Section Matter And Thermal Energy 1 - Weebly
Section1Matter and Thermal EnergyStates of Matter Can you identifythe states ofmatter present inthe photo shown?
Section1Matter and Thermal EnergyKinetic Theory The kinetic theory is an explanation of how particlesin matter behave.
Section1Matter and Thermal EnergyKinetic Theory The three assumptions of the kinetic theory are asfollows: All matter is composed of small particles (atoms,molecules, and ions). These particles are in constant, random motion. These particles are colliding with each other andthe walls of their container.
Section1Matter and Thermal EnergyKinetic Theory Particles lose some energy during collisions with otherparticles. But the amount of energy lost is very small and can beneglected in most cases.
Section1Matter and Thermal EnergyThermal Energy Atoms in solids are held tightly in place by theattraction between the particles. This attraction between theparticles gives solids adefinite shape and volume.However, the thermal energyin the particles causes themto vibrate in place.
Section1Matter and Thermal EnergyThermal Energy Thermal energy is the total energy of a material’sparticles, including kinetic—vibrations and movementwithin and between the particles—and potential—resulting from forces that act within or betweenparticles.
Section1Matter and Thermal EnergyAverage Kinetic Energy In science, temperature means the average kineticenergy of particles in the substance, or how fast theparticles are moving. On average, molecules of frozen water at 0 C willmove slower than molecules of water at 100 C.
Section1Matter and Thermal EnergyAverage Kinetic Energy Water molecules at 0 C have lower average kineticenergy than the molecules at 100 C. Molecules have kinetic energy at all temperatures,including absolute zero.
Section1Matter and Thermal EnergySolid State The particles of a solid are closely packed together. Most solid materialshave a specific type ofgeometric arrangementin which they form whencooled.
Section1Matter and Thermal EnergySolid State The type of geometric arrangement formed by asolid is important. Chemical and physicalproperties of solidsoften can be attributedto the type of geometricarrangement that thesolid forms.
Section1Matter and Thermal EnergyLiquid State What happens to a solid when thermal energy or heatis added to it? The particles on the surface of the solid vibrate faster. These particles collide with and transfer energy toother particles. Soon the particles have enough kinetic energy toovercome the attractive forces.
Section1Matter and Thermal EnergyLiquid State The particles gain enough kinetic energy to slip out oftheir ordered arrangement and the solid melts. This is known as the melting point, or the temperatureat which a solid begins to liquefy. Energy is required for the particles to slip out of theordered arrangement.
Section1Matter and Thermal EnergyLiquid State The amount of energy required to change a substancefrom the solid phase to the liquid phase at its meltingpoint is known as the heat of fusion. Particles in a liquid have more kinetic energy thanparticles in a solid.
Section1Matter and Thermal EnergyLiquid Flow This extra kinetic energy allows particles to partiallyovercome the attractions to other particles. The particles canslide past eachother, allowingliquids to flow andtake the shape oftheir container.
Section1Matter and Thermal EnergyLiquid Flow However, the particles in a liquid have not completelyovercome the attractive forces between them This causes the particles tocling together, giving liquidsa definite volume.
Section1Matter and Thermal EnergyGas State Gas particles have enough kinetic energy to overcomethe attractions between them. Gases do not have afixed volume or shape. Therefore, they canspread far apart orcontract to fill thecontainer that they are in.
Section1Matter and Thermal EnergyGas State How does a liquid become a gas? The particles in a liquid are constantly moving.
Section1Matter and Thermal EnergyGas State Some particles are moving faster and have morekinetic energy than others. The particles that aremoving fast enough can escape the attractive forces ofother particles and enter the gas state.
Section1Matter and Thermal EnergyGas State This process is called vaporization. Vaporization can occur in two ways—evaporation andboiling. Evaporation is vaporization that occurs at the surfaceof a liquid and can occur at temperatures below theliquid’s boiling point.
Section1Matter and Thermal EnergyGas State To evaporate, particles must have enough kineticenergy to escape the attractive forces of the liquid.They must be at the liquid’s surface and traveling awayfrom the liquid.
Section1Matter and Thermal EnergyGas State Unlike evaporation, boiling occurs throughout a liquid ata specific temperature depending on the pressure onthe surface of the liquid. The boiling point of a liquid isthe temperature at which thepressure of the vapor in theliquid is equal to the externalpressure acting on the surfaceof the liquid.Click image to view movie
Section1Matter and Thermal EnergyGas State Heat of vaporization is the amount of energy requiredfor the liquid at its boiling point to become a gas.
Section1Matter and Thermal EnergyGases Fill Their Container What happens to the attractive forces between theparticles in a gas? The gas particles are moving so quickly and are sofar apart that they have overcome the attractiveforces between them. Diffusion is the spreading of particles throughout agiven volume until they are uniformly distributed.
Section1Matter and Thermal EnergyHeating Curve of a Liquid This type of graph is called a heating curve because itshows the temperature change of water as thermalenergy, or heat, is added. Notice the two areas onthe graph where thetemperature does notchange. At 0 C, ice ismelting.
Section1Matter and Thermal EnergyHeating Curve of a Liquid The temperature remains constant during melting. After the attractive forcesare overcome, particlesmove more freely andtheir average kineticenergy, or temperature,increases.
Section1Matter and Thermal EnergyHeating Curve of a Liquid At 100 C, water is boiling or vaporizing and thetemperature remains constant again.
Section1Matter and Thermal EnergyPlasma State Scientists estimate that much of the matter in theuniverse is plasma. Plasma is matter consisting of positively and negativelycharged particles. Although this matter containspositive and negative particles, itsoverall charge is neutral becauseequal numbers of both charges arepresent.Click image to view movie
Section1Matter and Thermal EnergyPlasma State The forces produced from high-energy collisions areso great that electrons from the atom are strippedoff. This state of matter is called plasma.
Section1Matter and Thermal EnergyPlasma State All of the observed starsincluding the Sun consistof plasma. Plasma alsois found in lightning bolts,neon and fluorescenttubes, and auroras.
Section1Matter and Thermal EnergyExpansion of Matter Particles move faster and separate as the temperaturerises. This separation of particles results in anexpansion of the entire object, known as thermalexpansion. Thermal expansion is an increase in the size of asubstance when the temperature is increased.
Section1Matter and Thermal EnergyExpansion of Matter The kinetic theory can be used to explain the contractionin objects, too. When the temperature of an object is lowered, particlesslow down. The attraction between the particles increases and theparticles move closer together. The movements of theparticles closer together result in an overall shrinking ofthe object, known as contraction.
Section1Matter and Thermal EnergyExpansion in Liquids A common example ofexpansion in liquids occursin thermometers. The addition of energycauses the particles of theliquid in the thermometer tomove faster.
Section1Matter and Thermal EnergyExpansion in Liquids The particles in the liquidin the narrow thermometertube start to move fartherapart as their motionincreases.
Section1Matter and Thermal EnergyExpansion in Liquids The liquid has to expandonly slightly to show a largechange on the temperaturescale.
Section1Matter and Thermal EnergyExpansion in Gases Hot-air balloons are able to rise due to thermalexpansion of air. The air in the balloon is heated, causing the distancebetween the particles in the air to increase.
Section1Matter and Thermal EnergyExpansion in Gases As the hot-air balloonexpands, the numberof particles per cubiccentimeter decreases.
Section1Matter and Thermal EnergyExpansion in Gases This expansion resultsin a decreased densityof the hot air. Thedensity of the air in thehot-air balloon is lowerthan the density of thecooler air outside, whichallows the balloon willrise.
Section1Matter and Thermal EnergyThe Strange Behavior of Water Water molecules are unusual in that they have highlypositive and highly negative areas. These charged regionsaffect the behavior ofwater. As the temperature ofwater drops, theparticles move closertogether.
Section1Matter and Thermal EnergyThe Strange Behavior of Water The unlike charges will be attracted to each other andline up so that only positive and negative zones arenear each other. Because the water molecules orient themselvesaccording to charge, empty spaces occur in thestructure. These empty spaces are larger in ice than in liquidwater, so water expands when going from a liquid to asolid state.
Section1Matter and Thermal EnergySolid or a Liquid? Other substances also have unusual behavior whenchanging states. Amorphous solids and liquid crystals are two classes ofmaterials that do not react as you would expect whenthey are changing states.
Section1Matter and Thermal EnergyAmorphous Solids Not all solids have a definite temperature at whichthey change from solid to liquid. Some solids merely soften and gradually turn into aliquid over a temperature range. These solids lack the highly ordered structure foundin crystals They are known as amorphous solids from the Greekword for “without form.”
Section1Matter and Thermal EnergyAmorphous Solids The particles that make up amorphous solids aretypically long, chainlike structures that can be jumbledand twisted instead of being neatly stacked intogeometric arrangements. Liquids do not have an orderly arrangement ofparticles. Some amorphous solids form when liquid matterchanges to solid matter too quickly for an orderlystructure to form.
Section1Matter and Thermal EnergyAmorphous Solids One example of this isobsidian—a volcanic glass.Obsidian forms when lavacools quickly, such as whenit spills into water.
Section1Matter and Thermal EnergyLiquid Crystals Liquid crystals are another group of materials that donot change states in the usual manner. Liquid crystals start to flow during the melting phasesimilar to a liquid, but they do not lose their orderedarrangement completely, as most substances do.
Section1Matter and Thermal EnergyLiquid Crystals Liquid crystals are placed in classes depending uponthe type of order they maintain when they liquefy. They are highly responsive to temperature changesand electric fields.
Section2Properties of FluidsHow do ships float? Despite their weight, ships are able to float. This is because a greater force pushing up on the shipopposes the weight—or force—of the ship pushingdown.
Section2Properties of FluidsHow do ships float? This supporting force is called the buoyant force. Buoyancy is the ability of a fluid—a liquid or a gas—toexert an upward force on an object immersed in it. If the buoyant force is less than the object’s weight, theobject will sink.
Section2Properties of FluidsArchimedes’ Principle In the third century B.C., a Greek mathematician namedArchimedes made a discovery about buoyancy. Archimedes found that the buoyant force on an object isequal to the weight of the fluid displaced by the object.
Properties of FluidsSection2Density An object will float if its density is less than the densityof the fluid it is placed in.
Properties of FluidsSection2Density Suppose you form a steel block into the shape of a hullfilled with air. The steel has the same mass but takesup a larger volume. The overall density of the steelboat and air is less than the density of water. The boatwill now float.
Section2Properties of FluidsPascal’s Principle Pressure is force exerted per unit area. Blaise Pascal (1692-1662), a French scientist,discovered a useful property of fluids. According to Pascal’s principle, pressure applied to afluid is transmitted throughout the fluid.
Section2Properties of FluidsApplying the Principle Hydraulic machines are machines that move heavyloads in accordance with Pascal’s principle. Maybe you’ve seen a car raised using a hydraulic lift inan auto repair shop.
Section2Properties of FluidsApplying the Principle A pipe that is filled with fluidconnects small and largecylinders.
Section2Properties of FluidsApplying the Principle Pressure applied to the small cylinder is transferredthrough the fluid to the large cylinder. Because pressure remains constant throughout thefluid, according to Pascal’s principle, more force isavailable to lift a heavy load by increasing the surfacearea.
Section2Properties of FluidsBernoulli’s Principle According to Bernoulli’s principle, as the velocity of afluid increases, the pressure exerted by the fluiddecreases. One way to demonstrate Bernoulli’s principle is to blowacross the top surface of a sheet of paper. The paper will rise.
Section2Properties of FluidsBernoulli’s Principle The velocity of the air you blew over the top surface ofthe paper is greater than that of the quiet air below it. As a result, the air pressure pushing down on the top ofthe paper is lower than the air pressure pushing up onthe paper. The net force below the paper pushes the paper upward.
Section2Properties of FluidsBernoulli’s Principle Another application of Bernoulli’s principle is the hoseend sprayer.
Section2Properties of FluidsBernoulli’s Principle This allows the water in the hose to flow at a high rateof speed, creating a low pressure area above thestrawlike tube. The concentrated chemical solution is sucked upthrough the straw and into the stream of water. The concentrated solution is mixed with water,reducing the concentration to the appropriate leveland creating a spray that is easy to apply.
Section2Properties of FluidsFluid Flow Another property exhibited by fluid is its tendency toflow. The resistance to flow by a fluid is calledviscosity. When a container of liquid is tilted to allow flow to begin,the flowing particles will transfer energy to the particlesthat are stationary.
Section2Properties of FluidsFluid Flow In effect, the flowing particles are pulling the otherparticles, causing them to flow, too. If the flowing particles do not effectively pull the otherparticles into motion, then the liquid has a highviscosity, or a high resistance to flow. If the flowing particles pull the other particles intomotion easily, then the liquid has low viscosity, or a lowresistance to flow.
Behavior of GasesSection3Pressure Pressure is the amount of force exerted per unit ofarea, or P F/A. A balloon and a bicycle tire areconsidered to be containers. They remain inflated because ofcollisions the air particles havewith the walls of their container.
Behavior of GasesSection3Pressure This collection of forces, caused by the collisions ofthe particles, pushes the walls of the containeroutward. If more air is pumped into theballoon, the number of airparticles is increased. This causes more collisions withthe walls of the container, whichcauses it to expand.
Behavior of GasesSection3Pressure Pressure is measured in a unit called Pascal (Pa),the SI unit of pressure. Because pressure is the amount of force divided byarea, one pascal of pressure is one Newton per squaremeter or 1 N/m2.
Behavior of GasesSection3Pressure At sea level, atmospheric pressure is 101.3 kPa. At Earth’s surface, the atmosphere exerts a force ofabout 101,300 N on every square meter—about theweight of a large truck.
Section3Behavior of GasesBoyle’s Law What happens to the gas pressure if you decrease thesize of the container? If you squeeze gas into a smaller space, its particleswill strike the walls more often giving an increasedpressure. The opposite is true, too.
Section3Behavior of GasesBoyle’s Law Robert Boyle (1627-1691), a British scientist, describedthis property of gases. According to Boyle’s law, if you decrease the volumeof a container of gas and hold the temperatureconstant, the pressure of the gas will increase. An increase in the volume of the container causes thepressure to drop, if the temperature remains constant.
Section3Behavior of GasesBoyle’s Law Boyle’s law states that as pressure is decreased thevolume increases. The opposite also istrue, as shown by thegraph. As the pressure isincreased, thevolume willdecrease.
Section3Behavior of GasesBoyle’s Law in Action When Boyle’s law is applied to a real life situation,we find that the pressure multiplied by the volume isalways equal to a constant if the temperature isconstant.
Section3Behavior of GasesBoyle’s Law in Action You can use the equations P1V1 constant P2V2 toexpress this mathematically. This shows us that the product of the initial pressureand volume designated with the subscript 1 is equalto the product of the final pressure andvolume designated with the subscript 2.
Section3Behavior of GasesThe Pressure-Temperature Relationship What happens if you heat an enclosed gas? Theparticles of gas will strike the walls of the canister moreoften. If the pressure becomes greater than the canister canhold, it will explode. At a constant volume, an increase in temperatureresults in an increase in pressure.
Section3Behavior of GasesCharles’s Law Jacques Charles (1746-1823) was a French scientistwho studied gases. According to Charles’s law, the volume of a gasincreases with increasing temperature, as long aspressure does not change
Section3Behavior of GasesCharles’s Law As with Boyle’s law, the reverse is true, also.
Section3Behavior of GasesCharles’s Law Charles’s law can be explained using the kinetic theoryof matter. As a gas is heated, its particles move faster and fasterand its temperature increases. Because the gas particles move faster, they begin tostrike the walls of their container more often and withmore force.
Section3Behavior of GasesUsing Charles’s Law The formula that relates the variables of temperature tovolume shows a direct relationship when temperature isgiven in Kelvin. When using Charles’s law, the pressure must be keptconstant.
Section3Behavior of GasesUsing Charles’s Law What would be the resulting volume of a 2.0-L balloon at20.0 C that was placed in a container of ice water at3.0 C?
Section3Behavior of GasesUsing Charles’s Law As Charles’s law predicts, the volume decreased as thetemperature of the trapped gas decreased.
Matter and Thermal Energy Liquid State What happens to a solid when thermal energy or heat is added to it? The particles on the surface of the solid vibrate faster. These particles collide with and transfer energy to other particles. Soon the particles have enough kinetic
changes to thermal energy. Thermal energy causes the lamp's bulb to become warm to the touch. Using Thermal Energy All forms of energy can be changed into thermal energy. Recall that thermal energy is the energy due to the motion of particles that make up an object. People often use thermal energy to provide warmth or cook food. An electric space
Section 16.2 Thermal Energy . Three States of Matter Low Energy High School Dance Slow Song . Three States of Matter Medium Energy . Energy . Thermal Energy The total potential and kinetic energy of all the particles in an object Three things that thermal energy depends on: 1
using the words kinetic energy, thermal energy, and temperature. Use the space below to write your description. 5. Brainstorm with your group 3 more examples of thermal energy transfer that you see in everyday life. Describe where the thermal energy starts, where the thermal energy goes, and the results of the thermal energy transfer.
of matter. 474 Chapter 16 FOCUS Objectives 16.1.1 Explain how heat and work transfer energy. 16.1.2 Relate thermal energy to the motion of particles that make up a material. 16.1.3 Relate temperature to thermal energy and to thermal expansion. 16.1.4 Calculate thermal energy, temp
2:1 Matter and Energy MATTER: anything that has mass and takes up space Three States (phases) of Matter 1. SOLID: matter with definite volume and shape 2. LIQUID: matter with definite volume but no definite shape 3. GAS: matter with no definite volume nor shape How does Matter Change? PHYSICAL CHANGE: c
The electrical energy is transformed into thermal energy by the heat sources. The thermal energy has to meet the demand from the downstream air-conditioning system. Thermal en-ergy storage systems can store thermal energy for a while. In other words the storages can delay the timing of thermal energy usage from electricity energy usage. Fig. 1 .
Thermal Energy Changes in state are caused by changes in thermal energy. Thermal energy is the total potential and kinetic energies of an object. You can change an object’s state of matter by adding or removing thermal energy. When you add thermal energy to an object, these things can happen: Particles
Energies 2018, 11, 1879 3 of 14 R3 Thermal resistance of the air space between a panel and the roof surface. R4 Thermal resistance of roof material (tiles or metal sheet). R5 Thermal resistance of the air gap between the roof material and a sarking sheet. R6 Thermal resistance of a gabled roof space. R7 Thermal resistance of the insulation above the ceiling. R8 Thermal resistance of ceiling .
