1. Atomic Structure

2. The Atom Smallest form of an element that that elements properties stillretains Basic building Made of:  Protons  Neutrons  Electrons blockofmatter

3. TheAtom Composed of:  Nucleus  Electron Cloud

4. TheNucleus Positively charged Protons and neutrons  Protons – positively charged  Neutrons – neutrally charged  Neutrons act like glue

5. TheElectrons Negatively charged Occupy the “Electron cloud” surrounding the nucleus Arranged into shells or orbitals Electrons are NOT moving in perfect orbits around the nucleus. The electron movement is unpredictable Cloud gives us approximate location of where electrons are

7. SubatomicParticles LocationChargeMassSpecial Fact ProtonsProtonsNucleusPositive (+)1 amuNumber of protons determines the identity of the element NeutronsNucleusNeutral1 amu ElectronsElectron CloudNegative (-)0.00054 amuElectron cloud takes up 99.9999999% of the volume of the atom

8. PropertiesofAtoms Atomic Number Mass Number Average Atomic Mass

9. INSIDE THE SQUARES…

10. AtomicNumber Number of protons in the nucleus of an atom Each element has its own specific atomic number In a NEUTRAL ATOM, this is also the number of electrons

11. (Average)AtomicMass An average mass of each of the different isotopes found for that element in nature For example, Chlorine has 2 different isotopes Each one has 17 carbons and a different number of neutrons (This is what an isotope If you take the average atomic single carbon atom that exists, the average mass will be 35.453 amu is. More on that later) mass of every

12. MassNumber Mass number is the mass of a SPECIFIC isotope of atom. It is the SUM of the protons and neutrons in the nucleus an Mass Number=(# of neutrons) + (# of protons) Mass Number = Atomic Mass It is not the average unless we say AVERAGE How do we find # of neutrons?

13. . SohowhowdoIknow whatthe MassNumber is? I will tell you.One of two ways: 1) Give you the mass number or the neutrons in a table. PT If I don’t give it to you,gettherounded#offthe 2) Tell you in the symbol A) Isotope Notation: B) Isotope Name: Sodium-23

14. Figuring out some element parts… Element Symbol Atomic # Protons Neutrons Mass # Boron-11 B Carbon -12 6 6 Magnesium-23 12 23 Copper-64 29 35 20

15. Figuring out some element parts… Element Symbol Atomic # Protons Neutrons Mass # Boron-11 B 5 5 6 11 Carbon -12 C 6 6 6 12 Magnesium-23 Mg 12 12 11 23 Copper-64 Cu 29 29 35 64 ? ? ? ? 20 ?

16. Isotopes and Ions

17. Isotopes Isotopes: atoms of that have different neutrons the same numbers element of Two isotopes of an elementwill have the same atomic number, but different massnumbers(and atomic masses) CARBON (above right) 1. What is the mass number to the left? 2. What is the mass number to the right? 3. What is the atomic number to the left? 4. What is the atomic number to the right?

18. Isotope Example So, which of the following representisotopes of the sameelement? #1 234 #2 234 #3 235 #4 238 XXXX 929392 Whichelement are theseisotopes of?

19. IsotopeNotation Write the symbol with number on top and the on the bottom Example: the mass atomic number

20. Isotope Example Naturally occurring carbon consists of three isotopes, 14 N, 15 N, 16 N. andState the number of protons, carbon atoms. 16 N 7 neutrons, 14 N 7 andelectronsin each 15 N 7 ofthese #P #N #E

21. Ions IONS are charged atoms (or groups of atoms) positive or negative charge. Ions differ in the number of electrons For Neutral Atoms : Number of electrons = number of protons For Ions : protons the same, electrons are different Either lost or gained electrons Examples: Neutral Atom: Na, Ca, I, O thathavehavea Ion: Na + Ca +2 I-I- O -2

22. IONS Taking away an electron from an atom gives a positive charge protons becausetherearearenownowmore Called a CATION So if the Mg atom to the right Mg 2+ loses 2 electrons, it becomes

23. IONS Adding an electron to an atom gives a negative charge because there are now Called an ANION moremoreelectrons So if the F atom to the right F-F- gains 1 electron, it becomes

24. Ion Practice State the number these ions. 39 K + 19 ofofprotons, neutrons,andelectrons in eachof 16 O 8 -2 41 Ca 20 +2 #p + #n o #e -

26. Electron Arrangement

27. EnergyLevels Electrons that are closer to nucleus Further So the have lower energy away = Higher energy further away from the nucleus an electron is, the more energy it has The electron cloud is organized into shells. Each shell has a max. number of electrons it can hold

28. # ofElectronsinEachEnergyLevel 1 st 2 nd 3 rd 4 th Level = = 8 e- 2electrons ==== 18 32 e-e-e-e- Electrons must orbital first occupythe lowest energy level or

29. BohrDiagrams Bohr Diagrams show each of the energy levels of the atom Show every electron that the atom has orbiting around it. These electrons are organized orbital levels intothedifferentshellsor 1 st 2 nd 3 rd level - 2 electrons level - 8 electrons level - 18 electrons Examples:

30. BohrDiagrams: YouTryTry Draw metheBohrDiagramof eachofthefollowing: HB FSi

32. ValenceElectrons Electrons in outermost shell = valence electrons Determine the properties of the element Will it bond with other elements? Which ones? Valence electrons tell us the answers.

33. Each column (except for the transition metals) has a set number of valence electrons

34. YOU-TRY! Use the group determine the number above the column to number of valence electrons. 13781378 valence electrons Sodium – (Na) Boron – (B) Chlorine – (Cl) Neon – (Ne)

35. LewisDotDotDiagrams Uses the symbol of the element and dots to represent VALENCE electrons

36. LewisDot:HowHowTo… Write the symbol of the element Figure out how many valence electrons it has Each side of the symbol can only hold 2 electrons 1 dot = 1 electron Each side must get one electron before any side can Max Number = 8 dots for 8 electrons get 2 (You can’t have more than 8 electrons on the outside row)

37. NUCLEAR ENERGY! DAY 1: (RADIATION, FISSION, FUSION)

38. Nucleus Stability  Stability ofthe nucleusdepends on the nuclear forces and neutrons  Protons repel each other  Protons attract neutrons because of the strong nuclear force thatactbetweenbetweenprotons

39. Nucleus Stability  Nuclei with too many are unstable. protons or neutrons  Ifan atom is unstable,it will try to become stable by splitting into  Nuclei with more than 83 protons are ALWAYS unstable twosmalleratoms.

40. Nucleus Stability  Essentially, nuclear stability is basedon the arrangement ofthe protons and neutrons in the nucleus  The more efficient and tightly packed the nucleus orientation is, the more stable the nucleus is

41. FISSION  Fission is the process where a nucleus splits into two or more smaller fragments, releasing neutrons, and energy  Nucleus must be large Ex: Uranium-235 for this to happen Uranium-235 only makes up 0.7% of the Uranium in the world The rest is stable Uranium-238 – The largest naturally occurring element  Done in nuclear power plants and atomic bombs

42. FISSION  Neutrons are used as bullets to break apart the uranium- 235 nucleus.  3 Products form  Fission Products: Barium and Krypton  3 Free Neutrons  Energy is released

43. FISSION: MultiplePathways  There are a multiple pathways for Uranium to decay  The pathway we concentrate on involves Ba and Kr products  In any case, there will always be 3 products, regardless of pathway.  Fission Products  2-3 Free Neutrons  Energy is released

44. Chain Reactions  Chain Reaction: The 3 neutrons that are released from fission start an additional fission reaction in a different U-235 nucleus  This produces more neutrons and repeats.  The process may be controlled (nuclear power plants/submarines) uncontrolled (nuclear weapons).  Video – Chain Reaction with M Traps (3 min)Video – Chain Reaction with M Traps (3

45. Chain Reactions

46. FISSION ENERGY Hahn and Strassman found that the overall mass decreases after the reaction happens.  The missing mass changed into energy  E = mc 2  Energy = mass * speed of light 2  Speed of light = 300,000,000 m/s Sooo…   = mc 2 = (1kg) * (300,000,000m/s) 2 = 90,000,000,000,000,000 Joules = 9x10 16 joules  E E E E E E E E

47. FISSION ENERGY Converting 1 kg of Uranium-235 intoenergy.  = mc 2 = (1kg) * (300,000,000m/s) 2  E E E E E E E E = 90,000,000,000,000,000 = 9x10 16 joules Joules Energy produced burning  E = 31,000,000 joules  E = 3.1 x 10 7 joule 1 kgof coal(not using E = mc 2 )  So: 1kg of Uranium 235, undergoing fission, will produce over 1 trillion times the energy of 1kg of coal being burned Video: Fission Reactions (2Video: Fission Reactions (2 min)  

48. FUSION  Two lighter nucleus  Start with: nuclei combine to form a heavier  2 Hydrogen isotopes  End with with:  1 Helium atom  1 Neutron  Energy (deuteriumandtritium)  Occurs in stars/thesun

49. ENERGY INFUSION A large amount of energy is needed to create very high temperatures so that the isotopes can be hurled at each other and overcome the tendency of positively charged nuclei (the Hydrogen isotopes) to repel each other. This is why FUSION occurs in Stars and our Sun Video – Sun’s Energy (6 Video – Sun’s Energy (6 min)   

50. ARecap  And don’t forgetthat both release energy!

51. ENERGYCOMPARISONS  Finding the elements: Radiation (12 Finding the elements: Radiation (12min)  Starts at 1:44:30…

52. Nuclear Radiation  Radiation:  Emission of energy or particles from an unstable decaying atom

53. Nuclear Radiation  Background radiation:  Radiation that arises naturally radioactive isotopes in the soil from cosmic rays and air from  Continuously exposed to radiation from sun, soil, rocks, plants More than 80% of radiation exposure sources naturalsources: due to natural  You can change your exposure based on many things: Air travel, where you live, smoking, x rays, job, etc…

54. Nuclear Radiation  Radiation c omes in 3 Alpha particles Beta particle Gamma particle forms:

55. NUCLEAR ENERGY! DAY 2: (USES, PROS, CONS)

56. Ways WeUse NuclearEnergy  Nuclear Medicine Weapons Power  Nuclear power plants  Nuclear submarines

57. Nuclear Medicines Nuclear Medicine: The use of radioactive substances in the diagnosis or treatment of diseases POSITIVE:  Check body systems to make sure working properly  Radiopharmaceuticals are taken orally and then a “gamma camera” captures images of emitted radiation from inside body  Nuclear Medicine Therapy- Intravenous or oral administered drug  Used to treat conditions such as hyperthyroidism, thyroid cancer, and blood disorders

58. Nuclear Medicines Nuclear Medicine: The use of radioactive substances in the diagnosis or treatment of diseases NEGATIVE:  Produces mild radiation, so it can damage/cause cancer in healthy cells  Nuclear waste must be stored  VERY expensive to set up in a facility

59. Nuclear Weapons This is a “Uncontrolled Fission Reaction” Tremendous amounts of energy available from small amounts of fuel  can be “smuggled easily.” Tremendous amount of destruction Contamination of the environment for very long amounts time   of Video: Top 10 explosions ever http://www.youtube.com/watch?v=yRRGaxx8Zf4http://www.youtube.com/watch?v=yRRGaxx8Zf4 (4 min) Video: Effects of a nuclear bomb http://www.youtube.com/watch?v=Aza-http://www.youtube.com/watch?v=Aza- 2wopCFY (42wopCFY (4 minutes) Video: Time lapse of every nuclear explosion ever http://www.youtube.com/watch?v=gJe7fY-yowk (5http://www.youtube.com/watch?v=gJe7fY-yowk (5 min)   

60. Nuclear Weapons

61. Nuclear Reactor: HowItItWorks

62. Nuclear Reactor: This isa Controlled Nuclear FissionReaction

63. Nuclear Reactor: This isa Controlled Nuclear FissionReaction

64. Nuclear Reactor: Howititworks Video (5 min) http://www.youtube.com/watch?v=PKNbwcIaGnghttp://w.youtube.com/watch?v=PKNbwcIaGng

65. Nuclear Energy in 4 easy steps:  1) A Fission chain reaction begins while the fuel rods are in the water  The amount of fission is controlled by lead Control Rods  2)  3) The water heats up and changes to steam steam turns a turbine  4)Theturbine turns a generator, forming electricity  The steam is then cooled down in a cooling tower  The spent fuel rods need to be stored for hundreds/thousands of years

66. Nuclear Energy:  Used Fuel Rods

67. Nuclear Energy: Where AreTheyThey  65 Nuclear Power Plants in the United States  Produce 19.6% of our energy (2008)  SC has 4 plants, producing over ½ of our energy

68. Nuclear Energy BENEFITS  Tremendous amounts of energy available from small amounts of fuel  No air pollution of greenhouse gasses from the burning of fossil fuels  Can be used anywhere  Abundance of fuel  Non-reliance on fossil fuel

69. NUCLEAR ENERGY NEGATIVES:  Can cause thermal pollution to water systems (if you put the water back into rivers) hot  Waste must be stored until can be a very long time. it isno longer radioactive–  Improper handling of nuclear materials  Power plant failure – radioactive explosions  Fukushima Explained - http://www.youtube.com/watch?v=rBvUtY0PfB8 (5 min)http://www.youtube.com/watch?v=rBvUtY0PfB8 (5