1. 9.9 Warm Up Answer the following questions in your lab book: 1.What is all stuff made out of? 2.What is the previous answer made out of? What is the simplest form you can get? 3.Draw an example of it

2. Announcements 9.9 Research Papers turned into back tray 9.9 IRB Paperwork due – make sure it is all attached with a paperclip & handed to me 9.12 Materials & Methods due online 9.19 Journal Check & Experimental Design

3. Warm Up & Atoms http://learn.genetics.utah.edu/content/cells/scale/ So what does an atom really look like? How small is it? http://ed.ted.com/lessons/just-how-small-is-an-atom

4. Group Presentations Explain & expound on one of the atomic theories that led to our understanding of the atom today. Include: the name of the theory the name of the theoryScientist How they came up with the theory (key facts) Diagram or model of their atom

5. Clubs Studying: Independent studying Music is ok Reading or working on assignments Computers – wait for me to get Science Fair ppl finished

6. 9.11 Warm Up – answer the following questions as best as possible 1.Draw a simple Bohr model for one the following atoms: 2.What is the atomic number? 3.What is the atomic mass? 4.How many protons, neutrons & electrons does it have?

7. 1.Draw a simple Bohr model for the following atom: 1.What is the atomic number? Atomic # = 6 2.What is the atomic mass? Atomic mass = 12.011 amu 1.How many protons, neutrons & electrons does it have? P = 6, N = 6, E = 6

8. Announcements 9.9 Research Papers turned into back tray 9.9 IRB Paperwork due – make sure it is all attached with a staple, turn into tray 9.12 Materials & Methods due online 9.19 Journal Check & Experimental Design

9. Scale 1-4 Do you know how to apply an electron dot diagram to C & H atoms? Could you relate it to ionic bonding or covalent bonding?

10. Learning Scale – Structure of Matter 4. I can describe matter and no only the characteristics of the atom but how it relates to other atoms with bonding and properties 3. I can describe matter and the characteristics of an atom 2. I can describe the atom or matter but not how they relate 1. I know about atoms but need to review what it is composed of

11. The Atom… What would happen if your idea of the atom was wrong? Video What would happen if your idea of the atom was wrong? Video Early Greeks - Democritus

12. Make this Data Table ResearcherInstrumentName of Model Sketch of Model Major Discovery/ Idea

13. Modern Atomic Theory  All matter is composed of atoms  Atoms cannot be subdivided, created, or destroyed in ordinary chemical reactions. However, these changes CAN occur in nuclear reactions!  Atoms of an element have a characteristic average mass which is unique to that element.  Atoms of any one element differ in properties from atoms of another element  All matter is composed of atoms  Atoms cannot be subdivided, created, or destroyed in ordinary chemical reactions. However, these changes CAN occur in nuclear reactions!  Atoms of an element have a characteristic average mass which is unique to that element.  Atoms of any one element differ in properties from atoms of another element

14. Dalton Billiard Ball Model All matter is composed of indivisible particles called atoms. All atoms of the same elements are alike. Atoms of different elements different. Compounds are formed by a combination of 2 or more atoms Atoms cannot be created or destroyed

15. Thomsom Video about Cathode Ray Video about Cathode Ray Video on the Explanation of the Plum Pudding Model Video on the Explanation of the Plum Pudding Modelhttp://culturesciences.chimie.ens.fr/node/1230

16. Thomson’s Findings Thomson concluded that the negative charges came from within the atom. A particle smaller than an atom had to exist. The atom was divisible! Thomson called the negatively charged “ corpuscles, ” today known as electrons. Since the gas was known to be neutral, having no charge, he reasoned that there must be positively charged particles in the atom. But he could never find them. But he could never find them.

17. Thomson’s Atomic Model Thomson believed that the electrons were like plums embedded in a positively charged “pudding,” thus it was called the “plum pudding” model.

18. Rutherford’s Gold Foil Experiment  Alpha (  ) particles are helium nuclei  Particles were fired at a thin sheet of gold foil  Particle hits on the detecting screen (film) are recorded

19. Rutherford’s Findings  The nucleus is small  The nucleus is dense  The nucleus is positively charged  Most of the particles passed right through  A few particles were deflected  VERY FEW were greatly deflected Conclusions:

20. This could only mean that the gold atoms in the sheet were mostly open space. Atoms were not a pudding filled with a positively charged material. Rutherford concluded that an atom had a small, dense, positively charged center that repelled his positively charged “ bullets. ” He called the center of the atom the “ nucleus ” The nucleus is tiny compared to the atom as a whole. Rutherford reasoned that all of an atom ’ s positively charged particles were contained in the nucleus. The negatively charged particles were scattered outside the nucleus around the atom ’ s edge.

21. Niels Bohr

22. Bohr Model Orbits for electrons Energy Levels

23. Wave/Cloud Model 1920’s X-Ray Diffraction Noticed electrons behaved like particles & waves Electrons traveled in areas of high probability in areas called ORBITALS or CLOUDS 1932 Chadwick Discovered the neutron

24. Atom Definition Atomic model = consists of a nucleus that contains protons and neutrons, surrounded by a cloudlike region of moving electrons

26. Atomic Particles

29. Atomic Number Atomic number (Z) Atomic number (Z) of an element is the number of protons in the nucleus of each atom of that element.

30. Mass Number Mass number Mass number is the number of protons and neutrons in the nucleus of an isotope. Mass # = p + + n 0

31. Isotopes Isotopes are atoms of the same element having different masses due to varying numbers of neutrons.

32. Atomic Masses Atomic mass Atomic mass is the average of all the naturally occurring isotopes of that element. Carbon = 12.011

33. Mass Number Mass number Mass number is the number of protons and neutrons in the nucleus of an isotope. Mass # = p + + n 0 8818 Arsenic753375 Phosphorus1531 16

34. Drawing the Atom