2. Chapter 2 Atoms, Molecules, and Ions

3. History n Greeks n Democritus and Leucippus - atomos n Aristotle- elements. n Alchemy n 1660 - Robert Boyle- experimental definition of element. n Lavoisier- Father of modern chemistry. n He wrote the book.

4. Laws n Conservation of Mass n Law of Definite Proportion- compounds have a constant composition. n The react in specific ratios by mass. n 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.

5. What?! n Water has 8 g of oxygen per g of hydrogen. n Hydrogen peroxide has 16 g of oxygen per g of hydrogen. n 16/8 = 2/1 n Small whole number ratios.

6. Proof n Mercury has two oxides. One is 96.2 % mercury by mass, the other is 92.6 % mercury by mass. n Show that these compounds follow the law of multiple proportion. n Speculate on the formula of the two oxides.

7. Dalton’s Atomic Theory 1) Elements are made up of atoms 2) Atoms of each element are identical. Atoms of different elements are different. 3) Compounds are formed when atoms combine. Each compound has a specific number and kinds of atom. 4) Chemical reactions are rearrangement of atoms. Atoms are not created or destroyed.

8. n Gay-Lussac- under the same conditions of temperature and pressure, compounds always react in whole number ratios by volume. n Avagadro- interpreted that to mean n at the same temperature and pressure, equal volumes of gas contain the same number of particles. n (called Avagadro’s Hypothesis) A Helpful Observation

9. Experiments to determine what an atom was n J. J. Thomson- used Cathode ray tubes

10. Thomson’s Experiment Voltage source +-

11. Thomson’s Experiment Voltage source +-

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

13. Thomson’s Experiment n By adding an electric field

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

15. Thomsom’s Model n Found the electron. n Couldn’t find positive (for a while). n Said the atom was like plum pudding. n A bunch of positive stuff, with the electrons able to be removed.

16. Millikan’s Experiment Oil Atomizer Oil droplets Telescope - +

17. Millikan’s Experiment X-rays X-rays give some electrons a charge.

18. 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

19. Radioactivity n Discovered by accident n Bequerel n Three types –alpha- helium nucleus (+2 charge, large mass) –beta- high speed electron –gamma- high energy light

20. Rutherford’s Experiment n Used uranium to produce alpha particles. n Aimed alpha particles at gold foil by drilling hole in lead block. n Since the mass is evenly distributed in gold atoms alpha particles should go straight through. n Used gold foil because it could be made atoms thin.

21. Lead block Uranium Gold Foil Florescent Screen

22. What he expected

23. Because

24. Because, he thought the mass was evenly distributed in the atom.

25. What he got

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

27. +

28. Modern View n The atom is mostly empty space. n Two regions n Nucleus- protons and neutrons. n Electron cloud- region where you might find an electron.

29. Sub-atomic Particles n Z - atomic number = number of protons determines type of atom. n A - mass number = number of protons + neutrons. n Number of protons = number of electrons if neutral.

30. Symbols X A Z Na 23 11

31. Chemical Bonds n The forces that hold atoms together. n Covalent bonding - sharing electrons. n Makes molecules. n Chemical formula- the number and type of atoms in a molecule. n C 2 H 6 - 2 carbon atoms, 6 hydrogen atoms, n Structural formula shows the connections, but not necessarily the shape.

32. H H HH H HCC n There are also other model that attempt to show three dimensional shape. n Ball and stick.

33. Ions n Atoms or groups of atoms with a charge. n Cations- positive ions - get by losing electrons(s). n Anions- negative ions - get by gaining electron(s). n Ionic bonding- held together by the opposite charges. n Ionic solids are called salts.

34. Polyatomic Ions n Groups of atoms that have a charge. n Yes, you have to memorize them. n List on page 62

35. Periodic Table

36. Metals n Conductors n Lose electrons n Malleable and ductile

37. Nonmetals n Brittle n Gain electrons n Covalent bonds

38. Semi-metals or Metalloids

39. Alkali Metals

40. Alkaline Earth Metals

41. Halogens

42. Transition metals

43. Noble Gases

44. Inner Transition Metals

45. +1+2-2-3

46. Naming compounds n Two types n Ionic - metal and non metal or polyatomics. n Covalent- nonmetal and nonmetal

47. Ionic compounds Metal bonded to Nonmetal n Name the metal (CATION) first –Use a (Roman Numeral) for transition metals, tin, lead –If polyatomic- name it n If the ANION is monatomic- change the ending to -ide – If poly atomic- just name it n practice

48. Ionic Compounds n Cation: know what charged ions possible n Anion: charge from table, or from memory n CaS nK2SnK2SnK2SnK2S n AlPO 4 n K 2 SO 4 n FeS n CoI 3

49. Ionic Compounds n Fe 2 (C 2 O 4 ) n MgO n MnO n KMnO 4 n NH 4 NO 3 n Hg 2 Cl 2 n Cr 2 O 3

50. Ionic Compounds n KClO 4 n NaClO 3 n YBrO 2 n Cr(ClO) 6

51. Naming Covalent Compounds n Nonmetal bonded to nonmetal; covalent; use Prefixes! n mono, di, tri, tetra, penta, hexa, septa, nona, deca n First element name with the appropriate prefix (except mono) n Second element, -ide ending with appropriate prefix n Practice

52. n CO 2 n CO n CCl 4 nN2O4nN2O4nN2O4nN2O4 n XeF 6 nN4O4nN4O4nN4O4nN4O4 n P 2 O 10 Naming Covalent Compounds

53. Writing Formulas n Two sets of rules, ionic and covalent n To decide which to use, decide what the first word is. n If is a metal or polyatomic use ionic. n If it is a non-metal use covalent.

54. Ionic Formulas n Charges must add up to zero. n Get charges from table, name of metal ion, or memorized from the list. n Use parenthesis to indicate multiple polyatomics.

55. Ionic Formulas n Sodium nitride n sodium- Na is always +1 n nitride - ide tells you it comes from the table n nitride is N -3

56. Ionic Formulas n Doesn’t add up to zero. n Must cross the charges to get net zero Na +1 N -3 Na N 1 3 Na 3 N

57. Mixed practice: Write the formula n sulfur dioxide n sodium sulfite n calcium iodide n lead (II) oxide n nitrogen trichloride n lead (IV) oxide n mercury (I) sulfide

58. Mixed Practice cont’d n diflourine monoxide n barium chromate n aluminum hydrogen sulfate n cerium (IV) nitrite n diphosphorus pentoxide

59. Acids n Substances that produce H + ions when dissolved in water. n All acids begin with H. n H + oxygen containing ion = oxyacids –ATE ions make IC acids »“I ate it and got sick” –ITE ions make OUS acids »“It’s a’ite wi’ us”

60. Naming acids n Watch out for sulfuric and sulfurous n H 2 CrO 4 n HMnO 4 n HNO 2

61. Naming acids n H + monatomic anion = binary acids n add the prefix hydro- n change the suffix -ide to -ic acid hydro---------ic acid n HCl nH2SnH2SnH2SnH2S n HCN

62. Formulas for acids n Write H first n Write anion and add enough H to balance the charges.

63. Write the formulas n hydrofluoric acid n dichromic acid n carbonic acid n hydrophosphoric acid n hypofluorous acid n perchloric acid n phosphorous acid

64. Hydrates n Some salts trap water crystals when they form crystals. n These are hydrates. n Both the name and the formula needs to indicate how many water molecules are trapped. n In the name we add the word hydrate with a prefix that tells us how many water molecules.

65. Hydrates n In the formula you put a dot and then write the number of molecules. Calcium chloride dihydrate = CaCl 2  2  Calcium chloride dihydrate = CaCl 2  2  Chromium (III) nitrate hexahydrate = Cr(NO 3 ) 3  6H 2 O Chromium (III) nitrate hexahydrate = Cr(NO 3 ) 3  6H 2 O