Quantum Mechanics Review Sheet
Basic Quantum Questions (p. 101-116 and my typed notes/lecture):
1. What are the 4 quantum numbers? (in other words, what 4 letters represent them?)
2. What do each one of the quantum numbers tell you about the position of an electron?
3. What are the letters which represent the four basic sublevels?
4. How many orbitals can be found in each one of the sublevels?
5. How many electrons can be found in each one of the sublevels?
6. How many electrons can be found in one orbital? It doesn’t matter which orbital.
7. How do you determine the maximum number of electrons which can be held in any given energy level?
8. Quantum number l (“el”) has a maximum value for each energy level. How do you determine the maximum value for l (“el”) for an energy level? (look at my typed notes).
9. What is the maximum value for l (“el”) if you have an atom with 3 energy levels?
10. Write out the numerical values for l (“el”) and write the corresponding sublevel next to these values. (look at my typed notes if you don’t know them.)
11. What are the numerical values of m for the different sublevels? Write them out.
12. What are the two possible values for the quantum number s? What do these values represent?
13. Re-copy the periodic table I drew in class which indicates the order in which the energy levels, sublevels and orbitals fill.
Finding the electron in an atom if given the four quantum numbers: Given the following sets of four quantum numbers, draw the SINGULAR electron arrow configuration: (just write the energy level, sublevel and orbital with 1 arrow on it)
14. n = 1, l = 0, m = 0, s = +1/2 16. n = 3, l = 2, m = 2, s = +1/2
15. n = 2, l = 0, m = 0, s = -1/2 17. n = 4, l = 3, m = -2, s = -1/2
What element is described by these electron configurations?
18. [Ar] 4s2 20. [Ne] 3s2 3p5
19. [Xe] 6s2 4f14 5d6 21. [Rn] 7s2 6d1 5f7
Electron configurations – Sometimes called Electron Arrow Configurations
Draw out the electron configuration for the following elements: For numbers 22-25, use arrow configurations. For numbers 26-30, use the noble gas which precedes the element and then continue with the shorthand version (e.g. [Ne] 3s1 would be the correct answer for Na – see p. 111 table 4-4 to see what I mean)
22. N 24. V 26. W 28. Hf 30. Ag (careful)
23. Ca 25. Cr (careful) 27. U 29. Cu (careful)
The Periodic Table and its arrangement (p. 128-139):
31. Elements in the same horizontal row are in the same ___________.
32. Elements in the same vertical row are called __________
33. Elements in the same horizontal row have what one thing in common?
34. Elements in the same vertical row have what one thing in common?
35. Which elements are in the Alkali group? Give an important property (p. 132 & 728).
36. Which elements are in the Alkaline Earth Metals? Give a property (p. 132 & 734).
37. Which elements are in the Halogen group? Give an important property (137 & 780).
38. Which elements are in the Noble gas group? Give an important property (p. 125-126)
39. What is the ionic charge on any halogen ion?
40. What is the ionic charge on any Alkali metal ion?
41. What is the ionic charge on any Alkaline Earth Metal ion?
42. Where on the periodic table would you find the metal elements?
43. Name the 8 metalloid elements from the periodic table.
44. Name at least 3 non-metals
45. Look at page 22-24 and describe the basic characteristics of the following: Metals, Metalloids, Non-metals and Noble Gases. (Yes, page 22-24)
46. True or False: Metals tend to give up electrons easily and form a positive ion.
47. What period (number) do the Lanthanide series belong? (p. 126)
48. What period (number) do the Actinide series belong? (p. 126)
Looking at periodic table trends (p. 140-154):
49. The atomic radius increases or decreases as you go from left to right on the chart? Why?
50. The atomic radius increases or decreases as you go down a group on the chart? Why?
51. What is the definition of ionization energy?
52. What is the difference between and ion and a regular old atom (this is an easy question! Don’t get hung up on it!). What is the ion of Na. What is it of N?
53. The first ionization energy for an atom increases or decreases as you go from left to right on the chart? Why?
54. The first ionization energy for an atom increases or decreases as you go down a group on the chart? Why?
55. What element has the highest ionization energy? Why? Which the lowest. Why?
56. True or False: As a general rule, an element with a VERY low ionization energy will be quite reactive (explosive) with either water or maybe even air.
57. True or False: The second ionization energy is always lower than the first ionization energy.
58. Which element in the Alkali group will have the lowest first ionization energy?
59. As you go from left to right on the chart, do the ions of the atoms increase in size or decrease? Why? (you will need to differentiate between Cations and Anions)
60. As you go down a group on the chart, do the ions of the atoms increase in size or decrease? Why?
61. Which is positive and which is negative – Cation and Anion
62. Copy a rough sketch of figure 5-16 on p. 144. Why do He, Ne and Ar have the highest ionization energy while Li, Na and K have the lowest?
How to review for a test on Quantum:
1. Read through my typed notes and have the notes you took for those next to you as you read (for example, in class I drew diagrams to go along with the typed notes – you should have these diagrams in your notes). Be sure you understand what the notes are saying in relation to the diagrams you drew.
2. Read through the answers to the Quantum Mechanics Review Sheet. Be sure that you read the pages in the textbook that I mention on the review sheet and on the typed notes. Have a friend quiz you about some of these questions. The textbook is good at explaining and showing diagrams. Read those pages that I mentioned in the notes and on this review sheet.