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What are we expecting from you? 1. Do’s Find a clean, quiet space and dress appropriately. Let all household members know when and where you will be in class, and ask them not to disturb you. Make sure your full name shows up appropriately. Be aware of your background, lighting, and noise. Mute until you are required to talk. Use the Zoom functions to communicate if needed (chat, raise your hand, answer yes/no, etc.). Use an appropriate zoom background if you wish. Turn off/silence cell phone and close other windows on your computer. Be on time to class. Communicate with your instructor (via their preferred communication method listed on the syllabus) if you will be late or if you lose your connection during class. Pay attention! Maintain eye contact with the speaker on the screen. Be prepared to take notes (on your computer or in a designated notebook) or to access course material (have textbook, D2L course page, or readings available). 2. Don’ts Enter a zoom that you weren't invited to, share the zoom access information for your class with others, or enter under a different name. Take screenshots, cell phone pictures, or otherwise record the meeting, your classmates, or your instructor without express permission to do so. Change your name or change your zoom background during the meeting. Walk around during the class meeting. Use the chat for side conversations with classmates. Sit in front of a window or bright light, this will make your face too dark to see. Have conversations with household members off camera. Allow household members to walk around behind you during the meeting. Engage in texting, social media, work from other classes, or other distractions while in class Frequently asked questions

< Back Chapter 5: Stoichiometry Discover the quantitative relationships between reactants and products in chemical reactions and learn how to apply stoichiometric calculations. Chapter 5: Stoichiometry - This chapter covers the calculations involved in chemical reactions. Students will learn how to balance chemical equations, calculate limiting reactants, and determine percent yield. The chapter also covers the mole concept and how to use it in stoichiometry problems. Previous Next

< Back Naming Organic Compounds Files Download Day 5 Notes Naming Compounds The IGCSE Organic Chemistry Challenge .pdf Download PDF • 8.70MB Notes Topic Exercise Answers Naming Compounds HW The 30-Day IGCSE Organic Chemistry Challenge .pdf Download PDF • 11.41MB Naming Organic Compounds IGCSE 0620 .pdf Download PDF • 13.89MB Videos Previous Next

Activation energy: definition in SABIS Grade 10 SABIS as activated complex (AC). The AC i activated complex s found at the highest point of the potential energy curve. It is an unstable structure with energy higher than both reactants and products.

A stable compound has a low level of potential energy. Grade 10 SABIS

< Back Fuels and Petroleum Exploring the World of Fossil Fuels: Names, Extraction, and Uses of Petroleum Fractions Files Download DAY 1,2 The 60-Day IGCSE Organic Chemistry Challenge .pdf Download PDF • 25.65MB DAY 3 The 60-Day IGCSE Organic Chemistry Challenge .pdf Download PDF • 4.58MB Notes Topic Exercise Answers Hw fuels unanswered_230330_144316 .pdf Download PDF • 9.36MB Fuels HW The 60-Day IGCSE Organic Chemistry Challenge .pdf Download PDF • 8.24MB Videos Previous Next

< Back This is a Title 03 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

< Back Chapter 4: Electrochemistry Learn about the study of chemical reactions involving the transfer of electrons and their applications in various fields. Chapter 4: Electrochemistry - This chapter explores the relationship between electricity and chemical reactions. Students will learn about oxidation-reduction reactions, electrochemical cells, and the Nernst equation. The chapter also covers the applications of electrochemistry, including batteries and electrolysis. Previous Next

< 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 💎🔬 Purification 🔬💎 Purification involves using electrolysis to remove impurities from a metal. For instance, in the purification of copper: The cathode (-ve electrode) is pure copper. The anode (+ve electrode) is impure copper. The electrolyte is aqueous copper (II) sulfate. During electrolysis, copper ions (Cu2+) in the electrolyte are reduced (gain electrons) at the cathode and become solid copper atoms. Meanwhile, solid copper atoms at the anode are oxidized (lose electrons) and become copper ions (Cu2+), entering the electrolyte. This maintains the electrolyte's concentration, as the ions being deposited on the cathode are replaced by the ions from the anode. Any impurities in the anode copper do not dissolve and fall to the bottom. ⚗️🧪 Electroplating 🧪⚗️ Electroplating is a process that uses electrolysis to coat a metal object with a thin layer of another metal. The primary purposes of electroplating are to enhance the object's appearance and to protect it from corrosion. In a typical electroplating process: The cathode (-ve electrode) is the object to be electroplated. The anode (+ve electrode) is the metal used for coating (for example, silver). The electrolyte is a solution containing ions of the metal used for coating (for example, silver nitrate). As electrolysis proceeds, metal ions from the electrolyte are reduced at the cathode and become solid metal atoms, adhering to the object's surface. Meanwhile, at the anode, the metal is oxidized and releases ions into the electrolyte, maintaining its concentration. It's crucial to ensure the object to be electroplated is clean and entirely immersed in the electrolyte. Also, rotating it can help achieve an even coating. Regarding your reference to a past paper question (Specimen 2023, 2, q30), could you provide more context or the actual question? Unfortunately, I can't access specific past papers beyond my knowledge cut-off in September 2021. However, I'd be more than happy to help if you could provide more details about the question! Press Next for the next lesson Electricity Lesson 3 Next Topic

< Back Chapter 7 Pre requisite Previous Next 🌟📘 Prerequisites for Chapter 7: Redox Reactions 📘🌟Before diving into Chapter 7, which deals with redox reactions, students must have a solid understanding of the following concepts: 🔬 1. Basic Chemistry Concepts 🧪Understand atoms, molecules, ions, and chemical reactions. 🔬 2. Oxidation States 🔄Understand how to assign oxidation states to atoms in a molecule or ion. 🔬 3. Balancing Chemical Equations ⚖️Be able to write and balance chemical equations. 🔬 4. The Mole Concept 🐾Understand the concept of moles and Avogadro's number. 🌟 20 Multiple Choice Questions for Chapter 7: Redox Reactions 🌟What is the oxidation state of oxygen in H₂O? a) -2 b) -1 c) 0 d) +2In a redox reaction, the substance that is reduced... a) gains electrons. b) loses electrons. c) gains protons. d) loses protons.What is the oxidation state of hydrogen in H₂? a) -1 b) 0 c) +1 d) +2What is the term for a reaction in which both oxidation and reduction occur? a) Displacement reaction b) Redox reaction c) Combination reaction d) Decomposition reactionWhat is the oxidation state of sulfur in SO₄²⁻? a) +4 b) +6 c) -2 d) 0In the reaction 2H₂ + O₂ -> 2H₂O, what is the oxidizing agent? a) H₂ b) O₂ c) H₂O d) None of the aboveWhat is the sum of the oxidation states of all atoms in a neutral molecule? a) 0 b) 1 c) -1 d) 2What is the term for an atom or molecule that has lost electrons? a) Cation b) Anion c) Reductant d) OxidantIn a redox reaction, the substance that is oxidized... a) gains electrons. b) loses electrons. c) gains protons. d) loses protons.What is the oxidation state of chlorine in Cl₂? a) -1 b) 0 c) +1 d) +2What is the term for a substance that causes the oxidation of another substance? a) Oxidizing agent b) Reducing agent c) Catalyst d) SolventIn the reaction Zn + Cu²⁺ -> Zn²⁺ + Cu, what is the reducing agent? a) Zn b) Cu²⁺ c) Zn²⁺ d) CuWhat is the oxidation state of carbon in CO₂? a) -4 b) -2 c) +2 d) +4What is the term for a reaction in which electrons are transferred between species? a) Acid-base reaction b) Precipitation reaction c)Redox reaction d) Substitution reactionIn the reaction 2Na + Cl₂ -> 2NaCl, what is the oxidizing agent? a) Na b) Cl₂ c) NaCl d) None of the aboveWhat is the oxidation state of nitrogen in NO₃⁻? a) +3 b) +4 c) +5 d) -3What is the term for a substance that causes the reduction of another substance? a) Oxidizing agent b) Reducing agent c) Catalyst d) SolventIn the reaction 2Al + 3Cu²⁺ -> 2Al³⁺ + 3Cu, what is the oxidizing agent? a) Al b) Cu²⁺ c) Al³⁺ d) CuWhat is the oxidation state of iron in Fe₂O₃? a) +2 b) +3 c) -2 d) -3In a redox reaction, what happens to the oxidation state of an element that is reduced? a) It increases. b) It decreases. c) It remains the same. d) It becomes zero. 🌟 Answers 🌟a) -2a) gains electrons.b) 0b) Redox reactionb) +6b) O₂a) 0a) Cationb) loses electrons.b) 0a) Oxidizing agenta) Znd) +4c) Redox reactionb) Cl₂c) +5b) Reducing agentb) Cu²⁺b) +3b) It decreases.I will now proceed to create prerequisites, questions, and answers for Chapter 8: Equilibrium. Please let me know if you would like me to continue in the same message or create a new message for each chapter.

< Back Chapter 2: Solubility Understand the concepts of solubility and how different factors affect the solubility of substances in different solvents. Chapter 2: Solubility - This chapter focuses on the solubility of substances in water and other solvents. Students will learn about solubility rules, solubility products, and how to calculate the solubility of a substance. The chapter also covers the common ion effect and how it affects solubility. Previous Next