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Mid-Year Review

Mid-Year Review. Thursday January 29, 2009. Mrs. McCarthy’s 8 th Grade Physical Science. Test Set-up. 66 Total Multiple Choice Questions Including: 4 Understanding Diagram Questions 5 Measuring Questions Many Vocabulary Definitions 2 Open Response from a choice of 4 Questions.

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Mid-Year Review

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  1. Mid-Year Review Thursday January 29, 2009 Mrs. McCarthy’s 8th Grade Physical Science

  2. Test Set-up • 66 Total Multiple Choice Questions • Including: • 4 Understanding Diagram Questions • 5 Measuring Questions • Many Vocabulary Definitions • 2 Open Response from a choice of 4 Questions

  3. Study Tips • Study and Review with previous tests and quizzes (several repeat questions) • Book Walk and Chapter Highlights at the end of each unit • Midyear Exam study guide • Midyear Exam PowerPoint • After-school Extra-help

  4. Content Overview • Introduction to Physical Science (Notes/Ch 1 Text) • Scientific Method • Lab Safety • Metric Measurement • Properties of Matter (Chapter 1) • States and Phases of Matter (Chapter 2) • Atoms (Chapter 4) • Periodic Table (Chapter 5)

  5. Measurement • Mass • Weight • Volume • Temperature

  6. Mass • The amount of matter in an object • Doesn’t change with gravity • Measured with a triple-beam balance • SI unit of grams

  7. Inertia • A resistance to a change in motion • The more mass an object has, the more inertia it has • Example: Grocery Carts & Cars

  8. Weight • The amount of • Measured with a Spring Scale • Changes with gravity • Measured in Newtons

  9. Volume • The amount of space an object takes-up • Can be measured with a ruler using the formula: Volume = length * width * height

  10. OR • Volume can be measured with water and a graduated cylinder using displacement • Solid SI Unit of cm³ • Liquid SI Unit of mL

  11. Density • The amount of mass in a given volume • Measured with the Formula: Density = Mass / Volume * Labeled in g/cm³ Mass ______________ Density * Volume

  12. Density Stackers • Many liquid mixtures will stack up into layers by their densities • More dense materials will be below less dense materials • Example: Salad Dressing Least Dense Most Dense

  13. Characteristic Properties • Describe substances based upon their characteristics: Physical Properties Chemical Properties Statue of Liberty Log of Wood

  14. Physical Properties • Physically describe an object based upon observable and measurable observations Examples: COLOR Density Solubility Mass Malleability Texture Volume Temperature State Weight Ductility

  15. Physical Changes • A change in a substance that affects one or more physical properties of a substance • The substance does not change • Examples: Cutting Hair Crushing a Can Sanding Wood Broken Glass Melting Butter Freezing Water Dissolving Salt Bending Metal

  16. Chemical Properties • Describe substances based upon their ability to change into a new substance with different properties • Chemical properties are not easily observed with your senses and often need to be tested • Examples: Reactivity: Tarnishing, Rusting Flammability

  17. Chemical Changes • When substances change into new substances with different properties • Examples: Gas Formation & Bubbles Burning Cooking Reactivity

  18. States of Matter Plasma

  19. Solid • Has a definite shape and a definite volume • Movement: Particles are held tightly in together and vibrate in place Looks Like

  20. Liquid • Have a definite volume and no definite shape • Take the shape of a container • Can Pour • Particles slide past one another Looks Like

  21. Gas • Have NO Definite Shape or Volume • Fill their containers • Particles spread out and move independently Looks Like

  22. Plasma • Very high in energy • Plasma has no definite shape or volume • Particles are broken • Plasma is the most common phase of matter in the universe • Examples: Stars, Auroras, lightning, fire, neon lights

  23. Charles’ Law • The volume of a gas increases as its temperature increases T^ v^ • For Example: • A balloon expands and pops when it is heated. • A balloon contracts and gets smaller when it is cooled.

  24. Boyle’s Law • The volume of gas increases as the pressure decreases v^, Pv • Example: Piston • Lifting the Plunger Decreases the Pressure • Pushing the Plunger Increases the Pressure

  25. Atomic Theory • Democritus- Proposes the Atom 440 B.C. • Dalton- Atoms are the Smallest Particle • Thomson- “Plum Pudding” with Electrons • Rutherford- Gold Foil → Atom’s Nucleus • Bohr- Electrons Travel in Energy Paths • Schrödinger & Heisenberg- Electron Clouds

  26. Atomic Theory

  27. Atom • The Smallest Unit of an Element that has the characteristics of that element. Energy Levels Nucleus with Protons and Neutrons Electrons

  28. Atoms • Very small • Can’t be seen with the naked eye • Only seen with an extremely powerful microscope Scanning Tunneling Microscope is 3.5 million times magnified. The atom was first seen in 1981.

  29. Atoms • Everything that is MATTER is made of atoms • Atoms are the most basic form of matter: “Building Blocks of Matter”

  30. Protons • Charge: Positive • Mass:1 amu • Location: Nucleus • Proton count determines the element • Protons = atomic number

  31. Neutrons Charge: none Mass: 1 amu Location: Nucleus *To find the neutrons: atomic mass – atomic number

  32. Electrons • Charge: Negative • Mass: Almost Zero • Location: Electron Clouds • Balanced Atoms: Protons = Electrons

  33. Isotopes • Atoms that have the same number of protons but have different numbers of neutrons • Atoms that are isotopes of each other are always the same element because the number of the protons in each atom is the same.

  34. Valance Electrons • Electrons in the outermost energy level of an atom. • Valance Electrons are important in determining how an atom will bond to make compounds. • Example: 1 Valance Electron

  35. Charges • An atom is neutral with no overall charge because the protons are equal to the electrons. • If an atom gains or loses an electron it becomes unbalanced and is called an ion. Negative Ions have gained electrons Positive Ions have lost electrons

  36. Atomic Forces • *Strong Force: Holds Nucleus Together • *Electromagnetic Force: opposites attract • Gravity: very small because of atom size • Weak Force: radioactive

  37. Periodic Table • Organized Data of Elements • Organized by Atomic Number • Contains Many Patterns • Element Cube: An Element Cube Contains specific information about each element on the periodic table 2 Atomic Number He Chemical Symbol Helium Element Name 4.0 Atomic Mass

  38. Groups Also called families Vertical Columns on the Periodic Table Elements in the same group have similar properties Periods Horizontal Rows on the Periodic Table Organized by Atomic # Periodic Tableof the Elements

  39. Elements Left of zigzag line Right of zigzag line Border the zigzag line

  40. Pure Substances • A substance with only one type of particle • Examples: Elements & Compounds • Pure Substances Cannot be Broken Down and Retain their Properties

  41. Elements A pure substance that cannot be separated into simpler substances by physical or chemical means Smallest unit is an atom Examples: Iron – Fe Oxygen – O Gold – Au Compounds A pure substance made from 2 or more elements that are chemically combined Smallest Unit is a molecule Examples: Salt - NaCl Water - H2O Carbon Dioxide - CO2 Pure Substances

  42. Open Response • Four multi-part opens response questions will be included on your mid-year exam. • You will need to answer any two of the four questions asked. • Be sure to include: • Graphic Organizer • Vocabulary Words & Definitions • Explain • Examples • Labels • Diagrams

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