2. The Atom Chapters 4-5

3. Atomic Theories Democritus ~ 400 BC believed that atoms were indivisible and indestructible Dalton ~ 1800’s Developed through experiments First Atomic Model

4. Dalton’s Atomic Model All elements are composed of tiny indivisible particles called atoms Atoms of the same element are identical. The atoms of any one element are different from those of any other element.

5. Dalton’s Atomic Model (cont) Atoms of different elements can physically mix together or can chemically combine in simple whole-number ratios to form compounds. Chemical reactions occur when atoms are separated, joined, or rearranged. Atoms of one element, however, are never changed into atoms of another element as a result of a chemical reaction.

6. Discovery of Electron 1897 – JJ Thomson, using cathode ray tube, discovered negatively charged particles called electrons 1909 – Robert Millikan - Oil Drop Experiment Determined charge on an electron.

7. “Plum Pudding” Model Uniform positive sphere with negatively charged electrons embedded within.

8. Radiation Late 1800’s – discovery of radiation Three Types Alpha Beta Gamma

9. Rutherford Gold Foil Experiment - 1909 Shot alpha particles at gold foil Most went through foil with little or no deflection. Some were deflected at large angle and some straight back. A.K.A. Geiger Marsden Experiment

10. Rutherford Gold Foil Experiment - 1909

11. Rutherford Model Conclusions from Gold Foil Experiment Atom is Mostly Empty Space Dense positive nucleus Electrons moving randomly around nucleus

13. Subatomic Particles Electron Discovered in 1897 by JJ Thomson Negative charge (-1) Mass = 9.109389*10 -28 g Approx mass ~ 0 Found outside of nucleus

14. Subatomic Particles Proton Discovered in 1919 by Rutherford Positive charge (+1) Mass = 1.672623*10 -24 g Approx mass ~ 1 atomic mass unit (u) Found inside nucleus

15. Subatomic Particles Neutron Discovered in 1932 by James Chadwick No charge (0) Mass = 1.6749286*10 -24 g Approx mass ~ 1 atomic mass unit (u) Just slightly larger than a proton Found inside nucleus

16. Atomic Structure Atoms have no net charge # of electrons = # of protons # of electrons around nucleus = # of protons in nucleus

17. Atomic Structure Atomic Number Number of protons in an element All atoms of the same element have the same number of protons Mass Number Number of protons and neutrons in an atom

18. Atomic Structure # of Neutrons = Mass Number – Atomic Number Atoms of the same elements can have different numbers of neutrons Isotope – atoms of the same element with different number of neutrons

19. Chemical Symbols Cl-35 Chlorine-35 Mass Number Atomic Number

20. Ion Atom or group of atoms that have gained or lost one or more electrons Have a charge Example: H +, Ca 2+, Cl -, OH -

21. Ions H + 1 proton0 electrons Ca 2+ 20 protons18 electrons Cl - 17 protons18 electrons OH - 9 protons10 electrons

23. Atomic Theories Rutherford’s model could not explain the chemical properties of elements Niels Bohr believed Rutherford’s model needed to be improved Bohr proposed that electrons are found only in circular paths around the nucleus

24. Bohr Model Dense positive nucleus Electrons in specified circular paths, called energy levels These energy levels gave results in agreement with experiments for the hydrogen atom.

25. Bohr Model

26. Each energy level can only hold up to a certain number of electrons Level 1  2 electrons Level 2  8 electrons Level 3  18 electrons Level 4  32 electrons

27. Electron Configuration The way in which electrons are arranged in the atom Example: Na 2-8-1 Valence Electrons Electrons in the outermost energy level

28. Wave Mechanical Model More detailed view of the Bohr Model Schrödinger Wave Equation and Heisenberg Uncertainty provides region of high probability where electron COULD be. Orbital Modern Model AKA Quantum Mechanical Model, Electron Cloud Model

29. Wave Mechanical Model Orbital Regions of space where there is a high probability of finding an electron

31. M&M’s Demo What colors are found in a regular M&M’s bag? Green Yellow Orange Blue Red Brown

32. M&M’s Demo Do you get an equal amount of each color in each bag? If we opened up all the regular M&M bags in the world would we get an equal number of each color? Are you supposed to?

33. M&M’s Demo Color1 bagWorld Blue%24% Green%16% Yellow%14% Orange%20% Red%13% Brown%13%

34. M&M’s Demo M&M’s come in certain abundances (percentages) So do isotopes of each element Relative Abundance Percent of each naturally occurring isotope found in nature

35. Average Atomic Mass Atomic Mass Weighted average based on the relative abundance and mass number for all naturally occurring isotopes Example C-1298.9%12.011u C-131.1%

36. Atomic Mass C-1298.9% C-131.1% Carbon = 0.989*12 + 0.011*13 = 12.011u