2. Which scientist studied glowing metals and discovered that only certain wavelengths of light are emitted at each specific temperature & represented a certain energy that is quantized?

3. What happens to electrons in the photoelectric effect, when light of a minimum frequency hits a metal surface?

4. In order to explain the photoelectric effect, light behavior can be described as a ___________

5. Who proposed that LIGHT has a dual wave-particle nature?

6. Which model of the atom is pictured below?

7. Which element did the Bohr Model explained the line- emission spectrum?

8. How many colors of the visible spectrum are seen in hydrogen’s line-emission spectrum?

9. Describe the Bohr Model of the atom.

10. What rule/principle is not being followed in the following orbital notation?:

11. Who proposed that LIGHT (and all ER) has a dual wave-particle nature?

12. What is the lowest value for the principal quantum number?_______ highest?_______

13. What is meant by the Dual Wave- Particle Nature of Light/Electrons?

14. _______ is radiation moving at the speed of light; a form of energy that exhibits wavelike behavior as it travels through space.

15. Who explained the photoelectric effect?

16. How many electrons are contained in a full second main energy level?

17. ____________ is a three dimensional region around the nucleus that indicates the probable location of an electron. (fuzzy electron clouds)

18. Which scientist studied glowing metals and discovered that only certain wavelengths of light are emitted at each specific temperature & represented a certain energy?

19. Who developed the quantum mechanical model that treated electrons in atoms as waves & helps determine probable electron location in an atom?

20. _________ is a discrete “packet” of energy that can be gained or lost by an atom _________ is a discrete “packet” of energy that can be gained or lost by an atom

21. What model is illustrated?

22. List one Property that all ER has in common.

23. In the following, 1s 2 2s 2 2p 5, how many orbitals only have one electron?

24. Why do we see different colors during a flame test?

25. What quantum number indicates the spatial orientation of the orbital about the nucleus in which an electron is located?

26. How many quantum numbers is each electron given?

27. What is the lowest principal quantum number that an electron can have?

28. What quantum number Indicates the main energy level that the electron is found?

29. ______ is a general term for any type of energy that emanates or radiates outward in all directions

30. What quantum number indicates the shape of the orbital in which an electron is located?

31. What letters represent sublevels?

32. No two electrons in the same atom can have the same four quantum numbers (two electrons of opposite spin can occupy the same orbital) is known as what?

33. In the following 2s 1, what does the 1 represent?

34. What model was used to ONLY explain hydrogen’s line-emission spectrum and no other element?

35. An electron occupies the lowest- energy orbital that can receive it is known as what?

36. A______________________is a particle of electromagnetic radiation with no rest mass that carries a quantum of energy.

37. What quantum number indicates the spin of electron on its own axis?

38. How many orbitals does a f sublevel have?

39. All the forms of electromagnetic radiation are called the _______

40. _______specifies the properties of the atomic orbitals and the properties of electrons in those orbitals

41. What is the maximum number of electrons in a “s” sublevel?

42. What is the maximum number of electrons contained in an orbital?

43. How many orbitals does a “d” sublevel have?

44. ______ is the lowest state of energy for an electron

45. What is the maximum number of electrons contained in a “d” sublevel?

46. Explain what happens when an electron drops from a higher energy state to a lower energy state.

47. List two examples of ER

48. All electrons in singly occupied orbitals must have the same spin is known as what?

49. In the following, 1s 2 2s 2 2p 6 3s 1, what atom is represented?

50. In the following, 1s 2 2s 2 2p 5, how many unpaired electrons are present?

51. In the following 2s 1, what does the 2 represent?

52. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron is known as what?

53. In the following 2s 1, what does the s represent?

54. What is the maximum number of electrons contained in a “p” sublevel?

55. The state in which an electron has a higher potential energy than it has in its ground state is the __________

56. How many orbitals does a “p” sublevel have?

57. In the following, 1s 2 2s 2 2p 6, how many electrons are present in the highest main energy level?

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