1. PreAP Chemistry Chapter 3

2. Democritus was the early Greek philosopher who is credited with the concept of the atom (atomos) –which means invisible

3. Law of Definite Proportions states that the elements in a specific compounds always contain the same proportions by mass.

4. Law of Multiple Proportions states that if two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always a ratio of small whole numbers

5. Dalton is an English school teacher who proposed the law of conservation of mass, the law of definite proportions, and the law of multiple proportions.

6. He is also known as the Father of the Atomic Theory

7. Dalton’s atomic theory 1.All matter is composed of very small particles called atoms

8. Dalton’s atomic theory 1.All matter is composed of very small particles called atoms 2.Atoms of a given element are identical in size, mass, and other properties; atoms of different elements differ in these properties.

9. 3.Atoms cannot be subdivided, created, or destroyed

10. 4.Atoms of different elements combine in simple whole-number ratios to form chemical compounds.

11. 3.Atoms cannot be subdivided, created, or destroyed 4.Atoms of different elements combine in simple whole-number ratios to form chemical compounds. 5.In chemical reactions, atoms are combined, separated, or rearranged.

12. Two aspects of Dalton’s atomic theory proven to be incorrect: a.We now know atoms are divisible.

13. Two aspects of Dalton’s atomic theory proven to be incorrect: a.We now know atoms are divisible. b. Atoms of the same element can have different masses.

14. Atom --smallest particle of an element that retains the properties of that element.

15. Two regions of an atom 1.Nucleus -- small region near the center of the atom. Composed of two particles—the proton which is positively charged and the neutron which is neutral (zero) charged.

16. 2. Electron Cloud --composed of negatively charged electrons. It is very large in comparison to the nucleus.

17. Subatomic particles—protons, neutrons, electrons

18. 2. Electron Cloud --composed of negatively charged electrons. It is very large in comparison to the nucleus. Subatomic particles—protons, neutrons, electrons Cathode Ray tubes — the instrument used in the discovery of the electron

20. J. J. Thomson is the man credited with the discovery of the electrons in the late 1800’s

21. Millikan discovered the mass of the electrons

22. Knowledge of electrons led to two inferences about atomic structure: 1.Because atoms are electrically neutral, they must contain positive charge to balance the negative electrons.

23. Knowledge of electrons led to two inferences about atomic structure: 1.Because atoms are electrically neutral, they must contain positive charge to balance the negative electrons. 2.Because electrons have so little mass, atoms must contain other particles to account for most of their mass

24. Nucleus of the atom—discovered by Lord Ernest Rutherford

25. Gold foil experiment—actually done by Hans Geiger and Ernest Marsden

26. Observations: a.Majority of the alpha (α) particles penetrated foil undeflected. b.About 1 in 20,000 were slightly deflected c.About 1 in 20,000 were deflected back to emitter

28. Conclusions: 1. Mass of the atom and the positive charge are concentrated in small regions called nucleus

29. 2. Most of the atom is empty

30. Conclusions: 1. Mass of the atom and the positive charge are concentrated in small regions called nucleus 2.Most of the atom is empty 3.Magnitude of charge on the nucleus is different for different atoms

31. 4.Number of electrons outside the nucleus = number of units of nuclear charge (to account for the fact that the atom is electrically neutral)

32. Atoms are electrically neutral because they contain equal numbers of protons and electrons

33. 1. What kinds of particles are being emitted by the radioactive source? What is their charge?

34. Alpha Particles, positive

35. 2. Toward what are the alpha particles being directed?

36. Gold foil

37. 3.What happens when the charged particles strike the surface of the gold foil?

38. Most go straight through Some were slightly deflected Some were greatly deflected

39. 4.What was the purpose of the fluorescent screen?

40. See where the alpha particles hit

41. 5.What did Rutherford conclude from this gold foil experiment regarding the amount of empty space in the atom? Why was he able to conclude this?

42. Most of the atom is empty space because most of the particles went straight through.

43. 6.How does the deflection path of a charged particle that strikes the center of a gold atom differ from that path of a particle that passes only near the center?

44. If it hits the center it is deflected back to the emitter. If it passes near the center it is slightly deflected.

45. 7.Based on this experiment, where is most of the positive charge and mass of an atom found?

46. Nucleus – in the center

47. 8.What would have been observed if the positive charge of an atom had been thinly spread out throughout the atom?

48. All the alpha particles would have behaved the same – gone straight through.

49. Nuclear Forces the short-range proton- neutron, proton-proton, and neutron- neutron forces that hold the nuclear particles together

50. Mass of one proton = mass of neutron = mass of 1837 electrons

51. Atomic number—the number of protons in the nucleus of the atom.

52. --number of protons identifies the element and is equal to the number of electrons (of a neutral atom) --symbol is Z

53. Isotopes are atoms of the same element that have different masses because they have different numbers of neutrons but they still have similar chemical properties

54. Mass number – approximate atomic mass of an atom (nucleus) -- the number of protons + neutrons

55. Mass Number of Isotope Number of ProtonsNumber of Neutrons 862 963 1064 1165 1266 1367 1468 1569 16610 17611 18612 19613 20614 Isotopes of Carbon

56. Mass Number of Carbon Isotopes Name of Isotopes 8 carbon-8 9 carbon-9 10 carbon-10 11 carbon-11 12 carbon-12 13 carbon-13 14 carbon-14 15 carbon-15 16 carbon-16 17 carbon-17 18 carbon-18 19 carbon-19 20 carbon-20

57. Nuclide is the general term for any isotope of any element

58. Atomic Mass Unit (amu) is exactly 1 / 12 the mass of a carbon-12 atom

59. Average atomic mass is the weight average of the atomic masses of the naturally occurring isotopes of an element. Ave. Atomic mass = %abundace(mass of isotope 1) + %abundance(mass of isotope 2) +…..

60. Moles Mole (mol) is the amount of a substances that contains as many particles as there are atoms in exactly 12 g of carbon-12 (Mole comes from the German word for “pile”)

62. Avogadro’s number – 6.022 ×10 23 – is the number of particles in exactly 1 mole of a pure substance. Just as one dozen = 12 somethings, one mole = 6.022 ×10 23 somethings.

63. The mass of one mole of a pure substance (element or compound) is called the molar mass of that substance. The unit is g mol

64. Mole Review

66. How many grams are in 2.0 mol Carbon?

67. 2.0 mol C

68. How many grams are in 2.0 mol Carbon? 2.0 mol C 1 mol C

69. How many grams are in 2.0 mol Carbon? 2.0 mol C12 g C 1 mol C

70. How many grams are in 2.0 mol Carbon? 2.0 mol C12 g C = 24 g C 1 mol C

71. How many moles are in 0.58 g Al? 0.58 g Al

72. How many moles are in 0.58 g Al? 0.58 g Al 27 g Al

74. How many moles are in 0.58 g Al? 0.58 g Al1 mol Al 27 g Al

75. How many moles are in 0.58 g Al? 0.58 g Al1 mol Al = 0.021 mol Al 27 g Al

76. How many moles are equal to 1.20 x 10 25 atoms of sodium? (Na) 1.20 × 10 25 atom Na

77. How many moles are equal to 1.20 x 10 25 atoms of sodium? (Na) 1.20 × 10 25 atom Na1 mol Na = 19.9 mol Na 6.022 × 10 23 atoms

78. How many atoms are in 0.750 mol of zinc? (Zn)

79. 0.750 mol Zn6.022 × 10 23 = 4.52 × 10 23 atoms Zn 1 mol Zn

80. What is the mass in grams of 4.75 x 10 24 atoms of silver? (Ag)

81. 4.75 × 10 24 atoms Ag1 mol Ag107.9 g Ag = 851 g Ag 6.022 x 10 23 atoms 1 mol Ag

82. What mass of Antimony (SB) contains the same number of atoms as 9.0 g of aluminum?

83. What mass of Antimony (Sb) contains the same number of atoms as 9.0 g of aluminum? 9.0 g Al1 mol Al1 mol Sb122 g Sb = 41 g Sb 27 g Al1 mol Al1 mol Sb