1. ATOMIC THEORY REVIEW

2. Where did the elements come from? Hydrogen, a little helium and less lithium were created in the big bang. The universe is about 95% hydrogen. Clouds of hydrogen gas and dust are compressed by gravity into stars. When the star's core runs out of hydrogen, the nuclear reaction pauses, and gravity compresses the star, heating it up enough to fuse helium.

3. Where did the elements come from?  If the star is big enough, like a supernova, it can eventually create all the elements in the periodic table up to iron. If a giant star explodes as a supernova, it will releases enough energy to make all the elements heavier than iron. So stars created the first elements!

4. The most common Elements in the Earth’s CRUST ElementAmount Oxygen46.1 % Silicon28.2 % Aluminum8.23 % Iron5.63 % Calcium4.15 %

5. The most common Elements in the Earth’s OCEANS ElementAmount Oxygen85.84 % Hydrogen10.82 % Chlorine1.94 % Sodium1.08 % Magnesium0.1292 %

6. The most common Elements in the Earth’s ATMOSPHERE ElementAmount Nitrogen78.1 % Oxygen20.9 % Argon0.96 %

7. ATOMS !!! What are the 3 subatomic particles? Protons Neutrons Electrons What is ALL matter made of?

8. Subatomic Particle Charges protons (+) positive neutrons (0) neutral electrons (-) negative We know that there are the same number of p + and e - in atoms on the Periodic Table… So What is the overall charge of any atom? The overall charge of any atom is NEUTRAL… the positive charge cancels out the negative charge = 0!!!

9. What are the masses (amu) of the subatomic particles? p + = 1amu n = 1amu e - = 0 amu 1.66 x 10 -27 kg = 1 amu What is this AMU stuff????? Atomic mass unit (AMU) 2.2 lbs= 1 kg

10. What are the two areas of an atom? Nucleus and electron cloud P + & N o e-

11. Where are the p+, n, and e- located in an atom? p+ in the nucleus n o in the nucleus e- in the electron cloud

12. Nucleus Where is ALL the mass in an atom located? Where is most of the volume of an atom located? Electron Cloud

13. The nucleus contains the p+ and n… while the electrons “orbit” the nucleus in the energy rings of the e- cloud. What does a Bohr model of the atom look like?

14. So what are the charges of the different areas? 1. So what is the overall charge of the nucleus? Positive 2. So what is the overall charge of the electron cloud? Negative (opposite charges attract)

15. QUICK REVIEW- ATOMS Sub-atomic particles:. particleschargeamulocationabbrev. Protons Electrons e- Neutral (0) +p+nucleus 0 1 1 neutrons Electron cloud _ nucleusnono protons, neutrons, and electrons nucleus and electron cloudParts of the atom:

16. Energy Levels of the Atom 8 e- 2e- 32e- 8 e- 18 e- 18 e- 32e- The Nucleus P+ N 0 1 st shell 7 th shell 2 nd shell 3 rd shell 4 th shell 5 th shell 6 th shell Atoms can have several energy levels. Sometimes they are also called energy rings, shells or orbits.

17. Lets take a look at the Periodic Table! The periods equal the number of energy shells or rings in an atom.

18. Beginning with Bohr Models  Let’s try a few easy bohr models: Li Be

19. Bohr Model Practice 1. Ca 2. O 3. Ne 4. K 5. Rb 6. P 7. F 8. Cl 9. Br 10. I

20. More Bohr Model Practice 11. Fr 12. Te 13. Sn 14. Cs 15. Kr 16. At 17. Ga 18. Rn 19. Ag 20. W

21. CsFrSnTeKr At GaRnW Ag

22. Bohr Model Hvs.He Explain why we use helium filled balloons instead hydrogen filled balloons at Parties. Hydrogen is unstable and flammable and helium is stable! Energy rings are not filled Energy rings are filled Draw the bohr models for the following atoms.

23. Burning Hindenburg

24. Complete the Bohr Models for the following elements. Ne, Ar, Kr and Xe  What 4 patterns or trends did you notice they have in common?  “Predict” what you think Radon’s (Rn) bohr model would look like.  Six rings  Full shell  More massive  All of the rings or shell are full.  They are all in the same group (18)  They gain an energy ring as you go down a period.  They gain more subatomic particles as you go down.

25. Patterns from the Bohr Models. Ne Ar Kr Xe Radon Bohr Model

26. Even More Bohr Model Practice! 21. Os 22. Hf 23. Cm 24. Sr 25. Ho 26. Tc 27. Ac 28. Zr 29. Po 30. Np

27. “Life on the Edge” with Valence Electrons Valence electrons are electrons in the outermost shell of an atom. They determine whether the atom will bond with another atom. How many valence electrons does lithium have here? 1 valence electron Circle the valence electrons From your warm up. Valence electrons are electrons in the outermost shell of an atom. They determine whether the atom will bond with another atom. How many valence electrons does lithium have here? 1 valence electron Circle the valence electrons From your warm up.

28. Arrangement of the Periodic Table 1. What atom is this? Oxygen 2. Which subatomic “particle” helped you to determine that this Bohr model was of oxygen? Protons

29. Arrangement of the Periodic Table 1. The periodic table is arranged according to what? A. Atomic Symbol B. Atomic mass C. Atomic number D. Number of Energy Shells  Do the elements on the periodic table all increase according to their masses?  No !! Can you find where they are not? There are a few of them. Look carefully!

30. Periodic Table Card Sort Poster Breaking the Code Purpose : This lesson will help you identify many of the patterns that are contained in the periodic table of elements. Use the card sort poster to answer the following questions on your paper.

31. Do you notice any patterns here as the elements move to the right? Li NaK Rb Can you “predict” how many energy rings a bohr model of Francium (Fr) would have? Gaining more mass Gaining more energy rings Gaining more p+, n o, and e-.

32. Francium (Fr) Bohr Model Seven energy rings 1 valence electron

33. What Bohr model patterns are you starting to see develop?  Periodic Table Patterns  The atomic number is the same number as the number of protons and electrons.  Atoms get larger as you move down and two the right on the periodic table.  As you move from left to right on the periodic table, you gain protons and electrons and neutrons.  As you go down from the periodic table, the atom gains another energy shell or orbit.

34. ElementAtomic Number Atomic Mass # of Protons # of Electrons # of Neutrons Zn 3065 Xe 5477 Au 79118 Hg 80121 I 12753 30 54 197 8020180 79 54 131 3035 3053 79

35. Manganese First Energy Level: 2 Second Energy Level: 8 Third Energy Level: 8 Fourth Energy Level: 7 Yttrium First Energy Level: 2 Second Energy Level: 8 Third Energy Level: 8 Fourth Energy Level: 18 Fifth Energy Level: 3 P39 N50 2e8e 18e 3e P25 N30 2e8e 7e Yttrium Manganese

36. Krypton First Energy Level: 2 Second Energy Level: 8 Third Energy Level: 8 Fourth Energy Level: 18 Germanium First Energy Level: 2 Second Energy Level: 8 Third Energy Level: 8 Fourth Energy Level: 14 Krypton Germanium P36 N48 2e8e 18e P39 N50 2e8e 14e

37. Metals vs. Non-Metals Metals Non-metals Man made elements and Rare Earth metals Stair steps

38. Metalloids on the Periodic Table FAMILIES/ GROUPS Periods/ Rows Metalloids

39. Properties of Metals  Most elements are metals. 88 elements to the left of the stairstep line are metals or metal-like elements.  Tend to have Luster  High density  Ductile  Malleable (shininess) (heavy for their size) (most metals can be made into thin wires) (most metals can be hammered into thin sheets)

40. Properties of Non-metals  Nonmetals are found to the right of the stairstep line.  No luster  Brittle  Not ductile  Not malleable (dull) (breaks easily)

41. Properties of Metalloids  Metalloids are elements on both sides of the stair step line. They have properties of both metals and nonmetals.  Solids  Can be shiny or dull  Ductile  Malleable

42. Families on the Periodic Table

43. So where do the names come from? Iron (Fe)………….……Ferrum Sodium (Na)….. …….Natrium Gold (Au)……………Aurum Silver (Ag)………….Argentum Potassium (K)………… Kalium Copper (Cu) ………….Cuprum Mercury (Hg) ……Hydragyrum Antimony (Sb)………… Stibium Tin(Sn)….………… Stannum Lead(Pb) ……………..Plumbum Tungsten(W)………….Wolfran These abbreviations are for there LATIN names of the elements.

44. Steps for creating a bohr model 1. Complete the particle inventory for the atom (protons, electrons and neutrons). 2.Draw your nucleus. 3. Put the number of protons and neutrons in the nucleus. 4. Circle how many electrons you need to use in the shells. 5. Know how many electrons and shells you will need. 6. Put 2 electrons in the first shell. If there are more than 2, begin to fill the next shell (maximum of 8). 7. You cannot begin to fill the next shell until the previous shell is filled. 8. Remember` how many electrons each shell can hold a maximum of. (2, 8, 8, 18, 18, 32, 32,)