Review 1st 6_weeks

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Review 1st 6_weeks

  1. 1. 1 st 6 Weeks Review Test Wednesday Remember your pencil and calculator
  2. 2. Part I.  Classify each of the following substances as; an element, a compound, a solution, or a heterogeneous mixture. Salt Water Solution Salad Dressing Mixture Oxygen Element Bronze mixture Gold Element Carbon Dioxide Compound Pure Air Mixture Soda Solution Soil Mixture Pure Water Compound Salt Compound Sand Mixture
  3. 3. Part II.   In the spaces provided, describe the distinguishing characteristics of the major categories of matter. <ul><li>Element – A substance that cannot be separated or broken down into simpler substances by chemical means; can be found on periodic table. </li></ul><ul><li>Compound – A substance made up of atoms of two or more different elements joined by chemical bonds </li></ul><ul><li>Solution – a homogenous mixture throughout which two or more substances are uniform. </li></ul><ul><li>Mixture – a combination of two or more substances that are not chemically combined. </li></ul>
  4. 4. Part III.  Classification - State whether each of the following changes would be physical or chemical. Burning Propane Chemical Cooking Chemical Painting Wood Physical Breaking Glass Physical Burning Wood Chemical Melting Ice Physical
  5. 5. Part IV.  Define - Use your own words to define each of the following terms in the space provided. <ul><li>Chemical Change – a change that occurs when one or more substances change into entirely new substances with different properties. </li></ul><ul><li>Physical Change – A change of matter from one form to another without a change in chemical properties. </li></ul><ul><li>Change of State of Phase – When a substance changes from one state of matter to another. </li></ul>
  6. 6. Part V <ul><li>18 m = 1800 cm </li></ul><ul><li>167 mm = (typo change to m) 0.167 m </li></ul><ul><li>500 kg = 500,000 g </li></ul><ul><li>23 dm = 0.023 hm </li></ul><ul><li>1,589 dl = (typo change to kl) 0.1589 kl </li></ul><ul><li>700 ml = 0.000700 kl </li></ul><ul><li>5 cm = 50 mm </li></ul><ul><li>35.45 mg = 0.0003545 hg </li></ul><ul><li>0.5 l = 0.0005 kl </li></ul><ul><li>130 Dg = 13.0 kg </li></ul>
  7. 7. Density (#11) <ul><li>m = 453 g; V = 225 cm 3 </li></ul><ul><li>d = m/v = 453 g/225 cm 3 = 2.01 g/ cm 3 </li></ul><ul><li>b) m = 5.0 g; V = 10.0 cm 3 </li></ul><ul><li>d = m/v = 5.0g/10.0 cm 3 = 0.50 g/ cm 3 </li></ul><ul><li>c) m = 26.1 g; V = 2.0 mL </li></ul><ul><li>d = m/v = 26.1g/2.0 mL = 13.1 g/mL </li></ul>#12 m = 75.2 g; V = 89.2 mL d = m/v = 75.2 g / 89.2 mL = .84 g/mL
  8. 8. <ul><li>#13 m = 1450 g; V = 542 mL </li></ul><ul><li>d = m/v = 1450 g / 542 mL = 2.68 g/mL </li></ul><ul><li>#14 Scientific Method </li></ul><ul><li>Problem </li></ul><ul><li>Hypothesis </li></ul><ul><li>Experiment </li></ul><ul><li>Analyze Data </li></ul><ul><li>Conclusion/Retest </li></ul>
  9. 9. Gas Laws <ul><li>Boyles Law P 1 V 1 = P 2 V 2 (inverse relationship) </li></ul><ul><li>When pressure increases volume decreases </li></ul><ul><li>When pressure decreases volume increases </li></ul><ul><li>Charles Law V 1 /T 1 = V 2 /T 2 (direct relationship) </li></ul><ul><li>When temperature increases volume increases </li></ul><ul><li>When temperature decreases volume decreases </li></ul>

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