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Download Unit 3: Properties and States of Matter
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Feb 10 • Warm up – grab a packet from the black cart And • Warm up - Get your lab notebook set it up for a demo If you did not take the test or finish the test yesterday see me Demo # 2 Kinetic Theory • Introduction to unit 3 • Title = kinetic theory demo • Question – is the kinetic theory of matter true?? Demo – Kinetic theory • Main idea – all matter is made up of particles and these particles are always moving to some extent • Crushing this can without using my hands is an example of this Unit 3: Properties and States of Matter Kinetic Theory • The kinetic theory explains how particles move in different states of matter. – All matter is composed of small particles (molecules, atoms, and ions). – The particles are in constant, random motion. – The amount of motion is proportional to the temperature. Increased temperature means increased motion. – Solids, liquids and gases differ in the freedom of motion of their particles and the extent to which the particles interact. Three states of matter SOLID LIQUID GAS •Definite Shape •Definite Volume •Definite Volume •Can flow •No definite Volume •Cannot be compressed •Cannot flow •No definite Shape •Cannot be compressed •No definite Shape •Can flow •Can be compressed Plasma • The new fourth state of matter • When any matter becomes tooo hot the electrons are stripped / fall off • This matter shares properties of a gas and a liquid • Examples - sun Plasma TV • Different type of plasma • Here we have a gas that the electrons are just loose- not bound to any nucleus • lightning Kinetic Theory • Motion in a gas The constant motion of particles in a gas allows a gas to fill any container • Three Main points 1. Particles of a gas are in constant, random motion 2. The motion of one particle is unaffected by another unless they collide 3. The Forces of attraction among particles can be ignored • POSITIVE AND NEGATIVE CHARGES Ex) air freshener Kinetic Theory • Motion in a liquid – Particles in a liquid are more closely packed than particles in a solid • Attractive forces apply – A Liquid can take the shape of a container because the particles of a liquid can flow to new locations • The Volume of a liquid is constant because of the attractive forces between particles keep them together Kinetic Theory • Motion in a solid – Solids have a definite shape and volume because particles are in a solid vibrate in a fixed location ex) People sitting in a theatre or a classroom Warm-Up – get you lab notebook • Put this in your lab notebook • What state of matter has… – 1. Definite shape, definite volume – 2. No definite shape, no definite volume – 3. Definite volume, no definite shape – Choices – solid, liquid , and gases Schedule • Warm up-fast fact • Phase Changes • Kinetic theory lab • Phase change handout – in you packet from yesterday Fast Fact - What is the origins of Valentines day • 290 AD – Rome declared the soldiers could not be married • Secretly went to Bishop Valentine to get married • Became a saint and his day is Feb 14th Kinetic theory lab – put this in lab note book Title – kinetic theory lab Problem – we need to understand what is a phase change Data- leave space for a data table Conclusion – “ answer questions from lab ” Kinetic Theory Lab • Remember – Every minute take a reading from the thermometer – Once the beaker is on the hot plate DO NOT TOUCH IT – Mark , highlight when the ice has completely turned into water, and when water begins to boil – Continue to take data until the water has completely boiled for 5 minutes Example Data Table in notebook time (min) temperature (C) 0 1 1 5 2 11 3 12 4 13 5 14 6 15 7 15 After your done with the water • Build your graph • Answer the conclusion questions Honors • You must write a formal lab on this experiment Thermal Energy • Thermal energy is heat. It can also be defined as the sum of the kinetic energy of the particles in a substance. Has to do with temperature and mass. – Temperature is a measurement of the average kinetic energy of a substance. • Increases kinetic energy (speed of particles) • Higher Temperature = molecules moving faster – Solid < Liquid < Gas Phase Change • Definition – the reversible physical change that occurs when a substance changes from one state of mater into another • The temperature does not change during a phase change • Energy is either stored or released during a phase change Phase Change Graph Common Phase changes • • • • 1. Melting 2. Freezing 3. Vaporization 4. Evaporation solid -> liquid liquid -> solid liquid -> gas , endothermic liquid -> gas , below boiling point • 5. Condensation gas - > liquid, cloudy bathroom mirror • 6. Sublimation • 7. Deposition solid - > gas, dry ice Gas -> solid, Frost on a window Freezing / Melting point • Freezing point – Temperature in which a liquid becomes a solid • Molecules become more closely packed together • Water – below 0 degrees C • Melting Point – temperature in which a solid become a liquid – Every solid has a different MP • Water – Above 0 Celsius • Mercury - -32 C Boiling Point / Condensation • Boiling point – Temperature where a liquid becomes a gas • Water 90-100 degrees C Surface area – part of water that is exposed Larger surface area – faster reaction • Condensation – A Gas cools to become a liquid – Water on a mirror after a shower Sublimation • • • • Were a solid changes into a gas Dry ice Endothermic reaction – need energy Dry ice absorbed the heat energy from its environment and transformed straight into a gas After Lab • Vocab – now its late • Phase change handout • Was in back of packet • Atomic Model Project is due Monday Liquid Nitrogen • • • • Beaker: What is the boiling point? Balloons: Do you see the three phases? Apples and Bananas: Solids are Brittle Placed in a bottle: Can Anyone Explain? Composition of Matter Matter • Anything that has mass and takes up space • pure substance or mixture Pure Substance • A pure substance can not be broken down physically into anything else. –Element –Compound Element • Element – on periodic table • Elements are composed of only one type of atom • Has one capital letter – Na – Cl –F • Atom – smallest particle of an element Compound or Molecule • Compound – combo of 2 or more elements • Two or more capital letters – NaCl – H2O – MgO2 – CO2 • Molecule – smallest part of a compound Pure Substances • Compound – properties differ from those of individual elements – EX: table salt (NaCl) Pure Substances • For example… Two different compounds, each has a definite composition. Inorganic vs. Organic Compounds • Inorganic compounds have no Carbon – NaCl, H2O, NH4 • Organic compounds have carbon – C6H12O6 C2H6 Biological Organic Compounds • Proteins – egg, meat • Carbohydrates – bread, sugar, pasta • Lipids – lard, butter, oil Quick Quiz On A separate piece of paper answer the following question using your notes 1. 2. 3. 4. 5. What is the difference between the melting phase and the freezing phase? List the qualification of a liquid? Write an example of a substance in each phase of matter? What is the difference between an Element and a compound? What is the difference between a organic and inorganic compound? Mixtures • two or more substances that can be physically separated Heterogeneous Mixtures • Heterogeneous mixture: See component parts • Examples –Granite –Concrete –Dry Soup Mix Homogeneous Mixtures • Homogeneous mixture: cannot see component parts • Examples: –Kool Aid –Sweet Tea Mixtures can be… • • • • Gas in Gas (air) – what we breath Gas in Liquid (soda) the carbonation Liquid in Liquid (mixed fruit juices) Liquid in Solid (Iced Tea) – energy needs to be implied • Solid in Solid (Concrete, Alloys) A “microscopic” view Classifying Matter Quiz 1. Classify the following as an element, compound, or mixture (heterogeneous or homogeneous). HO E • _____ air _____ oxygen • _____ E tin can _____ OC sugar • _____ Windex _____ Salad dressing HO HE HE sand and sugar HO • _____ _____ gummi bear -Which box represents an 2. A white solid is dissolved in water. The resulting colorless, element, a compound a clear liquid is boiled in a beaker until dryness. White and crystals remain in the beaker. Themixture? liquid can be classified as a(n) Homogeneous mixture ______________. Complete Identification and Separation Lab Identify each of the items as an element, an inorganic compound, an organic Compound, a homogeneous mixture, or a heterogeneous mixture. If it is a Mixture, tell the type (gas/gas, gas/liquid, etc) • Example – Saltwater Composition Homo mixture Type of Mixture Solid/liquid Review Lab Mixtures can be separated by… • • • • • Dissolving Filtering Evaporating Magnetic Separation Chromatography Unit 6 Quiz Warm Up • Please place your formal lab report on the front table. • What type of substance can be separated using physical means such as evaporating, distilling, filtering, chromatography, or magnetic separation? – Answer choices: elements, compounds, or mixtures Review Quiz • More Practice Identifying Matter Physical/Chemical Properties Lab • Label the top of the next full page in your composition notebook with the title above and today’s date (2/21/2008). • Write the definition for Physical and Chemical properties. – Physical Properties: Any characteristic of a material that you can observe directly or measure with a tool without changing the composition of the substance. (It does not change chemically) – Chemical Properties: Any characteristic of a material that indicates whether it can undergo change that will alter the composition of the substance. (It does change chemically) Make a table like this in your composition notebook to record your data Physical/Chemical Properties Lab • You and your lab partner must go around to each station and identify whether the property being demonstrated is a physical or chemical property and state why. These are the properties you have to choose from • boiling point, combustion, freezing/melting point, density, oxidation, solubility, viscosity, conductivity, corrosion, acid or base Warm-Up • Please make a list of physical and chemical properties: Physical Properties (7) Boiling point Melting/freezing point Solubility Conductivity Density Viscosity Acid or base Chemical Properties (3) Oxidation Corrosion Combustion Physical Property • Any characteristic of a material that you can observe directly or measure with a tool without changing the composition of the substance. (It does not change chemically) • Examples: boiling point, freezing/melting point, density, solubility, viscosity, electrical conductivity. Viscosity • A fluid’s resistance to flow – High viscosity fluids take longer to pour. – Viscosity may change with temperature. • Viscosity Demo Conductivity • Ability to transmit electrons (electricity) – Conductors vs. insulators • Metals – good conductors • Non metals – insulators • Some solutions are good conductors that contain dissolved ions (electrolytes). Solubility • Ability to dissolve or be dissolved • Solubility increased by: 1. Temperature 2. Surface Area 3. Stirring Density • Density – the amount of mass of an object related to its volume • Density = mass (Kg) / volume (cm3) Complete Density Lab • When finished let me see your data. • Once I check your data: • Work on the density problems on the last page of your packet. • HW: Density Drill (In your packet) front side only Review Density Lab Density Problems • HW: Lab Report and Density Sheet due tomorrow Warm-Up • What is the density of a piece of wood that has a mass of 24.0 grams and a volume of 12.0 cm3? – What would the density be if the piece of wood were cut in half? • A piece of wood that measures 3.0 cm by 6.0 cm by 4.0 cm has a mass of 36.0 grams. What is the density of the wood? Would the piece of wood float in water? (volume = L x W x H) • The volume of a solution went from 40 ml to what you see above in a graduated cylinder after putting in a gold ring. If the mass of the gold ring is measured to be 30 grams, what is the density of the gold ring? Review Density Lab 1 cm3 = 1mL = 1 g Acids and Bases • Acids – – – – – – – – Form hydrogen (H+) ions in solution Low pH ( < 7 ) Sour/tart taste electrolytes React with metals to form H2 gas Corrosive – tissue damage/burns Change color of indicators React with bases to form salt & water • Bases – – – – – – – – – Form hydroxide (OH-) ions in solution High pH ( > 7 ) Bitter taste electrolytes Feel slippery Often crystalline solids when undissolved Corrosive – burns Change color of indicators React with acids to form salt & water pH • pH is a measure of the concentration of H+ ions in solution (0-14) – Acids < 7 – Neutral = 7 – Bases > 7 • pH meter uses electrodes to read electrical conductivity in solution • pH paper changes color when exposed to acids/bases – match pH paper color to a chart to get pH – Follows ROYGBIV A-B Litmus • Litmus paper is another common indicator – Acids turn it red – Bases turn it blue Common Examples • Acids – – – – – – Citric Lactic Acetic (vinegar) Carbonic (carbonated drinks) Hydrochloric (HCl – stomach acid) Sulfuric, Nitric, Phosphoric (fertilizers) • Bases – – – – Ammonia Clorox Magnesium Hydroxide (antacid) Sodium hydroxide (soap, oven/drain cleaners) – Aluminum Hydroxide (antacid, water purification, color-fast fabrics) LAB: Acids and Bases Warm Up • Get started on Acid-Base WS from your packet. – Omit #’s 7, 13, 15 on front and compound B on the back Neutralization • Acids and Bases neutralize each other – Acid + Base Salt + Water • HCl + NaOH H2O + NaCl Chemical Property • Characteristic of a material that indicates whether it can undergo change that will alter the composition of the substance. (It does change chemically) • Examples: Oxidation, Corrosion, Combustion Oxidation • Ability to bind with oxygen during a reaction – Iron rusting • Iron + Oxygen 2 Fe + O2 Iron oxide 2 FeO Combustibility • Ability to burn – Cremora Demo Corrosion • Ability to break down a metal – Silver Tarnishing • Silver + Sulfur Ag + S Silver Sulfide AgS Decomposition React/Not react with acids Warm Up • Get out practice test and get ready for review.