Because they can liquefy under certain conditionsB) Because they always stay as gasesC) Because they can solidifyD) Because they can evaporate Answer: A) Because they can liquefy under certain conditions If we recall the earlier concept, increasing temperature causes gas particles to move more rapidly, colliding more frequently and strongly with the container, thus increasing pressure. Now, consider a real gas under these conditions. As the pressure increases and volume decreases, what happens to the real gas? 🌡️⬆️➡️💥⬆️➡️❓A) It becomes an ideal gasB) It stays the sameC) It liquefiesD) It evaporates Answer: C) It liquefies Compare an ideal gas and a real gas. Which one perfectly follows the law PV = constant? 🅿️✖️🅱️=⏹️A) Ideal gasB) Real gasC) BothD) Neither Answer: A) Ideal gas Concept 4: Temperature, Volume, and Molar Mass Temperature not only affects the pressure and kinetic energy of a gas, but also its volume. Also, the molar mass of a gas affects its freezing point (FP) and boiling point (BP). Temperature and Volume: As the temperature of a fixed mass of gas at constant pressure increases, so does its volume. It's like blowing up a balloon - as you add more air (increase the temperature), the balloon (volume) gets bigger. 🎈⬆️ Temperature Units: T(K) = t(°C) + 273. This is how you convert temperature from Celsius to Kelvin. Kelvin is a temperature scale used in physical sciences. The Kelvin has the same magnitude as the degree Celsius, but it starts at absolute zero - the lowest temperature possible in the universe! 🌡️🔄 Molar Mass and FP/BP: The higher the molar mass, the higher the freezing point (FP) and boiling point (BP). It's like being heavier makes it harder for you to get moving (higher FP) and harder for you to stop once you're going (higher BP). ⚖️➡️❄️/🌡️ Quick Understanding Check: If the temperature of a gas increases, what happens to its volume (assuming the gas is at constant pressure)?Answer: If the temperature of a gas increases, its volume also increases.Test your understanding:What happens to the volume of a fixed mass of gas at constant pressure if its temperature increases? 🌡️⬆️➡️🅱️❓A) It decreasesB) It remains the sameC) It increasesD) It disappears Answer: C) It increases How do you convert temperature from degrees Celsius to Kelvin? 🌡️🔄A) T(K) = t(°C) + 273B) T(K) = t(°C) - 273C) T(K) = t(°C) * 273D) T(K) = t(°C) / 273 Answer: A) T(K) = t(°C) + 273 What does a higher molar mass mean for a gas's freezing and boiling points? ⚖️➡️❄️/🌡️A) Lower freezing and boiling pointsB) Higher freezing and boiling pointsC) Unchanged freezing and boiling pointsD) No freezing or boiling points Answer: B) Higher freezing and boiling points From our previous concepts, we know that increasing temperature causes an increase in both kinetic energy and pressure in gases. Now, if you increase the temperature of a fixed mass of gas at constant pressure, what happens to its volume? 🌡️⬆️➡️🅱️❓A) It decreasesB) It stays the sameC) It increasesD) It becomes zero Answer: C) It increases Considering all the concepts we've learned so far, if a real gas is at high temperatures and low pressures, and its volume is decreasing while its temperature is increasing, what would likely happen to this gas? 🌡️⬆️🅿️⬇️🅱️⬇️➡️❓A) It would behave like an ideal gasB) It would liquefyC) Its pressure would decreaseD) Its volume would increase Answer: B) It would liquefy Final Quiz - Chapter 5: Lesson 2 📝 (2 marks) Gas particles move in ________ directions. A) Straight B) Circular C) Random D) Back and forth (2 marks) If you increase the temperature of a gas, its pressure __________. A) Decreases B) Stays the same C) Increases D) Becomes zero (2 marks) An ideal gas follows the law __________ perfectly. A) PV = variable B) PV ≠ constant C) PV = constant D) PV = 0 (2 marks) Real gases behave like ideal gases under __________. A) High temperatures and high pressures B) Low temperatures and low pressures C) High temperatures and low pressures D) Low temperatures and high pressures Answer: C) High temperatures and low pressures (2 marks) If the temperature of a fixed mass of gas at constant pressure increases, its volume __________. A) Decreases B) Stays the same C) Increases D) Becomes zero Answer: C) Increases (2 marks) The higher the molar mass of a gas, the ________ its freezing point (FP) and boiling point (BP). A) Lower B) Higher C) Unchanged D) None of the above Answer: B) Higher (3 marks) If a real gas is under high temperatures and low pressures, and you increase its temperature while decreasing its volume, the gas is likely to ________. A) Behave like an ideal gas B) Liquefy C) Have its pressure decrease D) Increase in volume Answer: B) Liquefy (3 marks) The kinetic theory of gases assumes that gas particles move ________. A) Only when heated B) In a straight line always C) At random D) In a circular pattern Answer: C) At random (3 marks) The volume of an ideal gas is directly proportional to the __________. A) Pressure B) Absolute temperature C) Mass D) Molar mass Answer: B) Absolute temperature (3 marks) The average kinetic energy of a gas is constant at ________. A) Constant pressure B) Constant volume C) Constant temperature D) None of the above Answer: C) Constant temperature Total Marks: 24 Passing Score: 17 (Approximately 70%) To calculate your percentage, divide your score by the total marks and multiply by 100. For example, if your score is 20, your percentage would be (20/24)*100 = 83.33%. That's all for today's lesson! Keep practicing, and always be curious! 🎓🔬🚀 Go to Lesson 3

Chapter 3 SABIS Grade 10 Part 2 🧐 Lesson 11 🧐 Chapter Three Part Two: Identifying Substances and Mixtures 🎈 Prerequisite Quiz:🔹 Q1: 🤔 What is a pure substance? Ⓐ A substance that consists of multiple types of atoms. Ⓑ A substance that is composed of only one type of atom. Ⓒ A substance that cannot be broken down into simpler substances. Ⓓ Both B and C Answer: Ⓓ Both B and C. 👍 A pure substance is composed of only one type of atom and cannot be broken down into simpler substances. 🔹 Q2: 🤔 Which state of matter consists of atoms tightly packed together? Ⓐ Gas Ⓑ 🎯 Solid Ⓒ Liquid Ⓓ Plasma Answer: Ⓑ Solid. 👍 In solids, atoms are tightly packed together. 🔹 Q3: 🤔 What is a molecule? Ⓐ A single type of atom. Ⓑ 🎯 A group of atoms bonded together. Ⓒ A group of elements combined together. Ⓓ A single type of element. Answer: Ⓑ A group of atoms bonded together. 👍 A molecule is a group of atoms bonded together. 🔹 Q4: 🤔 What is a homogeneous mixture? Ⓐ A mixture where you can identify individual components. Ⓑ 🎯 A mixture that has a uniform composition throughout. Ⓒ A mixture that has different components in different phases. Ⓓ None of the above. Answer: Ⓑ A mixture that has a uniform composition throughout. 👍 A homogeneous mixture has a uniform composition throughout. 🔹 Q5: 🤔 What is a heterogeneous mixture? Ⓐ 🎯 A mixture where you can identify individual components. Ⓑ A mixture that has a uniform composition throughout. Ⓒ A mixture that has different components in different phases. Ⓓ None of the above. Answer: Ⓐ A mixture where you can identify individual components. 👍 A heterogeneous mixture is a mixture where you can identify individual components. 🔹 Q6: 🤔 What are physical properties? Ⓐ 🎯 Properties that can be observed without changing the identity of the substance. Ⓑ Properties that can only be observed during a chemical reaction. Ⓒ Properties that change the identity of the substance. Ⓓ None of the above. Answer: Ⓐ Properties that can be observed without changing the identity of the substance. 👍 Physical properties can be observed without changing the identity of the substance. 🔹 Q7: 🤔 How can substances be separated in a mixture? Ⓐ 🎯 By physical means. Ⓑ By chemical means. Ⓒ Both A and B. Ⓓ None of the above. Answer: Ⓐ By physical means. 👍 Substances in a mixture can be separated by physical means. 🔹 Q8: 🤔 What is the basic unit of a chemical element? Ⓐ Molecule Ⓑ Compound Ⓒ 🎯 Atom Ⓓ Particle Answer: Ⓒ Atom. 👍 The basic unit of a chemical element is an atom. 🔹 Q9: 🤔 What does it mean when a substance has a fixed composition? Ⓐ It has the same proportion of elements regardless of the sample size. Ⓑ It has different proportions of elements depending on the sample size. Ⓒ It cannot be separated into its components. Ⓓ 🎯 Both A and C. Answer: Ⓓ Both A and C. 👍 When a substance has a fixed composition, it means it has the same proportion 🧐 The Lesson: Think of pure substances like your best friends 😁, you can always identify them based on their unique characteristics 🧑👧. Similarly, we identify pure substances through their physical constants such as boiling point, melting point, etc 🌡️. A pure substance can either be an element or a compound. An element is like a super VIP person 👑, they cannot be split into simpler substances by physical means or through chemical reactions. It's a pure substance made up of one kind of atoms, pretty unique huh? On the other hand, a compound is like a football team ⚽, where you've got different players (atoms) working together. It's a pure substance containing more than one type of atoms. Some compounds don't even form molecules! For example, table salt (NaCl) and sand (SiO2). Now, let's talk about mixtures 🍕. Mixtures are like a pizza, made up of at least two different ingredients (pure substances). They don't have a fixed composition; you can put whatever toppings you like on your pizza! You can have homogeneous mixtures (solutions) 🥤, where all components mix so well, they exist in one phase. Just like a well-blended smoothie, you can't pick out individual fruits! But sometimes, you get heterogeneous mixtures 🥗, where components exist in more than one phase. Like a salad, where you can see and pick out different ingredients. Topics included 🔍 Topic 1: Pure Substances and Their Identification Pure substances 🧪, like your best friends, have unique characteristics that can be used to identify them. These are called physical constants and include properties like boiling point, melting point, etc. 🔍 Topic 2: Elements Elements 🌟 are like super VIPs; they can't be broken down into simpler substances, not even by chemical reactions. They are a pure substance made up of only one kind of atoms. 🔍 Topic 3: Compounds Compounds are like a soccer team ⚽, with different types of atoms (players) working together. They're a pure substance made up of more than one type of atoms, and sometimes they don't even form molecules (like table salt or sand). 🔍 Topic 4: Mixtures Mixtures 🍕 are like pizzas, consisting of at least two different ingredients (pure substances). The composition of a mixture is not fixed; it can vary depending on the proportions of the components. 🔍 Topic 5: Homogeneous Mixtures Homogeneous mixtures 🥤 are like a well-blended smoothie. All the components are so well mixed, they exist in a single phase, and you can't pick out individual ingredients. 🔍 Topic 6: Heterogeneous Mixtures Heterogeneous mixtures 🥗 are like salads, where the different components exist in more than one phase. You can see and pick out different ingredients. End of Lesson Quiz: 🔹 Q1: 🤔 What distinguishes a pure substance from a mixture? Ⓐ A pure substance cannot be separated into its components, but a mixture can. Ⓑ A pure substance has a fixed composition, but a mixture doesn't. Ⓒ Both A and B. Ⓓ Neither A nor B. Answer: Ⓒ Both A and B. 👍 A pure substance cannot be separated into its components and has a fixed composition, while a mixture can be separated and its composition can vary. 🔹 Q2: 🤔 An element is... Ⓐ A type of mixture. Ⓑ 🎯 A pure substance made up of one kind of atoms. Ⓒ A type of compound. Ⓓ A mixture of different atoms. Answer: Ⓑ A pure substance made up of one kind of atoms. 👍 An element is a pure substance made up of one kind of atoms. 🔹 Q3: 🤔 A compound is... Ⓐ A mixture of two or more elements. Ⓑ A pure substance made up of one kind of atoms. Ⓒ 🎯 A pure substance containing more than one type of atoms. Ⓓ None of the above. Answer: Ⓒ A pure substance containing more than one type of atoms. 👍 A compound is a pure substance that contains more than one type of atoms. 🔹 Q4: 🤔 Which of the following is a homogeneous mixture? Ⓐ Sand and water. Ⓑ Oil and water. Ⓒ 🎯 Salt dissolved in water. Ⓓ A bowl of fruit salad. Answer: Ⓒ Salt dissolved in water. 👍 Salt dissolved in water is a homogeneous mixture as it has a uniform composition throughout. 🔹 Q5: 🤔 Which of the following is a heterogeneous mixture? Ⓐ 🎯 A bowl of fruit salad. Ⓑ Salt dissolved in water. Ⓒ A glass of lemonade. Ⓓ Sugar dissolved in tea. Answer: 🎯 A bowl of fruit salad. 👍 A bowl of fruit salad is a heterogeneous mixture as you can identify individual components. 🔹 Q6: 🤔 What is the difference between homogeneous and heterogeneous mixtures? Ⓐ Homogeneous mixtures contain one type of particle, heterogeneous mixtures contain two. Ⓑ Homogeneous mixtures exist in one phase, heterogeneous mixtures in more than one phase. Ⓒ Homogeneous mixtures can't be separated, heterogeneous mixtures can. Ⓓ Homogeneous mixtures are always liquids, heterogeneous mixtures can be any state of matter. Answer: Ⓑ Homogeneous mixtures exist in one phase, heterogeneous mixtures in more than one phase. 👍 🔹 Q7: 🤔 Are all compounds made of molecules? Ⓐ Yes. Ⓑ No. Ⓒ Only if they are made from nonmetals. Ⓓ Only if they are made from metals. Answer: Ⓑ No. 👍 Some compounds, such as those formed from metals and nonmetals (e.g. NaCl), don't form molecules. 🔹 Q8: 🤔 Pure substances have a fixed... Ⓐ Color. Ⓑ Smell. Ⓒ Taste. Ⓓ Composition. Answer: Ⓓ Composition. 👍 The composition of a pure substance is fixed and doesn't vary. 🔹 Q9: 🤔 Mixtures have a fixed... Ⓐ Composition. Ⓑ Color. Ⓒ 🎯 None of the above. Ⓓ All of the above. Answer: Ⓒ None of the above. 👍 The composition, color, etc. of mixtures can vary. 🔹 Q10: 🤔 A compound can be broken down into... Ⓐ Molecules. Ⓑ 🎯 Its constituent elements. Ⓒ Other compounds. Ⓓ All of the above. Answer: 🎯 Its constituent elements. 👍 A compound can be broken down into its constituent elements through chemical reactions. 🔹 Q11: 🤔 Elements can be broken down into... Ⓐ Molecules. Ⓑ Compounds. Ⓒ 🎯 They can't be broken down into simpler substances. Ⓓ All of the above. Answer: Ⓒ They can't be broken down into simpler substances. 👍 An element is the simplest form of matter and cannot be broken down into anything simpler. 🔹 Q12: 🤔 Which of the following is true about mixtures? Ⓐ They are pure substances. Ⓑ They are made up of one type of particle. Ⓒ 🎯 Their composition can vary. Ⓓ Their composition is always the same. Answer: 🎯 Their composition can vary. 👍 The composition of mixtures can vary as they are made up of two or more substances. 🔹 Q13: 🤔 A solution is an example of a... Ⓐ Compound. Ⓑ Heterogeneous mixture. Ⓒ Element. Ⓓ 🎯 Homogeneous mixture. Answer: Ⓓ Homogeneous mixture. 👍 A solution is a homogeneous mixture as it has a uniform composition throughout. 🔹 Q14: 🤔 Sand and water form a... Ⓐ Solution. Ⓑ 🎯 Heterogeneous mixture. Ⓒ Compound. Ⓓ Element. Answer: Ⓑ Heterogeneous mixture. 👍 Sand and water form a heterogeneous mixture as the composition is not uniform. 🔹 Q15: 🤔 The physical constants of a substance refer to its... Ⓐ Color. Ⓑ Smell. Ⓒ 🎯 Boiling point, melting point, density, etc. Ⓓ Taste. Answer: Ⓒ Boiling point, melting point, density, etc. 👍 The physical constants of a substance, like its boiling point, melting point, and density, are properties that can be used to identify it. 🔹 Q16: 🤔 The components of a mixture can be separated by... Ⓐ Chemical reactions. Ⓑ 🎯 Physical methods. Ⓒ They can't be separated. Ⓓ Both chemical reactions and physical methods. Answer: Ⓑ Physical methods. 👍 The components of a mixture can be separated by physical methods, like filtration or distillation. 🔹 Q17: 🤔 A compound consists of two or more... Ⓐ Compounds. Ⓑ Mixtures. Ⓒ Elements. Ⓓ 🎯 Elements chemically combined. Answer: Ⓓ Elements chemically combined. 👍 A compound is a pure substance that is made up of two or more different elements that are chemically combined. 🔹 Q18: 🤔 In a mixture, the substances... Ⓐ Lose their original properties. Ⓑ 🎯 Retain their original properties. Ⓒ Chemically combine to form a new substance. Ⓓ Change into new substances. Answer: Ⓑ Retain their original properties. 👍 In a mixture, the substances retain their original properties. 🔹 Q19: 🤔 In a compound, the elements... Ⓐ Retain their original properties. Ⓑ 🎯 Lose their original properties. Ⓒ Are physically combined. Ⓓ Can be separated by physical methods. Answer: Ⓑ Lose their original properties. 👍 In a compound, the elements lose their original properties and have properties that are different from the elements that make them up. 🔹 Q20: 🤔 Elements and compounds are... Ⓐ Mixtures. Ⓑ Types of mixtures. Ⓒ 🎯 Pure substances. Ⓓ None of the above. Answer: Ⓒ Pure substances. 👍 Elements and compounds are both pure substances, not mixtures.

53e49697-409e-44ad-99bf-95f259a539b6 Health and safety issues related to Rate of reaction SABIS Summary Increasing the surface area of solid (by reduction of particle size) may cause explosion in some cases. For example  In flour mills, the air can fill with fine flour dust which has very large surface area. A spark can cause the flour to catch fire and explode.  In coal mines where the air is filled with very fine coal dust.

0680d4fb-a194-4c18-b4f1-2e7387586c8d Exothermic Reaction Summary Is a reaction which releases heat to the surrounding. As heat is released, the temperature of the surrounding increases. Cooling a substance, freezing, condensation are examples of exothermic processes

Laboratory Skills and Techniques Chapter 1 Part 2 SABIS Grade 10 Laboratory Skills and Techniques 🧪Lesson 2:🧪 List of Commonly used Laboratory Apparattus 🔬 1.Evaporating dish: Used in crystallization 🧪🌬️ Behold the Magnificent Evaporating Dish! 🌡️✨ This little hero, made of heat-resistant materials like glass or porcelain, holds secret powers in the lab. 🧪🔥 When we heat it up, magic happens! The liquid inside dances with excitement and slowly transforms into vapor, leaving behind solid treasures that were once dissolved within. 🌫️✨ This epic process allows us to perform the art of separation, bidding farewell to the liquid and welcoming the solid. 💦👋 The mighty evaporating dish fearlessly endures scorching temperatures, standing tall as a vital companion in countless scientific quests! 🌟 2.Burette: To measure variable volumes of liquids from 0 to 50 ml to the closet 0.05 cm3 per reading. Determining the Volume of liquid used requires two readings to be taken and subtracting one from the other, therefore, the uncertainty per measured V is ±0.1 cm3 🔍📏 Unlocking the Mysteries of Uncertainty! 🧪🔬 When we mention "uncertainty per measured V is ±0.1 cm³," a thrilling adventure in the world of measurement begins! 🌟🔍 It's like a secret door leading us into the realm of margin of error and uncertainty. 🚪✨ The value of ±0.1 cm³ acts as our guide, whispering that the true volume might be as much as 0.1 cm³ greater or smaller than what we measured. It's a thrilling dance of possibilities and surprises! 🎭🌠 So, let's embrace the unknown, for within the realm of uncertainty lies the magic of discovery! ✨🔍💫 🧪📏 Behold the Marvelous Burette! 🌟🔬 This long and slender glass tube is the maestro of precision, guiding scientists in their quest for accurate liquid measurements. 🎯✨ With its mystical valve at the bottom, the flow of liquid is controlled like a symphony, ensuring impeccable accuracy. 🎶🔐 Burettes take center stage in the captivating world of chemistry experiments, gracefully adding or measuring minuscule volumes of liquids with unparalleled precision. 💧🎭 They play a vital role in epic tasks like titrations, where every drop counts and accurate results are the ultimate treasure. 🏆🧪 Let's salute the remarkable burette, the guardian of meticulous measurements in the wondrous realm of chemistry! 🙌💫 3.Pipette: To measure specific Volume of liquid (exactly 5, 10, 25 or 50 cm3) with great accuracy, uncertainty of ∓0.05 cm3. It has one calibration mark. 🧪💧 Get Ready to Master the Art of Liquid Sorcery with the Amazing Pipette! 🪄🌟 This enchanting tool, resembling a thin tube with a bulb or magical mechanism, holds the key to measuring and transferring tiny drops of liquid with absolute finesse. ✨🔮 To unleash its powers, you simply squeeze the bulb or work its mystical mechanism, guiding the pipette's tip into the liquid abyss. 🧪🌊 As you release the bulb or mechanism, the pipette skillfully draws up the exact amount of liquid you desire, like a wizard conjuring a spell. 🌈💫 Pipettes are your trusty companions when precision is paramount, ensuring accurate measurements and seamless transfers of minuscule liquid wonders during mesmerizing experiments. 🧪🔬 Let's embark on a journey of liquid mastery with the remarkable pipette by our side! 🚀🔍 4. Measuring cylinder: To measure various volumes of liquids, accuracy depending on size and graduation of the cylinder (rather inaccurate) 📊🌈 Prepare to Conquer Volumetric Heights with the Majestic Measuring Cylinder! 🧪🔍 This tall and noble container stands proudly, adorned with volume markings that guide us through the world of liquid measurement. 🏰🌟 Its primary duty is to measure and gracefully cradle larger volumes of liquid, holding the secrets of precise measurements within its majestic walls. 💧✨ As you pour the liquid into this regal cylinder, your eyes are drawn to the enchanting meniscus, the captivating curve that adorns the liquid's surface. 🌌🌊 Reading the volume becomes a thrilling quest, as you decipher the secret message at the bottom of this liquid spectacle. 🧪🔬 Let us bow to the magnificence of the measuring cylinder, the loyal guardian of volumetric knowledge in the kingdom of chemistry! 🙌🔍💫 5. Volumetric flask: To prepare solutions with a specific volume, e.g. 250 cm3 , 1000 cm3 , etc., to the nearest 0.10 cm3. 🧪🧪 Prepare to Dive into the World of Precise Liquid Measurements with the Captivating Volumetric Flask! 🔬✨ This exceptional flask, featuring a flat bottom and an elegant long neck, holds the key to unparalleled accuracy in measuring and containing specific volumes of liquid. 🌊🌟 The volumetric flask stands as a symbol of perfection, ensuring that precise measurements are achieved when crafting solutions or dilutions. 🎯🧪 It is the go-to companion when accuracy becomes an art form, promising reliable results and impeccable scientific adventures. 🚀💧 Let's embrace the remarkable volumetric flask, the epitome of precision and the guardian of precise measurements in the vast realm of chemistry! 🙌🔍💫 6. Separating funnel: To separate two immiscible liquids Separating funnel: A separating funnel is a cone-shaped container with a stopcock at the bottom. It is used to separate immiscible liquids (liquids that do not mix) by taking advantage of their different densities. After pouring the liquids into the funnel, you open the stopcock to allow the lower density liquid to separate and collect at the bottom. 7. Beaker: To measure only approximate volumes of liquids, not to be used for precise quantities. It can be also used as a container. 🥼🌪️ Dive into the World of Mixing Marvels with the Versatile Beaker! 🧪🌟 This cylindrical container, boasting a flat bottom and a trusty spout, holds infinite possibilities within its glassy embrace. 💧✨ Known for its prowess in the art of mixing, heating, and cradling larger volumes of liquids or solids, the beaker reigns supreme. 🏆🔥 In the vast realm of the laboratory, beakers of various sizes stand as versatile companions, ready to fulfill a myriad of scientific missions. 🚀🌡️ Let us celebrate the beaker's unwavering presence, an emblem of experimentation and the heart and soul of the laboratory's rhythmic symphony! 🙌🔍🎶 8. Test tube holder: used to hold test tubes while heating them. 🧪🤝 Step into the Realm of Secure Test Tube Handling with the Mighty Test Tube Holder! 🔬✨ This formidable tool stands ready to ensure the safety and stability of test tubes in the thrilling world of experimentation. 🏋️♀️💪 Equipped with a versatile clamp or trusty tongs, it possesses the power to be adjusted and firmly grip the test tube, never letting go. 🚀🔒 The holder becomes an indispensable companion during heating, stirring, and the daring task of transporting test tubes, guaranteeing their safe passage through the realm of scientific exploration. 🌡️🌪️ Let us honor the mighty test tube holder, the unsung hero that upholds the banner of safety and stability in the grand arena of chemical experiments! 🙌🔍💥 9. Wire Gauze: used to allow uniform heat distribution when using a Bunsen-burner. 🔥🔗 Embrace the Fiery Dance with the Spectacular Wire Gauze! 🧪🌟 This fantastic creation, with its square or circular mesh of metal wires, takes center stage in the sizzling chemistry performance. 🎭✨ Placed gracefully on a tripod or support stand, it assumes the role of a reliable platform, lending its support to glassware during the passionate embrace of the Bunsen burner's flame. 🔥💃 As the dance of heat begins, the wire gauze takes on a magical role, orchestrating an enchanting symphony of even heat distribution. 🔥🎶 It ensures that no glassware dares to face the flame directly, safeguarding them from the fiery embrace. 🚫🔥 Let us applaud the remarkable wire gauze, the unsung hero that brings harmony to the realm of heating in the fascinating world of chemistry! 🙌🔍🌈 Common sizes of a pipette: 5, 10, 25 and 50ml. A drop of liquid has a volume of 0.050 ml. From the most to least accurate apparatus: pipette, beaker, cylinder, and burette. Go to Lesson 3 🔎

Filtration Chapter 1 Part 4 SABIS Grade 10 Filtration 💧 Lesson 4: Filtration 💧 Introduction: Welcome to today's lesson on filtration! Have you ever wondered how we can separate a liquid from an insoluble solid? Filtration is the answer! In this lesson, we will explore the process of filtration, its apparatus, and the concept of solubility. Get ready for an exciting journey into the world of separating mixtures! 🔍 Exploring Filtration: Filtration is a technique used to separate a liquid from an insoluble solid. Imagine you have a mixture of sand and water, and you want to separate them. Filtration is the perfect method to accomplish this task. By using a filtration apparatus, we can separate the solid particles from the liquid. 🌊 Solubility - Sugar and Salt: Before we dive into the details of filtration, let's understand a bit about solubility. Solubility refers to the ability of a substance to dissolve in a particular solvent. In this case, we will focus on the solubility of sugar and salt in water. 💧 Sugar's Solubility: Sugar is soluble in water, which means it can dissolve and form a homogenous mixture. Just think about when you stir sugar into a cup of tea or coffee. The sugar particles mix with the water, creating a sweet and tasty drink. 🧂 Salt's Solubility: Similar to sugar, salt is also soluble in water. When you add salt to a glass of water and stir it, the salt particles dissolve, making the water taste salty. This is because the salt molecules break down and become evenly distributed throughout the water. 🍸 Solubility in Alcohol: Now, let's explore the solubility of substances in alcohol. Unlike water, not all substances are soluble in alcohol. 🍬 Sugar's Solubility in Alcohol: Sugar is soluble in alcohol as well. You might have seen bartenders adding sugar to cocktails or using sugar to sweeten alcoholic beverages. The sugar dissolves in the alcohol, enhancing the taste of the drink. 🧂 Salt's Insolubility in Alcohol: On the other hand, salt is not soluble in alcohol. If you try to dissolve salt in alcohol, you'll notice that the salt particles do not break down and remain separate from the alcohol. 🔍 Filtration Apparatus: To carry out the process of filtration, we need specific equipment known as a filtration apparatus. The apparatus consists of several essential components: Beaker or Conical Flask: This is a container where the mixture is initially placed. It provides a suitable environment for the filtration process to take place. Funnel: The funnel is used to direct the mixture into the filter paper. Its shape allows for easy and controlled pouring of the mixture. Filter Paper: Filter paper is a special type of porous paper that acts as a barrier, allowing the liquid to pass through while trapping the solid particles. It is placed inside the funnel to collect the solid residue. Filter Stand: The filter stand holds the funnel securely in place during the filtration process. It ensures stability and prevents any accidental spills. 📝 Filtration Process: Now, let's walk through the filtration process step by step: Step 1: Set up the Filtration Apparatus: Place the filter paper inside the funnel and secure the funnel onto the filter stand. Position the funnel over a clean beaker or conical flask. Step 2: Pour the Mixture: Carefully pour the mixture containing the insoluble solid and liquid into the funnel. The liquid will pass through the filter paper, leaving the solid behind. Step 3: Collect the Filtrate: The liquid that passes through the filter paper is called the filtrate. It collects in the beaker or conical flask placed below the funnel. The filtrate is now separate from the solid. Step 4: Observe the Residue: The solid particles that remain on the filter paper are called the residue. Take a closer look at the residue to observe its characteristics and compare it to the original mixture. 🔍 Conclusion: Congratulations! You've successfully learned about filtration, solubility, and the process of separating solids from liquids. Filtration is a powerful technique that enables us to separate mixtures efficiently. Remember, solubility plays a crucial role in determining which substances can dissolve in a particular solvent. Now, you have the knowledge and skills to apply filtration in various real-life scenarios. So, the next time you encounter a mixture that needs separation, grab your filtration apparatus and embark on your own scientific adventure! Keep exploring and uncovering the wonders of chemistry! 🧪🔬✨ 📚 Multiple-Choice Questions (MCQs): Which of the following best defines filtration? a) Separating a liquid from a soluble solid b) Separating a liquid from an insoluble solid c) Separating two immiscible liquids d) Separating a soluble solid from a gas What is the purpose of using filter paper in the filtration process? a) To collect the liquid b) To trap the solid particles c) To measure the volume of the liquid d) To speed up the filtration process Which of the following substances is soluble in water? a) Sugar b) Sand c) Salt d) Alcohol In which of the following solvents is salt insoluble? a) Water b) Alcohol c) Oil d) Vinegar What is the liquid that passes through the filter paper called? a) Filtrate b) Residue c) Solution d) Precipitate 🖋 Fill-in-the-Blank Questions: Filtration is the process of separating a _________ from an insoluble solid. Sugar is soluble in _________ and _________. The solid left behind on the filter paper after filtration is called _________. The apparatus used for filtration consists of a beaker or conical flask, funnel, filter paper, and filter _________. The liquid that passes through the filter paper is known as the _________. 📝 Answers: MCQs: b) Separating a liquid from an insoluble solid b) To trap the solid particles a) Sugar b) Alcohol a) Filtrate Fill-in-the-Blank Questions: liquid water, alcohol residue stand filtrate Great job! You've completed the quiz on filtration. Keep up the excellent work! 🎉✨🔬 Go To Lesson 5

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Lesson 39 Introduction to the Periodic Table & Families of Elements Chapter 7 SABIS Grade 10 Part 2 Lesson 39 Introduction to the Periodic Table & Families of Elements Chapter 7 Structure of the atom and the periodic table Lesson 1 Content 7.1 Structure of the Atom 7.2 FILM: Chemical Families 7.2.1 Classification of the elements 7.2.2 Investigating the gaseous elements 7.2.3 Investigating H2, F2, Cl2, Br2, I2 7.2.4 Investigating Li, Na, K, Rb, Cs 7.2.5 In conclusion 7.3 The Periodic Table 7.4 The Simplest Chemical Family - The Noble Gases 7.4.1 Physical properties Boiling Points Melting Points 7.4.2 Number of electrons and stability of noble gases Neon, argon, krypton, xenon, radon Sodium chloride forms stable ions 7.5 The alkali metals 7.5.1 Group 1 elements 7.5.2 Theoretical explanation of electrical conductivity 7.5.3 Properties of the alkali metals 7.5.4 Chemistry of the alkali metals 📚Pre-Requisite Questions: Can you list some of the families in the periodic table? 📚 What's special about the Noble Gases? 💎 What makes Alkali Metals different from the Halogens? 🤷♀️ Break for Reflection 🤔✍️ (Answers: 1. Some families in the periodic table are the Alkali Metals, Alkaline Earth Metals, Transition Metals, Halogens, and Noble Gases. 2. Noble Gases are special because they have a full valence electron shell and are mostly non-reactive. 3. Alkali Metals are very reactive and have one electron in their outer shell, while Halogens are also reactive and have seven electrons in their outer shell.) 🚀 Lesson Begins! 💫 Chemical Families Just as human families have common traits, elements in the same chemical family share common properties. This is because they have the same number of valence electrons. It's like family members having the same eye color! 👀 ⚗️ The Noble Gases Noble gases are like the aristocrats of the periodic table - they're a bit aloof and tend not to react with other elements because their electron shells are full. They're the cool kids, hard to impress! 🕶️ 🔥 The Alkali Metals The Alkali Metals, on the other hand, are the life of the party! 🎉 They have one electron in their outer shell and are ready to react at the drop of a hat. They're like your friend who's always up for a new adventure. 🎢 🌩️ The Halogens Then come the Halogens, who are just one electron short of having a full outer shell. They're eager to form a bond with any element that can provide that one extra electron. They're like someone looking for their perfect match! 🤝 💡In conclusion: Chemistry is not just about memorizing the periodic table or complex equations. It's about understanding the relationships and interactions between different elements. It's about seeing the beauty in the organization and the patterns that emerge. It's about appreciating the elegant dance of atoms and molecules. 🌐 Review Questions: Which family of elements is generally non-reactive because their electron shells are full? a. Alkali Metals b. Halogens c. Noble Gases d. Transition Metals Why are Alkali Metals so reactive? a. They have a full outer shell b. They are one electron short of a full outer shell c. They have one electron in their outer shell ready to be given away d. They are shiny and malleable Which family of elements is eager to form bonds to gain one extra electron? a. Alkali Metals b. Halogens c. Noble Gases d. Transition Metals (Answers: 1. c, 2. c, 3. b) End of Lesson 2 ⭐Keep studying, keep learning!⭐

046f1805-79e0-4c9e-acb6-58f89c358f76 Cooling Curve Summary A graphical representation of the relationship between temperature and time as a substance cools.

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