Ch2 z53 particles


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Ch2 z53 particles

  1. 1. Chapter 2 Atoms, Molecules, and Ions pp
  2. 2. History Greeks Democritus and Leucippus - atomos Aristotle- elements. Alchemy 1660 - Robert Boyle- experimental definition of element. Lavoisier- Father of modern chemistry. He wrote the book.
  3. 3. Laws Conservation of Mass Law of Definite Proportion - compounds have a constant composition. They react in specific ratios by mass. Multiple Proportions - When two elements form more than one compound, the ratios of the masses of the second element that combine with one gram of the first can be reduced to small whole numbers.
  4. 4. What?! Water has 8 g of oxygen per g of hydrogen. Hydrogen peroxide has 16 g of oxygen per g of hydrogen. 16/8 = 2/1 Small whole number ratios.
  5. 5. Proof Mercury has two oxides. One is 96.2 % mercury by mass, the other is 92.6 % mercury by mass. Show that these compounds follow the law of multiple proportion. Speculate on the formula of the two oxides.
  6. 6. Dalton’s Atomic Theory Elements are made up of atoms Atoms of each element are identical. Atoms of different elements are different. Compounds are formed when atoms combine. Each compound has a specific number and kinds of atom. Chemical reactions are rearrangement of atoms. Atoms are not created or destroyed.
  7. 7. Gay-Lussac- under the same conditions of temperature and pressure, compounds always react in whole number ratios by volume. Avagadro - interpreted that to mean . . . at the same temperature and pressure, equal volumes of gas contain the same number of particles. (called Avagadro’s Hypothesis ) A Helpful Observation
  8. 8. Figure 2.4 Representation of some of Gay-Lussac’s Experimental Results on Combining Gas Volumes
  9. 9. Figure 2.5 Representation of Combining Gases at the Molecular Level
  10. 10. Early Experiments to determine what an atom was J. J. Thomson- used Cathode ray tubes
  11. 11. Thomson’s Experiment + - Voltage source
  12. 12. Thomson’s Experiment + - Voltage source
  13. 13. Passing an electric current makes a beam appear to move from the negative to the positive end. Thomson’s Experiment + - Voltage source
  14. 14. Thomson’s Experiment By adding an electric field Voltage source
  15. 15. Thomson’s Experiment By adding an electric field, he found that the moving pieces were negative + - Voltage source
  16. 16. Thomsom’s Model Found the electron. Couldn’t find positive (for a while). Said the atom was like plum pudding. A bunch of positive stuff, with the electrons able to be removed.
  17. 17. Millikan’s Experiment Oil Atomizer Oil droplets Telescope - +
  18. 18. Millikan’s Experiment X-rays X-rays give some electrons a charge.
  19. 19. Millikan’s Experiment Some drops would hover From the mass of the drop and the charge on the plates, he calculated the mass of an electron
  20. 20. Figure 2.10 Diagram of the Millikan Apparatus
  21. 21. Radioactivity Discovered by accident Bequerel Three types Alpha- helium nucleus (+2 charge, large mass) Beta - high speed electron Gamma - high energy light
  22. 22. Rutherford’s Experiment Used uranium to produce alpha particles. Aimed alpha particles at gold foil by drilling hole in lead block. Since the mass is evenly distributed in gold atoms alpha particles should go straight through. Used gold foil because it could be made atoms thin.
  23. 23. Lead block Uranium Gold Foil Florescent Screen
  24. 24. What he expected
  25. 25. Because
  26. 26. Because, he thought the mass was evenly distributed in the atom.
  27. 27. What he got
  28. 28. Atom is mostly empty Small dense, positive piece at center. Alpha particles are deflected by it if they get close enough. How he explained it +
  29. 29. +
  30. 30. Figure 2.12 Rutherford’s Experiment on  particle Bombardment of Metal Foil
  31. 31. Figure 2.13 Expected and Actual Results of Rutherford’s Experiment
  32. 32. Modern View The atom is mostly empty space. Two regions Nucleus - protons and neutrons. Electron cloud - region where you might find an electron.
  33. 33. Sub-atomic Particles Z - atomic number = number of protons Z determines type of atom. A - mass number = number of protons + neutrons. Number of protons = number of electrons if neutral.
  34. 34. The Mass and Change of the Electron, Proton, and Neutron
  35. 35. Symbols X A Z Na 23 11
  36. 36. Chemical Bonds The forces that hold atoms together. Covalent bonding - sharing electrons. Makes molecules. Chemical formula - the number and type of atoms in a molecule. C 2 H 6 - 2 carbon atoms, 6 hydrogen atoms, Structural formula shows the connections, but not necessarily the shape.
  37. 37. There are also other models that attempt to show three dimensional shape. Ball and stick or space-filling. H H H H H H C C
  38. 38. Ions Atoms or groups of atoms with a charge. Cations - positive ions - get by losing electrons(s). Anions- negative ions - get by gaining electron(s). Ionic bonding - held together by the opposite charges. Ionic solids are called salts.
  39. 39. Polyatomic Ions Groups of atoms that have a charge. Yes, you have to memorize them. See list on page 66
  40. 40. Periodic Table
  41. 41. Metals Conductors Lose electrons Malleable and ductile
  42. 42. Nonmetals Brittle Gain electrons Covalent bonds
  43. 43. Semi-metals or Metalloids
  44. 44. Alkali Metals
  45. 45. Alkaline Earth Metals
  46. 46. Halogens
  47. 47. Transition metals
  48. 48. Noble Gases
  49. 49. Inner Transition Metals
  50. 50. +1 +2 -1 -2 -3
  51. 51. Naming compounds Two types Ionic - metal with non metal or with polyatomic ions. Covalent - we will just learn the rules for non-metals combined with non-metal.
  52. 52. Ionic compounds If the cation is monoatomic - Name the metal (cation) just write the name. Include a Roman numeral to indicate the oxidation state if the cation (metal) has more than one. If the cation is polyatomic - name it. If the anion is monoatomic - name it but change the ending to –ide. If the anion is poly atomic - just name it Practice.
  53. 53. Figure 2.22 Common Cations and Anions
  54. 54. Covalent compounds Two words, with prefixes. Prefixes tell you how many. mono, di, tri, tetra, penta, hexa, septa, nona, deca First element - use whole name with the appropriate prefix, except mono. Second element, -ide ending with appropriate prefix. Practice
  55. 55. More Naming
  56. 56. Ionic compounds If the cation is monoatomic- Name the metal (cation) just write the name. If the cation is polyatomic- name it If the anion is monoatomic- name it but change the ending to -ide If the anion is poly atomic- just name it Practice problems on following slides
  57. 57. Ionic Compounds Have to know what ions they form Get from periodic table, polyatomic, or figure out CaS K 2 S AlPO 4 K 2 SO 4 FeS CoI 3
  58. 58. Figure 2.23 Flowchart for Naming Binary Compounds
  59. 59. Figure 2.24 Overall Strategy for Naming Chemical Compounds
  60. 60. Ionic Compounds Fe 2 (C 2 O 4 ) MgO MnO KMnO 4 NH 4 NO 3 Hg 2 Cl 2 Cr 2 O 3
  61. 61. Ionic Compounds KClO 4 NaClO 3 YBrO 2 Cr(ClO) 6
  62. 62. Naming Covalent Compounds Two words, with prefixes Prefixes tell you how many. mono, di, tri, tetra, penta, hexa, septa, nona, deca First element whole name with the appropriate prefix, except mono Second element, -ide ending with appropriate prefix Practice
  63. 63. CO 2 CO CCl 4 N 2 O 4 XeF 6 N 4 O 4 P 2 O 10 Naming Covalent Compounds
  64. 64. Writing Formulas Two sets of rules, ionic and covalent To decide which to use, decide what the first word is. If is a metal or polyatomic use ionic. If it is a non-metal use covalent.
  65. 65. Ionic Formulas Charges must add up to zero. Get charges from periodic table, name of metal ion, or memorized from the list. Use parentheses to indicate multiple polyatomics.
  66. 66. Ionic Formulas Sodium nitride Sodium - Na is always +1 nitride - ide tells you it comes from the periodic table nitride is N -3
  67. 67. Ionic Formulas Sodium nitride Sodium - Na is always +1 Nitride - ide tells you it comes from the table nitride is N -3 Doesn’t add up to zero (if 1:1 ratio). Na +1 N -3
  68. 68. Ionic Formulas Sodium nitride sodium- Na is always +1 nitride - ide tells you it comes from the table nitride is N -3 Doesn’t add up to zero So, need 3 Na (“Cross the charges”) Na +1 N -3 Na 3 N
  69. 69. Ionic Compounds Sodium sulfite calcium iodide Lead (II) oxide Lead (IV) oxide Mercury (I) sulfide Barium chromate Aluminum hydrogen sulfate Cerium (IV) nitrite
  70. 70. Covalent compounds The name tells you how to write the formula duh Sulfur dioxide difluorine monoxide nitrogen trichloride diphosphorus pentoxide
  71. 71. Chemical Naming pp : P = cation Q = anion
  72. 72. More Names and formulas
  73. 73. Acids Substances that produce H + ions when dissolved in water. All acids begin with H. Two types of inorganic acids: Oxyacids Non-oxyacids Organic acids have -COOH group
  74. 74. Naming acids If the formula has oxygen in it write the name of the anion, but change ate to -ic acid ite to -ous acid Hint: “m -ic- e” or more than a “m -ous- e” Watch out for sulf ur ic and sulf ur ous H 2 CrO 4 HMnO 4 HNO 2
  75. 75. Naming acids If the acid doesn’t have oxygen add the prefix hydro- change the suffix -ide to -ic acid HCl H 2 S HCN
  76. 76. Formulas for acids Working backwards from names. If it has hydro- in the name it has no oxygen Anion ends in -ide No hydro, anion ends in -ate or -ite (and it is an oxyacid) Write anion and add enough H to balance the charges.
  77. 77. Figure 2.25 Flowchart for Naming Acids pp
  78. 78. Formulas for acids hydrofluoric acid dichromic acid carbonic acid hydrophosphoric acid hypofluorous acid perchloric acid phosphorous acid
  79. 79. Hydrates Some salts trap water crystals when they form crystals. These are hydrates. Both the name and the formula need to indicate how many water molecules are trapped. In the name we add the word hydrate with a prefix that tells us how many water molecules.
  80. 80. Hydrates pp In the formula you put a dot and then write the number of molecules. Calcium chloride dihydrate = CaCl 2  2  Chromium (III) nitrate hexahydrate = Cr(NO 3 ) 3  6H 2 O