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Prepare for your AQA IGCSE Oxford Chemistry Exam with our comprehensive collection of syllabus material, tuition videos, notes, and study guides. Our resources cover essential topics including acids and bases, chemical reactions, and organic chemistry. With easy-to-follow materials, gain confidence in your knowledge and ability to answer exam questions with ease. , our AQA IGCSE Oxford Chemistry Exam study materials are perfect for students, tutors, and parents alike. E Past Paper Replacement Specimens and Mock Exams now to the help Specimen Past Papers Download OXFORD AQA IGCSE Chemistry 9202

Explain the Changes of state in terms of the Kinetic Theory Trending Now The 60-Day IGCSE Organic Chemistry Challenge DAY 1 Free Preview The 60-Day IGCSE Organic Chemistry Challenge DAY 2 Free Preview IGCSE CHEMISTRY CAMBRIDGE 1.Particulate Nature of Matter 1.3 Heating Curve Back to Chapter 1 Menu Notes : Heating and Cooling curves are Graphs that show how matter acts when changing the temperature and at which state substance is available versus time Changes of states can be explained by using the idea that particles are constantly in motion . This is called the kinetic particle theory we can explain a heating curve using ideas about the energy and motion of the particles. Heating Curve At point A Physical status is Solid From A to B increasing heat energy increases vibration of the solid particles so the temperature of the solid increases From B to C increasing the heat weakens the forces of attraction between particles so they begin to slide over each other . there is no temperature change because all energy supplied is used to overcome the forces between the particles instead of raising the temperature . the substance melts At C , the substance is all at liquid state. From C to D : increasing the energy increases the motion of the particles in the liquid so the temperature of the liquid increases. From D to E : forces of attraction between liquid particles weakens to particles start to move away from each other . there is no temperature change as the energy supplied is used to break the forces between the particles , the substance boils . From E to F : increasing the energy increases the speed of the gas particles . so the temperature increases and the gas particles are getting far away from each other. Cooling Curve Almost opposite is happening List of Topics Download as PDF Trending Now The 60-Day IGCSE Organic Chemistry Challenge DAY 1 Free Preview The 60-Day IGCSE Organic Chemistry Challenge DAY 2 Free Preview K-Chemistry About US READ MORE

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1.1 States of Matter 1.2 Changes in states of matter 1.3 Heating Curve 1.4 Diffusion 1.Particulate Nature of Matter IGCSE CHEMISTRY CAMBRIDGE Presentation Notes : 1.1 States Of Matter 1.2 Changes in States of Matter 1.3 Heating Curve 1.4 Diffusion List of Topics

< Back States of matter Previous Next 🔬 Chapter 5: States of Matter 🔬 Learning Outcomes 🎯: State the basic assumptions of the kinetic theory as applied to an ideal gas. Explain qualitatively in terms of intermolecular forces and molecular size, the conditions necessary for a gas to approach ideal behavior. State and use the general gas equation pV = nRT in calculations. Describe, using a kinetic-molecular model, the liquid state, melting, vaporization, and vapor pressure. Describe in simple terms the lattice structures of crystalline solids, including ionic, simple molecular, giant molecular, hydrogen bonded, or metallic. Discuss the finite nature of materials as a resource and the importance of recycling processes. Outline the importance of hydrogen bonding to the physical properties of substances, including ice and water. Recycling Materials ♻️: Recycling metals saves energy, conserves supplies of the ore, reduces waste, and is often cheaper than extracting metals from their ores. Recycling copper is important due to the low percentage of copper in most remaining ores and the energy savings in recycling compared to extraction. Recycling aluminum is much cheaper than extracting it from bauxite ore, and there is a 95% saving in energy by recycling aluminum compared to extracting it from its ore. The Gaseous State 💨: The kinetic theory of gases assumes that gas molecules move rapidly and randomly, the distance between gas molecules is much greater than the diameter of the molecules, there are no forces of attraction or repulsion between the molecules, and all collisions between particles are elastic. The Liquid State 💧: When a solid is heated, the energy transferred makes the particles vibrate more vigorously, the forces of attraction between the particles weaken, and the solid changes to a liquid (melting). In a liquid, particles are close together but have enough kinetic energy to slide past each other. Vaporization is the change from the liquid state to the gas state, and the energy required for this change is called the enthalpy change of vaporization. The Solid State 🧱: Solids have fixed shape and volume, with particles touching each other and usually arranged in a regular pattern. The state of a substance at room temperature and pressure depends on its structure and bonding, including simple atomic, simple molecular, giant ionic, giant metallic, and giant molecular structures.

< Back Chemical Thermodynamics Prerequisites Prerequisite Previous Next 🌟📘 Prerequisites for Chapter 6: Chemical Thermodynamics 📘🌟 Before diving into Chapter 6, which deals with chemical thermodynamics, students must have a solid understanding of the following concepts: 🔬 1. Basic Chemistry Concepts 🧪 Understand atoms, molecules, and chemical reactions. 🔬 2. Energy and Heat 🔥 Understand the concept of energy and the difference between heat and temperature. 🔬 3. Chemical Bonds 💪 Understand the energy involved in the formation and breaking of chemical bonds. 🔬 4. The Mole Concept 🐾 Understand the concept of moles and Avogadro's number. 🔬 5. Basic Mathematics 🧮 Be comfortable with algebra and solving equations. 🌟 20 Multiple Choice Questions to Check Mastery of Prerequisites 🌟 What is the smallest unit of an element that retains the properties of that element? a) Molecule b) Atom c) Electron d) Compound What is the energy called that is needed to break a chemical bond? a) Activation energy b) Bond energy c) Kinetic energy d) Potential energy How many atoms are in one mole of a substance? a) 6.022 x 10²³ b) 12 c) 1000 d) 1 What is the standard unit of temperature? a) Kelvin b) Celsius c) Fahrenheit d) Rankine What is the energy change of a system called? a) Enthalpy b) Entropy c) Heat d) Work What is the heat absorbed or released at constant pressure called? a) Internal energy b) Entropy c) Enthalpy d) Work What is the standard unit of energy? a) Joule b) Calorie c) Watt d) Newton What is the term for a reaction that absorbs heat from the surroundings? a) Exothermic b) Endothermic c) Isothermal d) Adiabatic What is the term for the average kinetic energy of particles in a substance? a) Heat b) Temperature c) Enthalpy d) Entropy Which law states that energy cannot be created or destroyed? a) First Law of Thermodynamics b) Second Law of Thermodynamics c) Hess's Law d) Law of Conservation of Mass What is the heat content of a system at constant pressure called? a) Internal energy b) Entropy c) Enthalpy d) Work What type of reaction releases heat to the surroundings? a) Exothermic b) Endothermic c) Isothermal d) Adiabatic What is the heat transfer into or out of a system called? a) Internal energy b) Entropy c) Enthalpy d) Heat What is the standard unit of pressure? a) Pascal b) Atmosphere c) Torr d) Bar What is the term for the heat transfer that occurs with no change in temperature? a) Latent heat b) Specific heat c) Enthalpy d) Entropy What is the term for the disorder or randomness of a system? a) Internal energy b) Entropy c) Enthalpy d) Heat In an exothermic reaction, the energy of the products is _______ than the energy of the reactants. a) Higher b) Lower c) The same d) Cannot be determined What is the heat required to raise the temperature of 1 gram of a substance by 1 degree Celsius called? a) Latent heat b) Specific heat c) Enthalpy d) Entropy What is the term for a reaction where the reactants and products are in equilibrium with each other? a) Dynamic equilibrium b) Static equilibrium c) Chemical equilibrium d) Physical equilibrium What is the term for the minimum energy required for a chemical reaction to occur? a) Activation energy b) Bond energy c) Kinetic energy d) Potential energy 🌟 Answers 🌟 b) Atom b) Bond energy a) 6.022 x 10²³ a) Kelvin a) Enthalpy c) Enthalpy a) Joule b) Endothermic b) Temperature a) First Law of Thermodynamics c) Enthalpy a) Exothermic d) Heat a) Pascal a) Latent heat b) Entropy b) Lower b) Specific heat a) Dynamic equilibrium a) Activation energy

⚛️ Lesson 3 ⚛️ < Back Atomic Structure Lesson 3 ⚛️ Lesson 3 ⚛️ This section explores the subatomic structure of atoms and ions, highlighting the role of protons as unchanging identifiers of elements and the flexible nature of electrons in forming ions. The calculation of protons, neutrons, and electrons in an unknown element is demonstrated, unveiling the subatomic structure and identity of the element. Understanding these concepts allows us to uncover the hidden structure of the universe, atom by atom. Previous Next ⚛️ 1.1.3 Determining Subatomic Structure ⚛️ 💥🔬 Cracking the Code of Subatomic Structures: Protons, Electrons, and Neutrons 🔬💥 ⚛️ Atoms & Ions: A Tale of Charges ⚛️ Imagine an atom as a tiny city, bustling with life and balance. At its heart, it's neutral—like a well-managed city where everyone has a role to play. But sometimes, atoms get adventurous! They might lose or gain citizens (electrons), leading to charged cities we call ions. ⚡🌆 💫 Protons: The Unchanging Pillars of Atomic Identity 💫 The number of protons is like the DNA of an atom—it doesn't change and identifies the element. Be it the lithium city with 3 protons or the beryllium city with 4, every atom and ion of the same element shares the same proton number (atomic number). So, how do we count these unchanging pillars (protons) in an unknown element? With some simple math! 🧮📚 Mass number = number of protons + number of neutrons Number of protons = mass number - number of neutrons 💡 E.g., for an unknown element X with a mass number of 63 and 34 neutrons: Number of protons = 63 - 34 = 29 🎉 We just revealed the identity of element X—it's copper! 🥳🎉 💨 Electrons: The Flexible Players 💨 While protons are the steadfast pillars, electrons are more flexible—they may change in ions. In a neutral atom, the number of electrons equals the number of protons. But ions dance to a different tune: positively charged ions (cations) have fewer electrons, and negatively charged ions (anions) have more! 🎶🔄 For our mystery element X: Number of protons (and electrons in a neutral atom) = 29 🎯 ⚖️ Neutrons: The Balancing Act ⚖️ And finally, let's not forget the neutrons. They don't carry any charge but contribute to the mass. We can find their number with another bit of math: Number of neutrons = mass number - number of protons 🔍 E.g., for our element X with a mass number of 63 and 29 protons: Number of neutrons = 63 - 29 = 34 🎉 Just like that, we've unveiled the full subatomic structure of element X—Copper with 29 protons, 29 electrons, and 34 neutrons! 🔍🔬 By understanding these concepts, you're not just learning chemistry—you're uncovering the unseen structure of the universe, one atom at a time! 💥🌌 What can atoms become when they gain or lose electrons? A) Ions 🌟 B) Neutrons 🧪 C) Protons ⚡ D) Isotopes 🔬 The number of __________ determines the identity of an element. A) Electrons 💫 B) Protons ⚛️ C) Neutrons ⚡ D) Isotopes 🌌 How can we calculate the number of protons in an unknown element? A) Mass number + number of neutrons 🧮 B) Mass number - number of neutrons 📚 C) Number of neutrons + number of electrons 🌟 D) Number of electrons - number of neutrons 💡 What is the charge of a neutral atom? A) Positive ⚡ B) Negative 💥 C) Neutral 🔋 D) Variable 🌈 What happens to the number of electrons in ions? A) They remain the same as in neutral atoms. 🔁 B) They decrease in cations and increase in anions. ⬇️⬆️ C) They increase in cations and decrease in anions. ⬆️⬇️ D) They become neutral. ⚖️ In a neutral atom, the number of electrons is equal to the number of __________. A) Protons 🌟 B) Neutrons 🌌 C) Ions ⚛️ D) Isotopes 🔬 Which subatomic particles contribute to the mass of an atom? A) Protons and electrons 💥💫 B) Protons and neutrons 🧪⚛️ C) Electrons and neutrons ⚡🌌 D) Protons, electrons, and neutrons 🔬💥💫 How can we calculate the number of neutrons in an atom? A) Mass number - number of protons 🧮 B) Mass number + number of protons 📚 C) Number of protons - number of electrons 🔍 D) Number of protons + number of electrons 💡 Copper has an atomic number of 29. How many protons does a copper atom have? A) 29 🌟 B) 63 🔬 C) 34 🧪 D) 0 💥 An element has a mass number of 47 and 20 neutrons. How many protons does it have? A) 20 🌌 B) 27 ⚛️ C) 47 🧪 D) 67 🌟 Keep up the great work in unraveling the mysteries of subatomic structures and their impact on determining the identity of elements! Let your vibrant and creative knowledge shine brightly! 🌟🔬💫

Exploring the Energetic World of Chemical Reactions and Thermodynamics < Back Chemical energetics Exploring the Energetic World of Chemical Reactions and Thermodynamics Introduction to Chemical Energetics: Definition and scope of chemical energetics in the context of A Level Chemistry. Importance of understanding energy changes in chemical reactions. Thermodynamics and Energy: Fundamental principles of thermodynamics and their application to chemical systems. Overview of energy transfer, work, and heat in chemical reactions. Enthalpy and Enthalpy Changes: Definition and significance of enthalpy in chemical reactions. Calculation and interpretation of enthalpy changes (∆H) using Hess's Law and bond enthalpies. Spontaneity and Gibbs Free Energy: Understanding spontaneity and the concept of Gibbs free energy (∆G) in determining reaction feasibility. Relationship between enthalpy, entropy, and temperature in predicting reaction spontaneity. Bond Energies and Thermochemical Equations: Exploring bond energies and their role in quantifying energy changes in chemical reactions. Use of thermochemical equations to calculate enthalpy changes. Standard Enthalpy Changes and Standard Conditions: Definition and determination of standard enthalpy changes (∆H°) under standard conditions. Application of standard enthalpy changes in calculating reaction enthalpy. Calorimetry and Heat Measurements: Introduction to calorimetry as a technique for measuring heat changes in chemical reactions. Practical aspects of conducting calorimetric experiments and data analysis. Hess's Law and Born-Haber Cycles: Understanding Hess's Law and its application to determine enthalpy changes indirectly. Introduction to Born-Haber cycles for calculating enthalpy changes in lattice energy and formation reactions. Thermodynamic Stability and Chemical Equilibrium: Relationship between energy changes and the stability of chemical species. Linking energy changes to the concept of chemical equilibrium. Energy Diagrams and Reaction Profiles: Construction and interpretation of energy diagrams (reaction profiles) for exothermic and endothermic reactions. Analysis of activation energy and reaction rate in relation to energy diagrams. Previous Next The Following Learning outcomes and topics are studied in the A Level Chemistry 5.1 Enthalpy change, ΔH Learning outcomes Candidates should be able to: 1 understand that chemical reactions are accompanied by enthalpy changes and these changes can be exothermic (ΔH is negative) or endothermic (ΔH is positive) 2 construct and interpret a reaction pathway diagram, in terms of the enthalpy change of the reaction and of the activation energy 3 define and use the terms: (a) standard conditions (this syllabus assumes that these are 298K and 101 kPa) shown by ⦵. (b) enthalpy change with particular reference to: reaction, ΔHr , formation, ΔHf , combustion, ΔHc , neutralisation, ΔHneut 4 understand that energy transfers occur during chemical reactions because of the breaking and making of chemical bonds 5 use bond energies (ΔH positive, i.e. bond breaking) to calculate enthalpy change of reaction, ΔHr 6 understand that some bond energies are exact and some bond energies are averages 7 calculate enthalpy changes from appropriate experimental results, including the use of the relationships q = mcΔT and ΔH = –mcΔT/n 5.2 Hess’s Law Learning outcomes Candidates should be able to: 1 apply Hess’s Law to construct simple energy cycles 2 carry out calculations using cycles and relevant energy terms, including: (a) determining enthalpy changes that cannot be found by direct experiment (b) use of bond energy data

Previous All Content Next Chapter 3 SABIS Grade 10 Part 4 ✅Lesson 13✅: Avogadro's Number and Molar Mass 🧪📊 Let's dive into the fascinating world of Avogadro's number and molar mass! 🚀 📝 Prerequisite Quiz 📝 Choose the correct answer for each question: Avogadro's number represents the number of particles in _______. A) 1 mole of gas B) 1 gram of gas C) 1 liter of gas D) 1 cubic meter of gas A mole is defined as _______. A) 6.02 × 10²³ particles B) 6.02 × 10⁻²³ particles C) 6.02 × 10²³ grams D) 6.02 × 10⁻²³ grams Atomic mass units (amu) were introduced because _______. A) the masses of atoms and molecules are too large to be measured in grams B) the masses of atoms and molecules are too small to be measured in grams C) the masses of atoms and molecules cannot be accurately measured D) the masses of atoms and molecules are equal to their number of particles The atomic mass of carbon-12 is defined as _______. A) 12 amu B) 6 amu C) 1 amu D) 24 amu The conversion factor from grams to amu is _______. A) 1 gram = 6.02 × 10²³ amu B) 1 gram = 1 amu C) 1 gram = 12 amu D) 1 gram = 1/6.02 × 10²³ amu Awesome! Let's check your answers. 📝✅ Explanation: Avogadro's number, which is approximately 6.02 × 10²³, represents the number of particles in one mole of a substance. A mole is a unit that allows us to count particles on a macroscopic scale. The concept of atomic mass units (amu) was introduced because the masses of single atoms and molecules are too small to be measured in grams. One amu is defined as 1/12th of the mass of a carbon-12 atom. By using conversion factors, we can convert between grams and amu. Now, let's move on to the next section to explore more about molar mass and its applications. 💡🔬 Examples: Suppose we have a sample of oxygen gas (O2). Each oxygen atom has an atomic mass of 16 amu. The molecular mass of oxygen gas (O2) is obtained by adding the atomic masses of two oxygen atoms, which gives us 16 + 16 = 32 amu. Let's consider a mole of oxygen gas (O2). Since the molecular mass of O2 is 32 amu, the mass of one mole of oxygen gas is 32 grams. This relationship holds true for any substance: the molar mass of a substance expressed in grams is numerically equal to its molecular or atomic mass expressed in atomic mass units (amu). End of Lesson Quiz 📝🔍 Now, let's test your knowledge with a few questions: What is the molar mass of carbon dioxide (CO2)? A) 12 grams B) 22 grams C) 44 grams D) 32 grams How many moles of hydrogen atoms are there in one mole of water (H2O)? A) 1 mole B) 2 moles C) 3 moles D) 4 moles The volume of one mole of any gas at STP conditions is _______. A) 22.4 cm³ B) 22.4 dm³ C) 22.4 liters D) 22.4 m³ The molecular formula of glucose (C6H12O6) corresponds to _______. A) 6 moles of carbon atoms, 12 moles of hydrogen atoms, and 6 moles of oxygen atoms B) 1 mole of carbon atoms, 2 moles of hydrogen atoms, and 1 mole of oxygen atoms C) 12 moles of carbon atoms, 6 moles of hydrogen atoms, and 12 moles of oxygen atoms D) 6 moles of carbon atoms, 6 moles of hydrogen atoms, and 6 moles of oxygen atoms Brilliant! You've completed Lesson 13 with flying colors. Avogadro's number and molar mass are crucial concepts in chemistry that help us understand the relationships between particles and their masses. If you have any questions, feel free to ask. Keep up the great work! 🌟😊

< Back Nitrogen and sulfur Previous Next 🔬 Chapter 13: Nitrogen and Sulfur 🔬 Learning Outcomes 🎯: Describe and explain the lack of reactivity of nitrogen gas, the basicity of ammonia, and the formation and structure of the ammonium ion. State the industrial importance of ammonia and nitrogen compounds derived from ammonia. State and explain the environmental consequences of the uncontrolled use of nitrate fertilizers. Describe the natural and man-made occurrences of oxides of nitrogen and their catalytic removal from exhaust gases of internal combustion engines. Describe the formation of sulfur dioxide gas from sulfur-contaminated fossil fuel, its role in the formation of acid rain, and how acid rain affects the environment. Nitrogen and Its Compounds 🌬️: Nitrogen gas is relatively unreactive due to the triple bond between nitrogen atoms in N2 molecules. Ammonia is a basic compound that forms the ammonium ion when it reacts with acids. Ammonia and its derivatives are industrially important, especially in the production of fertilizers. Environmental Impact of Nitrogen Compounds 🌍: The excessive use of nitrate fertilizers can lead to environmental problems such as water pollution and eutrophication. Oxides of nitrogen are pollutants that can be produced naturally or by human activities, such as combustion in engines. They play a role in the formation of acid rain. Sulfur Dioxide and Acid Rain ☔: Sulfur dioxide is produced when sulfur-containing fossil fuels are burned. It is a major contributor to acid rain, which can have harmful effects on the environment, including soil, water, and buildings.

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SABIS GRADE 11 Chapters Topics Term 1 Term 2 Term 3