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Particulate Nature of Matter for IGCSE CIE Questions Part 1 Questions show only in Desktop view See Also Questions Part 2 Questions Part 3 Questions Part 4

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IGCSE CHEMISTRY CAMBRIDGE 1.Particulate Nature of Matter 1.2 Changes in States Of Matter Back to Chapter 1 Menu Notes : Freezing : From liquid to solid Melting : From solid to liquid Boiling : From liquid to gas Condensation : From gas to liquid Sublimation : From Solid to gas directly Explain the Changes of state in terms of the Kinetic Theory To Change Matter from one physical state to another a certain amount of energy has to be absorbed or released. The amount of energy needed depends on the strength of the attraction forces between the particles of the substance. The stronger the forces of attraction between the particles the larger the amount of energy required. Melting Changing from a solid to liquid state by heating . Heat is absorbed to break the bonds between the solid particles and change it into liquid ( heat is changed into kinetic energy which makes the particles vibrate faster so it can break the bonds between them and change into liquid state). Happens at the Melting point. Boiling Changing from a liquid to gas state by heating . Occurs below the surface of the liquid. Requires heat to be absorbed to break the bonds between the liquid particles and change it into gas ( heat is changed into kinetic energy which makes the particles move faster so it can break the bonds between them and change into gas state ). Happens at the Boiling point. Evaporation Changing from a liquid to gas state. occurs only at the surface of the liquid. Requires heat to be absorbed to break the bonds between the liquid particles and change it into gas ( heat is changed into kinetic energy which makes the particles move faster so it can break the bonds between them). Freezing Changing from a liquid to solid state by decreasing temperature . Requires heat to be released (lost from system) to make new bonds between the liquid particles and change it into solid ( losing heat decreases the kinetic energy of the particles which makes the particles move slower and stick together) Happens at the Freezing point. Note : Freezing point and Melting point has the same value it depends only in the direction of change in state From Solid to liquid (Melting point) From liquid to solid (Freezing point) Condensation Changing from a gas to liquid state. Requires heat to be released (lost from system) to make new bonds between the gas particles and change it into liquid ( losing heat decreases the kinetic energy of the particles which makes the particles move slower) Note that condensation is the opposite of evaporation Sublimation Changing from a solid to gas directly. It happens in certain types of substances , and is related to the nature of the substance not to the method of heating. example : Solid iodine , solid carbon dioxide , solid ammonium chloride. The reverse reaction also happens and is also called sometimes called deposition or de-sublimation. Sublimation occurs at a specific temperature which is unique for a pure substance. Describe qualitatively the pressure and the temperature of a gas in terms of motion of its particles As mentioned earlier the particles of gas moves rapidly and randomly in all directions this causes the particles of gas to collide with each other and with the walls of its container. this causes the particles to exert pressure. The Higher the temperature the more rapid the particles will hit each other and collide with the walls of the container exerting higher pressure. When the gas is compressed to a smaller volume , the particles also hit each other more frequently and hit the walls more frequently increasing the gas pressure. List of Topics Download as PDF

Catalyst: Definition SABIS Grade 10 SABIS a substance that increases the reaction rate without itself being used up. It speeds up both forward and reverse reactions. A catalyst takes part in the reaction, but is regenerated, so it is not used up.A catalyst acts: by providing a new path of lower activation energy for reactants to follow, so the catalyzed and uncatalyzed pathways proceed simultaneously.

Cambridge IGCSE Chemistry 0620 The Ultimate Summary with MCQs OCT/NOV 2023 Topic 1 . PDF States of Matter Topic 2 . PDF Atoms Elements and Compounds Part 1 Topic 3. PDF Atoms Elements and Compounds Part 2 Topic 4. PDF Topic 5. PDF Electrochemistry Topic 6. PDF Thermochemistry Topic 7. PDF Chemical react ions Part 1 Topic 7. PDF Chemical reactions Part 2 Topic 7.Part3 Topic 8. PDF Acids Bases and Salts Topic 9. PDF Topic 10. PDF Topic 11. PDF Topic 12. PDF More Revision For IGCSE Exams Organic Chemistry Download Full Syllabus (Cambridge Website)

Particulate Nature of Matter for IGCSE CIE Questions Part 4 Questions chapter 1 IGCSE 1 Questions chapter 1 IGCSE 2 Questions chapter 1 IGCSE 3 Questions chapter 1 IGCSE 1 1/3 Click on the pages to open them Opens only in desktop view not in mobile view See Also Questions Part 1 Questions Part 2 Questions Part 3

Know that in for endothermic reactions H products > H reactants, ∆ H> 0 and reaction absorbs energy Grade 10 SABIS In chemical reactions, an endothermic reaction is one that absorbs energy from the surroundings. It is characterized by the fact that the enthalpy (H) of the products is greater than the enthalpy of the reactants. This change in enthalpy (∆H) is positive, indicating that energy is absorbed during the reaction. To understand endothermic reactions, let's consider an everyday example: the process of cooking pasta. When you boil water and add pasta to it, the reaction between the pasta and the hot water is endothermic. The energy from the heat source is absorbed by the pasta, causing it to cook and increase in temperature. In an endothermic reaction, the potential energy of the products is higher than that of the reactants. This means that the reactants have a lower energy level compared to the products. As the reaction progresses, energy is absorbed from the surroundings, leading to an increase in potential energy. On a potential energy diagram for an endothermic reaction, the reactants are represented at a lower energy level compared to the products. The curve starts at a lower point (representing the energy of the reactants) and gradually increases (representing the increase in potential energy) as the reaction proceeds towards the products. The difference in potential energy between the reactants and products is the amount of energy absorbed from the surroundings. The positive value of ∆H indicates that the reaction absorbs energy. This energy can be in the form of heat, light, or any other form of energy. In the case of the cooking pasta example, the absorbed energy is in the form of heat from the boiling water. Endothermic reactions are essential in various processes. For instance, in photosynthesis, plants absorb energy from sunlight to convert carbon dioxide and water into glucose and oxygen. This process requires energy input to drive the reaction. Another example is the process of evaporation. When a liquid evaporates, it absorbs energy from the surroundings, causing a cooling effect. This is because the liquid particles need to gain energy to break the intermolecular forces and transform into a gas state. Endothermic reactions are also prevalent in chemical reactions used for cooling, such as instant cold packs or ice packs. These packs contain chemicals that undergo an endothermic reaction when activated, absorbing heat from the surroundings and providing a cooling sensation. In summary, endothermic reactions are characterized by the absorption of energy from the surroundings. The enthalpy of the products is greater than that of the reactants, resulting in a positive change in enthalpy (∆H). On a potential energy diagram, the potential energy increases from the reactants to the products, indicating the energy absorbed during the reaction. Understanding endothermic reactions helps us comprehend processes that require energy input and have a cooling effect, such as cooking, photosynthesis, evaporation, and cooling packs.

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Particulate Nature of Matter for IGCSE CIE Questions Part 2 See Also Questions Part 1 Questions Part 3 Questions Part 4

Trending Now The 60-Day IGCSE Organic Chemistry Challenge Free Preview IGCSE 0620 Grade 12 SABIS Grade 11 SABIS Most Downloaded Chemistry 0620 Final Revision for IGCSE 2023 Week 1 $0.00 (Was 5.00 $) DOWNLOAD

Grade 12 SABIS Concise resources for the SABIS Chemistry: Grade 12 course. Chapter 1 Concise resources for the SABIS Chemistry: Grade 12 course. Chapter 2 Concise resources for the SABIS Chemistry: Grade 12 course. Chapter 3 Concise resources for the SABIS Chemistry: Grade 12 course. Chapter 4 Concise resources for the SABIS Chemistry: Grade 12 course. Chapter 5 Concise resources for the SABIS Chemistry: Grade 12 course. Chapter 6 Concise resources for the SABIS Chemistry: Grade 12 course.

Boyle's Law The principle that states the volume of a given amount of gas is inversely proportional to its pressure at a constant temperature.