1 / 83

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

soo
Download Presentation

Feb 10

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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

More Related