States of matter
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This document discusses the three phases of matter - solid, liquid, and gas - and how particles behave in each phase according to the kinetic molecular theory. It explains that all matter is made up of particles that are in constant motion, and the amount of energy they possess determines whether the substance is a solid, liquid or gas. It also defines melting point, freezing point and boiling point as the temperatures at which substances change phase between solid, liquid and gas.
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This document discusses the three common states of matter - solids, liquids, and gases. It explains their key properties including definite mass and varying volume and shape. The document then introduces the particle theory of matter, which states that all matter is made up of tiny particles that are in constant motion. It describes how the motion and interaction of these particles determines whether a substance is a solid, liquid or gas, and how physical changes like melting, boiling and condensation occur as particles gain or lose energy.
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The document discusses the three states of matter - solid, liquid, and gas. It introduces kinetic theory, which explains that matter is made up of particles that are constantly in motion. The way these particles are arranged determines the three states of matter and their properties. Solids have particles that are close together and do not move much. Liquids have particles close together but able to move and change position. Gases have particles far apart that move freely throughout their container.
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States of matter
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This document discusses concepts of thermal physics including the four states of matter, microscopic and macroscopic properties, phases of matter, and changes of state. It explains that matter can exist as solids, liquids, gases, or plasmas depending on temperature and pressure. Microscopically, the kinetic energy and potential energy of particles determines the state. Heat is the transfer of thermal energy between objects due to temperature differences. Specific heat capacity refers to the amount of energy required to change the temperature of a substance and can vary between materials. Methods for determining specific heat capacity include direct calorimetry and indirect calculations.
9th matter in_our_sorounding__notes
This document discusses the five states of matter: solid, liquid, gas, plasma, and Bose-Einstein condensate. It describes the characteristics of each state and how matter can change between states through processes like melting, vaporization, boiling, and sublimation which involve the addition or removal of heat. A key point is that all matter is made of particles that are in constant motion, and the amount and type of motion determines which state the matter is in.
9th matter in_our_sorounding__notes (1)
This document discusses the five states of matter: solid, liquid, gas, plasma, and Bose-Einstein condensate. It describes the key properties of each state. Solids have a definite shape and volume, while liquids have a definite volume but take the shape of their container. Gases have no definite shape or volume. Plasma is a superheated gaseous state found at extremely high temperatures. Bose-Einstein condensate is a supercooled state where atoms lose their identity and behave as a single "super atom". Matter can change between solid, liquid, and gas states through heating and cooling processes like melting, freezing, vaporization, and condensation.
9th matter in_our_sorounding__notes
This document discusses the five states of matter: solid, liquid, gas, plasma, and Bose-Einstein condensate. It describes the key properties of each state. Solids have a definite shape and volume, while liquids have a definite volume but take the shape of their container. Gases have no definite shape or volume. Plasma is a superheated gaseous state found at extremely high temperatures. Bose-Einstein condensate is a supercooled state where atoms lose their identity and behave as a single "super atom". Matter can change between solid, liquid, and gas states through heating and cooling processes like melting, freezing, vaporization, and condensation.
Session1
This document discusses the kinetic particle theory which is used to explain the three states of matter - solids, liquids, and gases. It explains that in solids, particles are locked in place, in liquids they can move past each other but the substance retains its volume and shape, and in gases particles are in constant random motion and the substance will expand to fill its container. It also discusses how heating can cause pressure changes in gases by increasing particle kinetic energy, and how energy must be added or removed during state changes through the absorption or release of latent heat.
2.1 form 3 simple kinetic molecular model of matter
This document describes the kinetic molecular model of matter. It explains that matter exists in three states - solid, liquid, and gas - depending on how tightly or loosely bound the particles are and how much they move. Solids have a fixed shape and volume as particles vibrate in place. Liquids have no fixed shape but a fixed volume as particles move past each other. Gases have no fixed shape or volume as particles move freely in all directions at high speeds with little attraction. Higher temperatures means particles have more kinetic energy and evaporation occurs when the most energetic particles overcome attractive forces and escape as a gas.
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Chapter 10.1 The Kinetic-Molecular Theory
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Chapter 1 kinetic particle theory (1)
1. The kinetic particle theory describes the three states of matter (solid, liquid, gas) based on how closely particles are packed and how they move. In solids, particles vibrate in fixed positions; in liquids, they slide over each other; and in gases, they are far apart and move rapidly.
2. Changes of state like melting, freezing, boiling, and condensation can be explained by how particle kinetic energy changes with temperature. During melting and boiling, particle motion overcomes attractive forces, while freezing and condensation occur as particles slow down.
3. The temperatures at which changes of state occur (melting point, boiling point) remain constant as long as the change of state is happening
Chapter 1 kinetic particle theory (1)
1. The kinetic particle theory describes the three states of matter (solid, liquid, gas) based on how closely particles are packed and how they move. In solids, particles vibrate in fixed positions; in liquids, they slide over each other; and in gases, they are far apart and move rapidly.
2. Changes of state like melting, freezing, boiling, and condensation occur when particles gain or lose enough kinetic energy to overcome the forces between them. Melting and boiling happen when particles break away from fixed positions and spread out. Freezing and condensation occur when particles slow down and settle into fixed positions.
3. Evaporation and sublimation are also changes of state: evap
The Particle Nature of Matter
All matter is particulate in nature. This simply means that matter is made up of tiny bit bits material known as particle.
Matter & its composition 2
This document discusses key concepts in chemistry including thermal energy, the kinetic molecular theory of matter, and states of matter. It begins by defining thermal energy as the energy of a body due to the motion of its particles, which is directly proportional to temperature. It then explains kinetic and potential energy. The document goes on to discuss how the three states of matter arise from a competition between intermolecular forces and thermal energy. It also summarizes the kinetic molecular theory and how it applies to solids, liquids, and gases. Finally, it briefly defines and compares the processes of diffusion and effusion.
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The document discusses the kinetic molecular theory and how it can be used to explain the properties of liquids and solids. It defines the kinetic molecular theory and its key postulates, including that matter is made of particles in constant motion, kinetic energy increases with temperature, and the amount of space between particles depends on the state of matter. It then describes the properties of solids, liquids, and gases based on this theory, noting that solids have the greatest intermolecular forces and particles vibrate in fixed positions, while liquids have less forces but particles can slide past one another.
Matter
This document outlines 10 student learning outcomes (SLOs) for a unit on Matter & Atoms for Year 9 students. The SLOs cover topics including the particle nature of matter, the three states of matter, density, diffusion, expansion and contraction, and conduction and convection. It also includes an SLO on describing the current atomic model and relating historical atomic models. Accompanying the SLOs are sections providing more details on these topics, including explanations, diagrams, examples and success criteria for students.
ICSE Class VIII Chemistry Matter Around Us - TopperLearning
Anything which occupies space or volume, has mass and can be perceived by our senses is called matter.
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2.1 form 3 simple kinetic molecular model of matter
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States of matter
- 1. 3. States of matter and the kinetic molecular theory Chemistry: Matter and materials Grade 10
- 2. Three phases of matter Solid e.g. ice Liquid e.g. water Gas e.g. steam
- 3. All matter is made up of particles. To see this we can look at diffusion. Diffusion is the movement of particles from a high concentration to a low concentration. Brownian motion is the diffusion of many particles.
- 5. Freezing point is the temperature at which a liquid changes its phase to become a solid.
- 6. Boiling point is the temperature at which a liquid changes phase to become a gas.
- 7. Kinetic Molecular Theory (KMT) The kinetic theory of matter attempts to explain the behaviour of matter in different phases. The kinetic theory of matter says that all matter is composed of particles which have a certain amount of energy which allows them to move at different speeds depending on the temperature (energy). There are spaces between the particles and also attractive forces between particles when they come close together. Energy Space between particles Strength of intermolecular forces
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