2. Chapter 4 Atomic Structure Hingham High School Mr. Clune

3. History of the atom  Not the history of atom, but the idea of the atom.  Original idea Ancient Greece (400 B.C.)  Democritus and Leucippus- Greek philosophers.

4. Democritus’s Atomic Theory  Atoms are indivisible and indestructible.

5. History of Atom  Looked at beach  Made of sand  Cut sand - smaller sand n Smallest possible piece? n Atoms - not to be cut

6. Another Greek  Aristotle - Famous philosopher  All substances are made of 4 elements  Fire - Hot  Air - light  Earth - cool, heavy  Water - wet  Blend these in different proportions to get all substances

7. Who’s Next?  Late 1700’s - John Dalton- England.  Teacher- summarized results of his experiments and those of others.  Dalton’s Atomic Theory  Combined ideas of elements with that of atoms.

8. John Dalton (1766-1844)

9. Dalton 1803

10. Dalton’s Atomic Theory  All matter is made of tiny indivisible particles called atoms.  Atoms of the same element are identical, those of different atoms are different.  Atoms of different elements combine in whole number ratios to form compounds.  Chemical reactions involve the rearrangement of atoms. No new atoms are created or destroyed.

11. Just How Small Is an Atom?  Think of cutting a piece of lead into smaller and smaller pieces  How far can it be cut?  An atom is the smallest particle of an element that retains the properties of that element

12. Homework Section Assessment Page: 103 1 – 7 Due: 10/19/04

13. Section 4.2 Structure of the Nuclear Atom  OBJECTIVES: –Distinguish among protons, electrons, and neutrons in terms of relative mass and charge.

14. Section 5.2 Structure of the Nuclear Atom  OBJECTIVES: –Describe the structure of an atom, including the location of the protons, electrons, and neutrons with respect to the nucleus.

15. Parts of Atoms  J. J. Thomson - English physicist. 1897  Made a piece of equipment called a cathode ray tube.  It is a vacuum tube - all the air has been pumped out.

16. J.J. Thompson (1856 – 1940)

17. Thompson 1897

18. Thomson’s Experiment Voltage source +- Vacuum tube Metal Disks

19. Thomson’s Experiment Voltage source +-

20. Thomson’s Experiment Voltage source +-

21. Thomson’s Experiment Voltage source +-

22. n Passing an electric current makes a beam appear to move from the negative to the positive end Thomson’s Experiment Voltage source +-

23. n Passing an electric current makes a beam appear to move from the negative to the positive end Thomson’s Experiment Voltage source +-

24. n Passing an electric current makes a beam appear to move from the negative to the positive end Thomson’s Experiment Voltage source +-

25. n Passing an electric current makes a beam appear to move from the negative to the positive end Thomson’s Experiment Voltage source +-

26. Thomson’s Experiment  By adding an electric field

27. Voltage source Thomson’s Experiment n By adding an electric field + -

28. Voltage source Thomson’s Experiment n By adding an electric field + -

29. Voltage source Thomson’s Experiment n By adding an electric field + -

30. Voltage source Thomson’s Experiment n By adding an electric field + -

31. Voltage source Thomson’s Experiment n By adding an electric field + -

32. Voltage source Thomson’s Experiment n By adding an electric field he found that the moving pieces were negative + -

33. Other particles  Proton - positively charged pieces 1840 times heavier than the electron – by E. Goldstein  Neutron - no charge but the same mass as a proton – by J. Chadwick  Where are the pieces?

34. Ernest Rutherford (1871-1937)

35. Rutherford

36. Rutherford’s experiment  Ernest Rutherford -English physicist. (1910)  Believed in the plum pudding model of the atom (discussed in Chapter 13).  Wanted to see how big they are.  Used radioactivity.  Alpha particles - positively charged pieces- helium atoms minus electrons  Shot them at gold foil which can be made a few atoms thick.

37. Rutherford’s experiment  When an alpha particle hits a fluorescent screen, it glows.  Here’s what it looked like (page 111)

38. Lead block Uranium Gold Foil Fluorescent Screen

39. He Expected  The alpha particles to pass through without changing direction very much.  Because…?  …the positive charges were thought to be spread out evenly. Alone they were not enough to stop the alpha particles.

40. What he expected

41. Because

42. He thought the mass was evenly distributed in the atom

43. Since he thought the mass was evenly distributed in the atom

44. What he got

45. How he explained it +  Atom is mostly empty.  Small dense, positive piece at center.  Alpha particles are deflected by it if they get close enough.

46. +

47. Density and the Atom  Since most of the particles went through, it was mostly empty space.  Because the pieces turned so much, the positive pieces were heavy.  Small volume, big mass, big density.  This small dense positive area is the nucleus.

48. Subatomic particles – p.106 Electron Proton Neutron NameSymbolCharge Relative mass Actual mass (g) e-e- p+p+ n0n0 +1 0 1/1840 1 1 9.11 x 10 -28 1.67 x 10 -24

49. Homework Section Assessment Page: 108 8-14 Due: 10/20/04

50. The Periodic Table: Organizing the Elements  OBJECTIVES: –Identify the position of groups, periods, and the transition metals in the periodic table.

51. Counting the Pieces  Atomic Number = number of protons in the nucleus  # of protons determines kind of atom (since all protons are alike!)  the same as the number of electrons in the neutral atom.  Mass Number = the number of protons + neutrons.  These account for most of mass

52. Symbols  Contain the symbol of the element, the mass number and the atomic number. X Mass Number Atomic Number

53. Protons, Neutrons and Electrons p + = Atomic Number -n 0 = Atomic Number Atomic Mass e - = p +

54.  Find the –Mass Number –Atomic Number –number of protons –number of neutrons –number of electrons F 19 9 p + = 9 e - = 9 n 0 = 19 - 9=10

55. n Find the –Mass Number –Atomic number –number of protons –number of neutrons –number of electrons Br 80 35 p + = 35e - = 35 n 0 = 80 – 35 = 45

56. Symbols n if an element has an atomic number of 34 and a mass number of 78 what is the –number of protons –number of neutrons –number of electrons –Complete symbol p + = 34 n 0 = 78 – 34 = 44 e - = 34 Se

57. n if an element has 91 protons and 140 neutrons what is the –Atomic number –Mass number –number of electrons –Complete symbol At # = 91 Mass # = 91+140 231 e - = 91 Pr

58. n if an element has 78 electrons and 117 neutrons what is the –Atomic number –Mass number –number of protons –Complete symbol At # = 78 Mass # =78+117 195 p + = 78 Pt

59. Isotopes  Dalton was wrong.  Atoms of the same element can have different numbers of neutrons.  different mass numbers.  called isotopes.

60. Isotopes Atoms of the same element with different number of neutrons. 1P + 2N 1e- Tritium Average Atomic Mass for H = 1.00794 1P + 1N 1e- Deuterium 1P + 0N 1e- Protium

61. Naming Isotopes  We can also put the mass number after the name of the element.  carbon- 12  carbon -14  uranium-235

62. Atomic Mass  How heavy is an atom of oxygen? –There are different kinds of oxygen atoms.  More concerned with average atomic mass.  Based on abundance of each element in nature.  Don’t use grams because the numbers would be too small.

63. Measuring Atomic Mass  Unit is the Atomic Mass Unit (amu)  One twelfth the mass of a carbon-12 atom.  Each isotope has its own atomic mass, thus we determine the average from percent abundance.

64. Calculating averages  Multiply the atomic mass of each isotope by it’s abundance (expressed as a decimal), then add the results.  Sample Problem – Page 117

65. Atomic Mass #23 Calculate the atomic mass of copper if copper has two isotopes. 69.2% has a mass of 62.93 amu and the rest has a mass of 64.93 amu.

66. Atomic Mass #23 69.2% of 62.93 amu (100% - 69.2%) of 64.93 amu.692 X 62.93 amu = 43.55 amu.308 X 64.93 amu = 20.00 amu + 63.55 amu

67. Atomic Mass #24 Calculate the atomic mass of bromine. The two isotopes of bromine have atomic masses and relative abundance of 78.92 amu (50.69%) and 80.92 amu (49.31%).

68. Atomic Mass #24 50.69% of 78.92 amu 49.31% of 80.92 amu 49.31% of 80.92 amu.5069 X 78.92 amu = 40.00 amu.4931 X 80.92 amu = 39.90 amu + 79.90 amu

69. Atomic Mass  Magnesium has three isotopes. 78.99% magnesium 24 with a mass of 23.9850 amu, 10.00% magnesium 25 with a mass of 24.9858 amu, and the rest magnesium 25 with a mass of 25.9826 amu. What is the atomic mass of magnesium?  If not told otherwise, the mass of the isotope is the mass number in amu

70. Atomic Mass  Is not a whole number because it is an average.  are the decimal numbers on the periodic table.

71. Development of the Periodic Table  mid-1800s, about 70 elements  Dmitri Mendeleev – Russian chemist  Arranged elements in order of increasing atomic mass  Thus, the first “Periodic Table”

72. Dimitri Mendeleev

73. Mendeleev Periodic Table

75. Mendeleev  Left blanks for undiscovered elements  When discovered, good prediction  Problems? –Co and Ni; Ar and K; Te and I

76. New way  Henry Moseley – British physicist  Arranged elements according to increasing atomic number  The arrangement today  Symbol, atomic number & mass

77. Henry Moseley

78. Periodic table  Horizontal rows = periods –There are 7 periods  Periodic law:  Vertical column = group (or family) –Similar physical & chemical prop. –Identified by number & letter

79. Areas of the periodic table  Group A elements = representative elements –Wide range of phys & chem prop. –Metals: electrical conductors, have luster, ductile, malleable

80. Groups of Elements The vertical columns in the Periodic Table. Elements in each group have similar properties.

81. Groups of Elements Example: Group 11 Copper Silver Gold

82. Metals  Group IA – alkali metals  Group 2A – alkaline earth metals  Transition metals and Inner transition metals – Group B  All metals are solids at room temperature, except _____.

83. Nonmetals  Nonmetals: generally nonlustrous, poor conductors of electricity –Some gases (O, N, Cl); some are brittle solids (S); one is a fuming dark red liquid (Br)  Group 7A – halogens  Group 0 – noble gases

84. Division between metal & nonmetal  Heavy, stair-step line  Metalloids border the line –Properties intermediate between metals and nonmetals  Learn the general behavior and trends of the elements, instead of memorizing each element property

85. Metals Transition Elements Non- Metals Metalloids Halogens Noble Gases Alkali Metals Alkaline Earth Metals

86. Homework Review Sheets 4.1 and 4.2 Due: 10/27/04 4.31 Due: 10/28/04 Test: 10/29/04

87. Dc 102 50