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  1. 1. 3.4 Elements and Compounds Objective Addressed: 1.11 Distinguish between elements and compounds
  2. 3. Elements <ul><li>Pure substance that can’t be broken down by physical or chemical means </li></ul><ul><li>92 naturally occurring on Earth (#1-92) </li></ul><ul><li>Each has a symbol of 1-3 letters </li></ul><ul><ul><li>First letter is always capital </li></ul></ul><ul><ul><li>Second, third are always lower case </li></ul></ul>
  3. 4. Periodic Table <ul><li>Organized listing of elements </li></ul><ul><li>Modern version devised by Dmitri Mendeleev (1869) </li></ul><ul><ul><li>Put elements in order by atomic mass </li></ul></ul><ul><ul><li>Noticed patterns of physical properties </li></ul></ul>
  4. 5. Compounds <ul><li>2 or more elements combined chemcially </li></ul><ul><li>Approx. 10 million known </li></ul><ul><ul><li>Plus 100,000 each year </li></ul></ul><ul><li>Chemical Formula </li></ul><ul><ul><li>Lists elements by symbol </li></ul></ul><ul><ul><li>Show relative amounts with subscripts </li></ul></ul><ul><ul><li>Eg. NaCl H 2 O C 6 H 12 O 6 </li></ul></ul>
  5. 6. Separating compounds <ul><li>Can’t be done by physical means </li></ul><ul><ul><li>Chemical Reaction </li></ul></ul><ul><ul><li>Addition of energy (maybe a lot!) </li></ul></ul><ul><li>Compounds have completely DIFFERENT properties than components </li></ul>
  6. 7. Types of Matter
  7. 8. Law of Definite Proportions <ul><li>Compounds always composed of same elements in the same proportions by mass </li></ul><ul><li>Eg. Water is made of 2 parts H to 1 part O </li></ul><ul><li>Expressed as percent by mass </li></ul>
  8. 9. Percent by mass of Sucrose
  9. 10. Practice Problems p. 88 <ul><li>19 . 15.9% </li></ul><ul><li>20 . 5.0% </li></ul><ul><li>21 . X = 25%; Y = 75% </li></ul><ul><li>22 . No </li></ul><ul><li>23 . No </li></ul><ul><li>Don’t need to review any </li></ul>
  10. 11. 19. A 78.0-g sample of an unknown compound contains 12.4 g of hydrogen. What is the percent by mass of hydrogen in the compound?
  11. 12. 20. 1.0 g of hydrogen reacts completely with 19.0 g of fluorine. What is the percent by mass of hydrogen in the compound that is formed?
  12. 13. 21. If 3.5 g of element X reacts with 10.5 g of element Y to form the compound XY, what is the percent by mass of element X in the compound that is formed?
  13. 14. 22. Two unknown compounds are tested. Compound I contains 15.0 g of hydrogen and 120.0 g of oxygen. Compound II contains 2.0 g of hydrogen and 32.0 g of oxygen. Are the compounds the same? Explain your answer.
  14. 15. 23. CHALLENGE: All you know about two unknown compounds is that they have the same precent by mass of carbon. With only this information, can you be sure the two compounds are the same? Explain.
  15. 16. Law of Multiple Proportions <ul><li>Different compounds can be made of the same elements </li></ul><ul><li>Elements will be present in different proportions by mass </li></ul><ul><li>Eg. </li></ul><ul><ul><li>Water (H 2 O) and </li></ul></ul><ul><ul><li>Hydrogen Peroxide (H 2 O 2 ) </li></ul></ul>
  16. 17. Multiple Proportions con’t <ul><li>Mass ratios of various compounds will relate to each other in a small whole-number ratio </li></ul>
  17. 18. End of section questions <ul><li>24. Elements are made of single atoms and cannot be easily divided; Compounds are made of molecules and can be divided chemically </li></ul><ul><li>25. In order by atomic mass, grouped by recurring properties </li></ul><ul><li>28. Not the same. Ratio is </li></ul><ul><li>29.H = 5.5953%; O = 88.809% </li></ul>
  18. 19. 24. Compare and contrast elements and compounds
  19. 20. 25. Describe the basic organizational feature of the periodic table of the elements
  20. 21. 28. Complete the table, and then analyze the data to determine if Compounds I and II are the same compound. If the compounds are different, use the law of multiple proportions to show the relationship between them.
  21. 22. 29. Calculate the mass percent of hydrogen in water and th mass percent of oxygen in water.
  22. 23. 66. Correct the following statements: <ul><li>An element is a combination of two or more compounds. </li></ul><ul><li>When a small amount of sugar is completely dissolved in water, a heterogeneous solution is formed. </li></ul>
  23. 24. 67. Name the elements contained in the following compounds: <ul><li>Sodium chloride (NaCl) </li></ul><ul><li>Ammonia (NH 3 ) </li></ul><ul><li>Ethanol (C 2 H 6 O) </li></ul><ul><li>Bromine (Br 2 ) </li></ul>
  24. 25. 68. What was Dmitri Mendeleev’s major contribution to the field of chemistry?
  25. 26. 70. How are th properties of a compound related to those of the elements that comprise it?
  26. 27. 72. Find the percent by mass of: <ul><li>Carbon in 44g of Carbon Dioxide (CO 2 ) </li></ul><ul><li>Oxygen in 44g of Carbon Dioxide (CO 2 ) </li></ul>
  27. 28. 73. Complete the table: H 2 O 2 H 2 0 CuO NaCl Ratio of elements Compound Ratios of Elements in Compounds
  28. 29. 74. A 25.3-g sample of an unknown compound contains 0.8 g of oxygen. What is the percent by mass of oxygen in the compound?
  29. 30. 75. Magnesium combines with oxygen to form magnesium oxide. If 10.57 g of magnesium reacts completely with 6.96 g of oxygen, what is th percent by mass of oxygen in magnesium oxide?
  30. 31. 76. When mercury oxide is heated, it decomposes into mercury and oxygen. If 28.4 g of mercury oxide decomposes, producing 2.0 g of oxygen, what is the percent by mass of mercury in mercury oxide?