Chapter 4 matter and substance
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This document discusses different types of phase changes that can occur in matter: 1) Melting occurs when a solid absorbs heat at its melting point, gaining kinetic energy until its structure can no longer hold its fixed form and it becomes a liquid. 2) Freezing is the reverse of melting, as a liquid cools and loses kinetic energy, decreasing the distance between molecules until they bond to form a solid. 3) Boiling occurs when a liquid directly changes to a gas upon absorbing enough heat to overcome molecular attractions, such as with dry ice subliming. 4) Condensation is the reverse of boiling as a gas cools and loses kinetic energy, decreasing distance between molecules until they bond to
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Solution
generally the ,
Solids - vibrational (and rotational); moving very slowly.
Liquids - vibrational, rotational, and translational; moving quickly.
Gases - vibrational, rotational, and translational; moving very quickly.
Explanation:
Particles are always moving. No matter what. There is a certain point where they move so slowly it is considered minuscule, but they are in fact moving.
Thus, in solids, liquids, and gases, you can expect particles to move in a certain trend. That trend is average kinetic energy of the particles and the forces holding them together (attraction).
Solids
When you have little to no heat, the particles are moving very slowly, so slowly that they atomic attractions result in bonds that are difficult to break without adding energy. At this stage, this is known as a solid.
In a solid, the particles are vibrating. Only some solids have the ability to rotate. They cannot translate regardless.
Liquids
When you add energy (heat) to a solid, you \"excite\" the particles so much that they break their bond; their attraction is too weak to hold them together - yet strong enough to keep a form
As a result, you get a liquid.
In a liquid, the particles are not only vibrating (their bonds are not present but they still vibrate), but they are also rotating and translating. The particles are moving much faster than in a solid.
Gases
When you add even more energy to the substance, you increase the kinetic energy of those particles so much, that they lose their state form, becoming a gas.
In a gas, particles have vibrational, rotational, and translational motion, allowing them to \"bounce\" off of one another. Particles in a gas state move much faster than a liquid.
Light is a form of energy that can be released by an atom. It is made up of many small particle-like packets that have energy and momentum but no mass. These particles, called light photons, are the most basic units of light.
When the atom gains or loses energy, the change is expressed by the movement of electrons. When something passes energy on to an atom -- heat , for example -- an electron may be temporarily boosted to a higher orbital (farther away from the nucleus). The electron only holds this position for a tiny fraction of a second; almost immediately, it is drawn back toward the nucleus, to its original orbital. As it returns to its original orbital, the electron releases the extra energy in the form of a photon, in some cases a light photon
.
Thermal 3.1
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.
2.1 Concept of Matter
The document discusses the basic concept of matter according to the kinetic theory. It states that:
1) Matter can exist in three physical states - solid, liquid, and gas - depending on the arrangement and movement of its particles.
2) In solids, particles are closely packed and arranged orderly, while in liquids they are farther apart but not in an orderly arrangement. In gases, particles are very far apart and move freely at high speeds.
3) Changes in temperature can cause changes in a substance's state as it absorbs or releases heat, altering the kinetic energy and motion of its particles. For example, melting occurs when a solid absorbs enough heat energy to allow its particles to vibrate vigorously
Notes for science
The document provides information about the particle models of gases, liquids, and solids. It explains that gases have no fixed shape or volume, while liquids have a fixed volume but not shape, and solids have both a fixed volume and shape. It also discusses the states of matter and how heating and cooling can cause phase changes between solid, liquid, and gas. Additionally, it covers topics like light, heat, temperature, and magnets.
Notes for science
The document provides information about the particle models of gases, liquids, and solids. It explains that gases have no fixed shape or volume, while liquids have a fixed volume but not shape, and solids have both a fixed volume and shape. It also discusses the states of matter and how heating and cooling can cause phase changes between solid, liquid, and gas. Additionally, it covers topics like evaporation, boiling, reflection of light, heat transfer, and properties of magnets.
Notes for science
The document provides information about the particle models of gases, liquids, and solids. It explains that gases have no fixed shape or volume, while liquids have a fixed volume but not shape. Solids have both a fixed shape and volume. It also discusses phase changes like evaporation, boiling, melting, and freezing in terms of particle motion and interactions. Additional topics covered include light, heat, temperature, and magnets.
Notes for science
The document provides information about the particle models of gases, liquids, and solids. It explains that gases have no fixed shape or volume, while liquids have a fixed volume but not shape, and solids have both a fixed volume and shape. It also discusses phase changes like evaporation, boiling, melting, and freezing in terms of particle motion and interactions. Additional topics covered include light, heat, temperature, and magnets.
Unit c heat & temperature notes(changes between states)
This document discusses the effect of heat on the states of matter and phase changes. It explains that adding heat provides kinetic energy to particles, causing them to move faster and take up more space. This allows matter to change states from solid to liquid to gas through processes like melting, boiling, condensation, freezing, sublimation, and deposition which are described.
LSS Kinetic Particle Theory
Kinetic Particle Theory describes the three states of matter and changes between them. It states that all matter is made of tiny particles in constant random motion. The states - solid, liquid, gas - differ in how the particles are arranged and how they move. In solids, particles are closely packed in an orderly arrangement and can only vibrate. In liquids, particles are closely packed randomly and can move past each other. Gases have particles far apart, moving freely in any direction. Changes of state occur when particles gain or lose kinetic energy from heat, allowing them to overcome or increase attractive forces between particles.
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
22 the states of matter
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.
Physical properties of matter
This document discusses various physical properties of matter including the three main phases of matter, phase changes, heat energy, melting and boiling points, volume and mass, density, thermal expansion, solubility, and heat and electrical conductivity. Key points covered include definitions of solids, liquids and gases, how heat energy causes phase changes, temperature relationships, defining melting and boiling points, the relationship between volume and mass, how density is calculated, examples of thermal expansion and solubility, and how conductivity transfers heat and electrical energy.
States of matter kashish
The document discusses kinetic molecular theory and how it can be used to explain the properties of solids, liquids, and gases. It states that all matter is made up of extremely small particles that are constantly in motion. In solids, the particles are close together and do not move far from their fixed positions. In liquids, the particles can move around each other but remain in contact. In gases, the particles move very fast and are far apart from each other. A change in temperature can cause a substance to change states from a solid to a liquid to a gas as the particles gain or lose kinetic energy.
Thermodynamics
Thermodynamics is the study of heat and thermal energy. The document discusses several key concepts in thermodynamics including:
- Kinetic molecular theory explains that matter is made up of atoms and molecules in constant motion, with higher temperatures resulting from faster atomic motions.
- Internal energy is the sum of the kinetic and potential energy of all particles in a system due to their random motions. Temperature is proportional to average kinetic energy.
- Heat is the transfer of internal energy between objects due to a temperature difference, while internal energy is the total thermal energy of a single object.
- Temperature scales like Celsius, Fahrenheit and Kelvin relate to molecular kinetic energy and absolute zero, the coldest possible temperature
Matter & its composition
This document provides an overview of matter and its properties according to the ICSE curriculum for upper primary classes. It defines matter as anything that occupies space, has mass and volume, and can be sensed. All matter is composed of molecules, which are made up of atoms. Matter can exist in three states - solid, liquid, and gas - depending on the strength of intermolecular forces and the distance between molecules. Changes in state, such as melting, boiling, and sublimation, occur when matter gains or loses heat. Heating matter can also cause chemical changes in addition to physical changes like expansion and changes in state.
Heat energy
This document discusses heat transfer and thermal energy. It defines heat as a form of energy that causes particles to move and take up more space. Heat is transferred between objects by conduction, convection, or radiation. Conduction involves direct contact between particles, convection involves the movement of fluids like gases and liquids, and radiation transfers heat through electromagnetic waves without a medium. The document differentiates between heat and temperature, explaining that temperature measures how hot an object is while heat refers to the total thermal energy. It also covers how heating and cooling affect the expansion and contraction of materials.
Similar to Chapter 4 matter and substance (20)
Redesign- Make a prediction relating heat to the movement of molecules.docx
Redesign- Make a prediction relating heat to the movement of molecules.docx
Unit c heat & temperature notes(changes between states)
Unit c heat & temperature notes(changes between states)
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Chapter 4 matter and substance
- 1. A change in state is always accompanied by either a loss or gain in HEAT
- 3. Occurs at melting point of the solid; ice is at 0ºC The heat absorbed increase the kinetic energy causes them to vibrate vigorously The attractive forces between them can no longer hold them in their fixed structure as in solid
- 4. Reverse of melting Happens at freezing point at 0ºC The liquid is cooled and heat is released Kinetic energy decreased, molecule’s motion slowed down The distance between molecules decreased Attractive forces increased and caused molecules to be bonded forming the solid
- 5. Reverse of boiling When vapour(gas) is cooled, heat is removed This reduced kinetic energy and speed of molecules The distance between them is reduced and attraction between molecules increase Liquid formed
- 6. Occurs when a solid changes directly into its gaseous state Happen at fixed temperature Heat is absorbed by the solid is converted to kinetic energy and sufficient to overcome the forces of attraction and take them far apart into gaseous state Examples: iodine, dry ice, ammonium chloride crystal
- 7. Occurs at 100ºC Liquid is heated, the heat is absorbed causes the kinetic energy increased When *KE gained is sufficient to overcome the forces of attraction, the molecule escape the liquid surface and become molecule of gas
- 9. P to Q - The substance is in a solid state.The particles absorb heat energy and vibrate faster.The temperature of the substance increases. Q to R - At Q(melting starts), the particles have enough energy to break away from one another. From Q to R the substance is MELTING, and the temperature DOES NOT RISE.The energy absorbed is used to overcome the force of attraction between the particles.
- 10. R to S - At R, the substance has completely melted. The particles are free to move.The particles move faster as more energy is absorbed and the temperature rises
- 11. K to L - The substance is in a liquid state. As it cools, heat energy is RELEASED.The particles LOSE kinetic energy and move close to one another L to M - At L, the substance begins to SOLIDIFY.The particles begin to arrange themselves in an orderly manner. At M, the substance has turned into a solid state M to N - The substance is now in a SOLID state. It loses heat and its temperature gradually cools to the room temperature. At N, the substance is at *RT
- 13. Made up of a central nucleus: protons+neutrons The electrons are continuously moving around in permissible orbits
- 14. Protons and neutrons in a nucleus are collectively called nucleons Ex: irons have 26 protons and 30 protons, the sum will be 56 nucleons Total number of nucleons is nucleon number (mass number,A) is equal to the sum of the no of neutrons(neutron number,N) and the number of protons, the proton number (also called atomic number, Z) For a neutral atom,total no of electron is equal to the proton no.
- 16. The proton no of a nucleus determines what element it is However, the no of neutrons can varies Isotopes are atoms of the same element that have the same proton number but differing nucleon number