1. Atoms, Molecules and Ions Chapter 2

2. Foundations of Atomic Theory Law of conservation of mass: Antoine Lavoisier –Mass is neither created nor destroyed. The total mass of a compound must be the same as the total mass of individual elements. Law of definite composition: Joseph Proust –a chemical compound contains the same elements in exactly the same proportions by mass regardless of the size of the sample or source of the compound HgO  Hg + O 433.2 g 401.2g + 32g Sugar: 42.1 % Carbon 51.4 % Oxygen 6.5 % Hydrogen Whether you have a teaspoon or a truckload!

3. 8 X 2 Y 16 X8 Y +

4. Law of multiple proportions: John Dalton –Applies to different compounds made from the same elements –The mass ratio for one of the elements that combines with a fixed mass of the other element can be expressed as a whole number ratio. H 2 O H 2 O 2 WaterPeroxide 2g H 2g H 16g O 1:2 Ratio 32g O

5. 2

6. Dalton’s Atomic Theory (1808) 1. Elements are composed of extremely small particles called atoms. All atoms of a given element are identical, having the same size, mass and chemical properties. The atoms of one element are different from the atoms of all other elements. 2. Compounds are composed of atoms of more than one element. The relative number of atoms of each element in a given compound is always the same. 3. Chemical reactions only involve the rearrangement of atoms. Atoms are not created or destroyed in chemical reactions.

7. J.J. Thomson, measured mass/charge of e - (1906 Nobel Prize in Physics)

8. JJ Thomson’s Cathode Ray Tube Negatively Charged Electrode Positively Charged Electrode

9. Cathode Ray Tube Scientists studied the flow of electric current in a glass vacuum tube with electrodes at each end. When connected to electric current the remaining gas glowed forming a BEAM OF LIGHT. The beam always originated at the NEGATIVE electrode and toward the POSITIVE electrode. The electrode is named by what type of particle it attracts –Cathode: Negative (-) –Anode: Positive (+)

10. 1897 JJ Thomson used magnets to deflect the beam proving that particles had a NEGATIVE CHARGE. Now with the knowledge of electrons, and knowing the atom is neutral, there must be a particle that is positive to balance the negative charge. A small paddle wheel was placed inside and it rolled toward the anode, providing evidence that some PARTICLE MUST BE STRIKING THE WHEEL to make it move.

11. JJ THOMSON DISCOVERED A NEGATIVE PARTICLE CALLED THE ELECTRON!

12. CRT Video

13. Plum Pudding Model

14. Plum PuddingOR Chocolate Chip Cookie

15. Robert A. Millikan Performed the Oil Drop Experiment Determined the exact charge of an electron

16. e - charge = -1.60 x 10 -19 C Thomson’s charge/mass of e - = -1.76 x 10 8 C/g e - mass = 9.10 x 10 -28 g Measured Charge of e - (1923 Nobel Prize in Physics)

17. Oil Drop Experiment Video

18. Radioactivity Becquerel –discovered RADIATION uranium would expose photographic plates in the dark –The properties of an element changed as it gave off radiation Curie –Discovered radium and polonium The radioactive emissions of alpha, beta and gamma rays were identified.

19. (Uranium compound)

21. Ernest Rutherford’s Gold Foil Experiment Set up Gold Foil with a detection sheet around it. Set up radioactive source emitting alpha particles. ALPHA PARTICLES shot at gold foil. MOST particles went through the gold foil SOME particles BOUNCED back

22. Rutherford’s Gold Foil Experiment

23.  particle velocity ~ 1.4 x 10 7 m/s (~5% speed of light) 1.atoms positive charge is concentrated in the nucleus 2.proton (p) has opposite (+) charge of electron (-) 3.mass of p is 1840 x mass of e - (1.67 x 10 -24 g)

24. Gold Foil Conclusions 1.The atom is made up of mostly EMPTY SPACE 2.The center of the atom contains a POSITIVE CHARGE 3.Rutherford called this positive bundle of matter the NUCLEUS

25. Gold Foil Experiment Video

26. Rutherford’s Model of the Atom atomic radius ~ 100 pm = 1 x 10 -10 m nuclear radius ~ 5 x 10 -3 pm = 5 x 10 -15 m

27. Goldstein and Wien - 1886 Cathode Ray Tube with perforated cathode Discovered collection of positively charged particles **DISCOVERED THE PROTON!!

28. Chadwick’s Experiment - 1932 Found that alpha particles shot at beryllium made a beam form The beam had the same mass of a proton but was electrically neutral **DISCOVERED THE NEUTRON!!

29. Chadwick’s Experiment (1932) H atoms - 1 p; He atoms - 2 p mass He/mass H should = 2 measured mass He/mass H = 4  + 9 Be 1 n + 12 C + energy neutron (n) is neutral (charge = 0) n mass ~ p mass = 1.67 x 10 -24 g

30. Niels Bohr – 1913 Developed a new diagram of the atom Electrons can only be at certain energies Electrons must gain a specific amount of energy to move to a higher level, called a quantum **DISCOVERED ENERGY LEVELS!!

31. Bohr’s Model of the Atom

32. Subatomic Particles (Table 2.1) mass p = mass n = 1840 x mass e -

33. Atomic number (Z) = number of protons in nucleus Mass number (A) = number of protons + number of neutrons = atomic number (Z) + number of neutrons Isotopes are atoms of the same element (X) with different numbers of neutrons in their nuclei X A Z H 1 1 H (D) 2 1 H (T) 3 1 U 235 92 U 238 92 Mass Number Atomic Number Element Symbol

35. How many protons, neutrons, and electrons are in C 14 6 ? How many protons, neutrons, and electrons are in C 11 6 ? 6 protons, 8 (14 - 6) neutrons, 6 electrons 6 protons, 5 (11 - 6) neutrons, 6 electrons Do You Understand Isotopes?

36. Period Group

37. A molecule is an aggregate of two or more atoms in a definite arrangement held together by chemical bonds H2H2 H2OH2ONH 3 CH 4 A diatomic molecule contains only two atoms H 2, N 2, O 2, Br 2, HCl, CO A polyatomic molecule contains more than two atoms O 3, H 2 O, NH 3, CH 4

38. An ion is an atom, or group of atoms, that has a net positive or negative charge. cation – ion with a positive charge If a neutral atom loses one or more electrons it becomes a cation. anion – ion with a negative charge If a neutral atom gains one or more electrons it becomes an anion. Na 11 protons 11 electrons Na + 11 protons 10 electrons Cl 17 protons 17 electrons Cl - 17 protons 18 electrons

39. A monatomic ion contains only one atom A polyatomic ion contains more than one atom Na +, Cl -, Ca 2+, O 2-, Al 3+, N 3- OH -, CN -, NH 4 +, NO 3 -

40. 13 protons, 10 (13 – 3) electrons 34 protons, 36 (34 + 2) electrons Do You Understand Ions? How many protons and electrons are in Al 27 13 ? 3+3+ How many protons and electrons are in Se 78 34 2- ?

42. Atomic Mass Unit One atom is the standard – Carbon Mass of other elements are based off of the standard Carbon: 6 p and 6 n = 12 amu 1/12 mass of Carbon atom Periodic table lists weighted average atomic masses of elements (like a GPA calculation) Relative Atomic Mass

43. Calculation AVERAGE Atomic Mass Steps: 1. Percent to decimal 2. Multiply by mass 3. Add it up! 75% 133 Cs 20% 132 Cs 5 % 134 Cs