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Feb 10

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

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Feb 10

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  1. 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

  2. Demo # 2 Kinetic Theory • Introduction to unit 3 • Title = kinetic theory demo • Question – is the kinetic theory of matter true??

  3. 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

  4. Unit 3: Properties and States of Matter

  5. 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.

  6. SOLIDLIQUIDGAS Three states of matter • Definite Shape • Definite Volume • Cannot be compressed • Cannot flow • Definite Volume • Can flow • No definite Shape • Cannot be compressed • No definite Volume • No definite Shape • Can flow • Can be compressed

  7. 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

  8. Plasma TV • Different type of plasma • Here we have a gas that the electrons are just loose- not bound to any nucleus • lightning

  9. Kinetic Theory • Motion in a gas The constant motion of particles in a gas allows a gas to fill any container • Three Main points • Particles of a gas are in constant, random motion • The motion of one particle is unaffected by another unless they collide • The Forces of attraction among particles can be ignored • POSITIVE AND NEGATIVE CHARGES Ex) air freshener

  10. 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

  11. 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

  12. 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

  13. Schedule • Warm up-fast fact • Phase Changes • Kinetic theory lab • Phase change handout – in you packet from yesterday

  14. 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

  15. 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 ”

  16. 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

  17. ExampleData Table in notebook

  18. After your done with the water • Build your graph • Answer the conclusion questions

  19. Honors • You must write a formal lab on this experiment

  20. 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

  21. 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

  22. Phase Change Graph

  23. Common Phase changes • 1. Melting solid -> liquid • 2. Freezing liquid -> solid • 3. Vaporization liquid -> gas , endothermic • 4. Evaporation liquid -> gas , below boiling point • 5. Condensation gas - > liquid, cloudy bathroom mirror • 6. Sublimation solid - > gas, dry ice • 7. Deposition Gas -> solid, Frost on a window

  24. 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

  25. 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

  26. 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

  27. After Lab • Vocab – now its late • Phase change handout • Was in back of packet • Atomic Model Project is due Monday

  28. 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?

  29. Composition of Matter

  30. Matter • Anything that has mass and takes up space • pure substance or mixture

  31. Pure Substance • A pure substance can not be broken down physically into anything else. • Element • Compound

  32. 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

  33. 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

  34. Pure Substances • Compound • properties differ from those of individual elements • EX: table salt (NaCl)

  35. Pure Substances • For example… Two different compounds, each has a definite composition.

  36. Inorganic vs. Organic Compounds • Inorganic compounds have no Carbon • NaCl, H2O, NH4 • Organic compounds have carbon • C6H12O6 C2H6

  37. Biological Organic Compounds • Proteins – egg, meat • Carbohydrates – bread, sugar, pasta • Lipids – lard, butter, oil

  38. Quick Quiz On A separate piece of paper answer the following question using your notes • 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?

  39. Mixtures • two or more substances that can be physically separated

  40. Heterogeneous Mixtures • Heterogeneous mixture: See component parts • Examples • Granite • Concrete • Dry Soup Mix

  41. Homogeneous Mixtures • Homogeneous mixture: cannot see component parts • Examples: • Kool Aid • Sweet Tea

  42. 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)

  43. A “microscopic” view

  44. Classifying Matter

  45. Quiz 1. Classify the following as an element, compound, or mixture (heterogeneous or homogeneous). • _____ air _____ oxygen • _____ tin can _____ sugar • _____ Windex _____ Salad dressing • _____ sand and sugar _____ gummi bear 2. A white solid is dissolved in water. The resulting colorless, clear liquid is boiled in a beaker until dryness. White crystals remain in the beaker. The liquid can be classified as a(n) ______________. HO E E OC HO HE HE HO -Which box represents an element, a compound and a mixture? Homogeneous mixture

  46. 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 Type of Mixture Solid/liquid Composition Homo mixture

  47. Review Lab

  48. Mixtures can be separated by… • Dissolving • Filtering • Evaporating • Magnetic Separation • Chromatography

  49. Unit 6 Quiz

  50. 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

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