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< Back Grade 10 Material Revision Are you a Grade 11 SABIS chemistry student looking to refresh your memory and solidify your understanding of the material you studied in Grade 10? Look no further than our dedicated webpage designed to help you revise key concepts and skills! Our webpage is packed with engaging and interactive content that is tailored to meet your revision needs. We have organized the material by topic and included multimedia resources such as videos, animations, and images to help you better understand abstract concepts. Plus, we have included practice questions throughout the page to help you test your knowledge and identify areas where you need to focus your revision. But that's not all! Our webpage also provides additional resources such as links to relevant websites, books, and articles to help you delve deeper into the topics that interest you most. And with interactive features such as quizzes and games, we've made revising chemistry a fun and engaging experience! We've designed this webpage specifically for you, the Grade 11 SABIS chemistry student, to help you review the material you studied in Grade 10 and prepare for the challenges of the year ahead. So why wait? Start exploring our webpage today and take the first step towards mastering chemistry! Previous Next Material Discussed Glassware : Volumetric Flask Burette Pipette Measuring Cylinder Conical Flask States of Matter States of Matter conversion Boiling Evaporation Melting Freezing Sublimation

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Properties of helium: a monatomic gas, has a very low boiling point, cannot be solidified at any temperature unless it subjected to pressure, unreactive. Grade 10 SABIS

Mole Grade 10 SABIS SABIS A unit used in chemistry to count entities at the atomic and molecular scale. One mole contains Avogadro's number of entities (6.022 x 10^23).

Volume at STP Grade 10 SABIS SABIS 1.00 mole of ANY gas occupies 22.4 dm3

2 carry out calculations using cycles and relevant energy terms, including: (a) determining enthalpy changes that cannot be found by direct experime A Level Chemistry CIE Applying Hess's Law is a powerful method in thermochemistry that allows us to calculate the overall enthalpy change of a reaction using known enthalpy changes of other reactions. This principle is based on the concept that enthalpy is a state function, meaning it depends only on the initial and final states of a system and not on the path taken. To construct a simple energy cycle using Hess's Law, we start with a target reaction for which we want to determine the enthalpy change. This target reaction may not have direct experimental data, but we can use known enthalpy changes of other reactions to derive the desired enthalpy change. The key idea is to break down the target reaction into a series of intermediate reactions, known as the "thermochemical equations," for which we have the corresponding enthalpy changes. By carefully selecting and manipulating these equations, we can cancel out common reactants and products to obtain the desired target reaction. For example, suppose we want to determine the enthalpy change for the combustion of methane (CH4). However, we don't have direct experimental data for this specific reaction. We can construct an energy cycle using known enthalpy changes of reactions involving the combustion of other compounds, such as hydrogen (H2) and carbon monoxide (CO). First, we identify the known reactions that can be used to build the energy cycle. In this case, we can use the combustion reactions of H2 and CO, for which we have the corresponding enthalpy changes. These reactions become the intermediate steps in the energy cycle. Next, we manipulate the intermediate reactions and their enthalpy changes to cancel out common species and align the stoichiometry with the target reaction. This can involve reversing reactions, multiplying them by coefficients, or combining multiple reactions to achieve the desired cancellation. By summing up the enthalpy changes of the manipulated intermediate reactions, taking into account the stoichiometric coefficients, we obtain the overall enthalpy change for the target reaction. This value represents the enthalpy change that would be measured if the reaction were directly carried out under standard conditions. It's important to note that the validity of applying Hess's Law relies on the assumption that enthalpy changes are additive. This assumption holds as long as the reactions occur under the same conditions and there is no change in temperature or pressure during the process. By applying Hess's Law and constructing simple energy cycles, we can determine the enthalpy changes of reactions that are difficult or impractical to measure directly. This approach provides a powerful tool for calculating enthalpy changes and understanding the energy transformations in chemical reactions. In summary, applying Hess's Law involves constructing energy cycles using known enthalpy changes of intermediate reactions to determine the enthalpy change of a target reaction. By manipulating and combining these reactions, we can cancel out common species and obtain the desired enthalpy change. This method allows us to calculate enthalpy changes for reactions that lack direct experimental data and enhances our understanding of energy transformations in chemical systems.

< Back Atomic Structure Lesson 2 ⚛️ Lesson 2 ⚛️ This section delves into the mass and charge distributions within the atom, emphasizing the nucleus as the center of mass and the dance of electrostatic attraction that holds the atom together, while also highlighting the distinct movements of electrons, protons, and neutrons in an electric field. Previous Next ⚛️ 1.1.2 Mass, Charge & Subatomic Particles ⚛️ ✨🔬 Unmasking the Atom: Unveiling Mass & Charge Distributions 🔬✨ 1️⃣ The Mighty Nucleus: A Mass Reservoir 🏋️♀️🎯 Like a dense treasure chest in the heart of the atom, the nucleus is where the hefty subatomic heroes reside—the mighty protons and neutrons. They hoard nearly all of the atom's mass, with their combined weight making the nucleus the weightlifting champion of the atomic world. 🏆🌍 2️⃣ Electrons: The Lightweight Performers 💃⚡ Flirting around this massive nucleus, you'll find the feathery electrons. Their mass is so negligible, they're like tiny dancers pirouetting around a grand stage. Despite their lightness, they wear cloaks of negative charge, creating a bustling 'cloud' of negativity around the positive heart of the atom. ⛅💨 3️⃣ The Atom's Secret Glue: Electrostatic Attraction 🔗🧲 And what stops these nimble electrons from flitting away? The invisible ties of electrostatic attraction! The positive nucleus and negative electrons are drawn to each other, a captivating dance of opposite charges that keeps the atom together. 💖 ✨🎢 Subatomic Particles: Performers in an Electric Field 🎢✨ 1️⃣ The Electron's Graceful Waltz 🩰🌀 Imagine our subatomic performers, each moving at the same pace, but through a charged, electric stage. The electron, wearing its negative charge, is deflected away from the negative plate and is lured towards the positive plate with ease. This behavior not only proves its negative charge but also showcases its incredibly small mass as it pirouettes nimbly in the electric field. 🎭💫 2️⃣ The Proton's Powerful Stride 🏃♂️⚡ In contrast, the proton, with its positive charge, displays a different performance. It strides away from the positive plate and towards the negative one, asserting its positive nature. But compared to the electron's swift deflection, the proton's move is less pronounced, hinting at its greater mass. 💪🎖️ 3️⃣ The Neutron's Neutral Stand 🧍♂️🎭 What about the neutron? Well, the neutron, true to its neutral character, remains unaffected by the charged plates. It does not veer towards or shy away from either plate, simply continuing its journey unaffected—an applause-worthy performance proving its neutral nature. 👏🎭 So, there you have it—our subatomic performers illuminating the atom's inner workings through their mesmerizing dance in the atomic world and electric field! 🌠🌌 Quiz: Mass, Charge & Subatomic Particles ✨🔬 Unmasking the Atom: Unveiling Mass & Charge Distributions 🔬✨ Complete the missing words in the following questions: What resides in the nucleus and holds nearly all of the atom's mass? Answer: 🌟 Protons and neutrons Electrons have __________ mass compared to protons and neutrons. Answer: 🌌 Negligible/lightweight What creates an electric field that influences the movement of charged particles? Answer: 🔋 Charged plates Electrons are ____________ to the positive nucleus due to electrostatic attraction. Answer: 💞 Attracted In an electric field, electrons are deflected ____________ from the negative plate and toward the positive plate. Answer: 🌪 Away The proton, with its positive charge, moves ____________ from the positive plate and toward the negative plate in an electric field. Answer: 💥 Away Neutrons remain ____________ by the charged plates in an electric field due to their neutral nature. Answer: 🌟 Unaffected Protons have a ____________ mass compared to electrons. Answer: 💪 Greater The electron's movement in an electric field showcases its ____________ charge and small mass. Answer: 💫 Negative Neutrons demonstrate their ____________ nature by not veering towards or away from the charged plates in an electric field. Answer: 👏 Neutral Keep up the great work in understanding the mesmerizing dance of subatomic particles and their role in the atom's mass and charge distributions! 🎉🌠

< Back Chemical bonding This is placeholder text. To change this content, double-click on the element and click Change Content. This is placeholder text. To change this content, double-click on the element and click Change Content. Want to view and manage all your collections? Click on the Content Manager button in the Add panel on the left. Here, you can make changes to your content, add new fields, create dynamic pages and more. You can create as many collections as you need. Your collection is already set up for you with fields and content. Add your own, or import content from a CSV file. Add fields for any type of content you want to display, such as rich text, images, videos and more. You can also collect and store information from your site visitors using input elements like custom forms and fields. Be sure to click Sync after making changes in a collection, so visitors can see your newest content on your live site. Preview your site to check that all your elements are displaying content from the right collection fields. Previous Next 🔬 Chapter 4: Chemical Bonding 🔬 Learning Outcomes 🎯: Describe different types of bonding using dot-and-cross diagrams, including ionic, covalent, and co-ordinate (dative covalent) bonding. Explain shapes and bond angles in molecules using electron-pair repulsion. Describe covalent bonding in terms of orbital overlap, sigma and pi bonds, and hybridization. Explain terms like bond energy, bond length, and bond polarity. Describe intermolecular forces based on permanent and induced dipoles, hydrogen bonding, and metallic bonding. Deduce the type of bonding present from given information. (Page 48) Van der Waals’ Forces 💨: Van der Waals’ forces are weak forces of attraction between atoms or molecules. They arise due to temporary dipoles set up by the movement of electron charge clouds. These forces increase with the increasing number of electrons and contact points between molecules. They play a significant role in the boiling points of noble gases and other substances. (Page 14) Bond Length and Bond Energy ⚛️: Double bonds are shorter and stronger than single bonds. Bond energy is the energy needed to break one mole of a given bond in a gaseous molecule. Bond strength influences the reactivity of a compound. (Page 6) Metallic Bonding 🧲: Metals have a giant metallic structure with positive ions surrounded by a sea of delocalized electrons. This structure explains why metals are good conductors of electricity and have high melting points. (Page 22) Hydrogen Bonding and Boiling Point 🌡️: Hydrogen bonding can cause compounds to have higher boiling points than expected. Water has a much higher boiling point and enthalpy change of vaporization due to extensive hydrogen bonding. (Page 17)

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