2. Atomic Models 100 points –Performance Due Friday, February 26th

3. Thomson's Model (Plum Pudding Model) Do I need to represent, electrons, protons, and neutrons? Common mistake: Do not represent positive sphere as being “solid”.

4. Thomson’s Model (Plum Pudding Model)

5. Rutherford's Model Do I need to represent, electrons, protons, and neutrons? Small dense positive nucleus and a lot of empty space. Common mistake- represent protons and neutrons in the nucleus and not enough empty space.

6. Rutherford's Model

7. Bohr Model Do I need to represent, electrons, protons, and neutrons? Bohr models will be of a rare isotope. Common mistake- Groups that choose a larger atom don’t come talk to me about the fourth “shell”.

8. Bohr Model

9. Quantum Mech. Model Do I need to represent, electrons, protons, and neutrons? QMM will need to be of the most common isotope and ion for your element. Choose to represent orbital model or electron cloud model Common Mistake- Don’t ask for help in determine the most common ion or write it on their key. Make sure to clarify whether it the orbital model or electron cloud model on their key or poster.

10. Quantum Mech. Model

11. Key and Poster Key should be able to stand on their own or nicely hang from your model. Information Poster can be hand written or types on 8 by 11 sheet of paper.

12. This is an out of class assignment, however you can come in for this IP and next to build your model. I will have some supplies you can use. You can use the next 10 minutes to plan with your group. Due Friday February 26 th

13. End of Day

14. Key Concept 20: The 3 I’s of Chemistry I dentity- Protons I sotopes- Neutron I ons- Electron

15. I dentity- Protons Each element contains a unique positive charge in their nucleus. Key Concept 21: The number of protons in the nucleus of an atom identifies the element and is known as the element’s atomic number.atomic number

16. All neutral atoms of a particular element have the same number of protons and electrons but the number of neutrons in the nucleus can differ. Key Concept 22: Atoms with the same number of protons but different numbers of neutrons are called isotopes.isotopes 1913 Fredrick Soddy discovered isotopes. “certain elements exist in two or more forms which have different atomic weights but which are indistinguishable chemically.” Isotope- Neutrons

18. Greek Philosophers (cont.) What were the errors in the Dalton’s Atomic Theory?

20. Mass of Atoms One atomic mass unit (amu) is defined as 1/12 th the mass of a carbon-12 atom.atomic mass unit One amu is nearly, but not exactly, equal to one proton and one neutron.

21. Isotopes containing more neutrons have a greater mass. Isotopes have the same chemical behavior. Key Concept 23: The mass number is the sum of the protons and neutrons in the nucleus.mass number Isotope- Neutrons

22. The relative abundance of each isotope is usually constant. Isotope- Neutrons

23. X Atomic Mass Atomic Number Isotope- Neutrons Key Concept 24: Isotope Format Element (X)- Atomic Mass

24. B 11 5 Boron- 11 What is this atom mass?

25. C 12 6 Room # 169429 What is this atom’s mass?

26. c 14 How many neutrons does this atom have?

27. c ? 6 What would this atom’s mass be if it has 7 neutrons?

28. He 4 How many neutrons does this atom have?

29. Key Concept 25: An ion is an atom or bonded group of atoms with a positive or negative charge.ion Ion- Electron

30. Cation – positively charged ion Anion – negatively charged ion Polyatomic Ions “Poly” = many“atomic” = atoms Ion = charged – Polyatomic ion - many atoms bonded together having an overall charge Look at your Periodic Table

32. Li + How many electron does this ion have?

33. Li +1 What type of ion is this?

34. Be +2 How many electron does this ion have?

35. C 4±

36. C -4 What type of ion is this? How many electron does this ion have?

37. Ca +2 How many electron does this ion have?

38. F -

39. The Basics The Foundations The Building Blocks of Chemistry Call It Whatever You Want They Are Must Knows

40. You must be able to: Read a periodic table and use to key to determine: Understand isotope format: lithium-6 verse lithium-7 6 Li 7 Li Understand how to write ions: Na 1+ Fe 2+

41. 1.What is my name? 2.What is my atomic number? 3.What is my average atomic mass? 4.(Pick one of my isotopes on the left side of the card). What is the atomic mass of that particular atom? 5. How many protons do I have (in the isotope)? 6. How many neutrons do I have (in isotope)? 7. How many electrons do I have if I am neutral(in isotope)? 8.(Pick an ion of the right side of the card) How many protons and electrons do I have? 9.(Consider that I am the previous chosen isotope in question 4 and a neutral atom) What happens to me if I gain a p+ (I become _________.) n o ( I become _________.) e- ( I become _________.) 10. What happens to me if I lose a p+ (I become _________.) n o ( I become _________.) e- ( I become _________.)

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43. Mass of Atoms (cont.) Key Concept 26: The average atomic mass of an element is the weighted average mass of the isotopes of that element.average atomic mass

44. Practice Problems Key Concept 27: The four isotopes of lead and its abundances are: Pb-204, 1.37%; Pb-206, 26.26%; Pb-207, 20.82%; and Pb-208, 51.55%. Calculate lead’s approximate atomic mass.

45. Practice Problems Key Concept 28: Calculate the estimated average atomic mass of neon if neon exists naturally as 90.92% neon-20, 0.257% neon-21, and 8.82% neon-22.

46. Misconception There is only one type of carbon atom There is only one type of carbon atom

47. Ground-State Electron Configuration (cont.)

48. Noble gas notation uses noble gas symbols in brackets to shorten inner electron configurations of other elements.

49. Now Lets Practice

50. Write the Nobel Gas Configuration for the following: Calcium Aluminum Bromine

51. Valence Electrons Key Concept 29: Valence electrons are defined as electrons in the atom’s outermost orbitals—those associated with the atom’s highest principal energy level.Key Concept 29: Valence electrons

52. Circle Valence Electrons Calcium Aluminum Bromine

53. Valence Electrons Key Concept 30: Electron-dot structure (Lewis Structure) consists of the element’s symbol representing the nucleus, surrounded by dots representing the element’s valence electrons.Key Concept 30: Electron-dot structure

54. Lewis Structure Calcium Aluminum Bromine

55. Valence Electrons (cont.)

56. Key Concept 30: Now Lets Practice

57. Identify the number of valence electrons and draw their Lewis Structure Magnesium Argon

58. Draw their Lewis Structure Phosphorus Iodine

59. Valence Electrons The number of valence electrons and the dot structure follow a pattern based on which column the element is in