1. How many electrons occupy the 2p orbitals in atoms where 2p orbitals are completely filled?
   1. 1
   2. 2
   3. 3
   4. 6
   5. 10

2. A Na lamp emits yellow light with a wavelength of 589 nm. What is the energy of a single photon in this light?
   1. 3.37 x 10^-19 Joules.
   2. 1.12 x 10^-25 Joules.
   3. 1.17 x 10^-33 Joules.
   4. 5.09 x 10¹⁵ Joules.
   5. 5.09 x 10¹⁴ Joules.

3. Which of the following is a possible electron configuration?
   1. 1s²2s³2p⁶
   2. 1s²2s¹2p⁷
   3. 1s²2s²2p⁶3s²3p⁸3d⁷
   4. 1s²2s²2p⁶3s²3d¹²
   5. 1s²2s²2p⁶3s¹3d⁹

4. In all the following pairs, the element and electron configuration are correctly matched EXCEPT for:

   (a)	1s22s22p63s2	Mg
   (b)	1s22s22p63s23p1	Al
   (c)	1s22s22p5	F
   (d)	1s22s22p63s23p64s23d6	Co
   (e)	1s22s22p63s23p64s23d2	Ti

5. The energy associated with the transition of an electron from the n=1 state to the n=3 state of H atoms is:
   1. +1.74 x 10^-17 Joules.
   2. +1.94 x 10^-18 Joules.
   3. -1.94 x 10^-18 Joules.
   4. -1.74 x 10^-17 Joules.
   5. none of these

6. Which of the following is a permissible set of quantum numbers for an electron in a hydrogen atom?

   	n	l	ml
   (a)	1	0	-1
   (b)	2	1	+1
   (c)	2	1	+2
   (d)	3	3	0
   (e)	4	2	-3

7. The number of distinct emission spectral lines that originate from electron transitions between the first four energy levels in a hydrogen atom is:
   
   1. 3.
   2. 4.
   3. 6.
   4. 9.
   5. 16.
   The next three questions refer to the photoelectric loss of an electron from metallic Li which requires light of 5.51 x 10¹⁴ s^-1 frequency.

8. The energy for loss of an electron from a metallic Li atom is:
   1. 1.20 x 10^-48 Joules.
   2. 6.62 x 10^-34 Joules.
   3. 3.65 x 10^-19 Joules.
   4. 5.51 x 10^-14 Joules.
   5. none of these

9. The wavelength (in nm) corresponding to the above frequency is:
   1. 300 nm
   2. 333 nm
   3. 544 nm
   4. 551 nm
   5. none of these

10. The maximum kinetic energy (in J) of an electron removed from a Li atom by light of 6.51 x 10¹⁵ s^-1 frequency is:
    1. 4.67 x 10^-18 Joules.
    2. 4.31 x 10^-18 Joules.
    3. 3.95 x 10^-18 Joules.
    4. 0.365 x 10^-18 Joules.
    5. none of these

11. The electron has:
    1. a negative charge, and much smaller mass than a proton.
    2. a negative charge, and the same mass as a proton.
    3. no wavelike properties.
    4. none of the above.

12. The velocity (s), frequency (f), and wavelength (w) of light are related by:
    1. s = f/w
    2. s = fw
    3. s = f²w
    4. s = w/f
    5. none of the above

13. Which of the following subatomic particles is responsible for the majority of chemical reactivity of an element or compound?
    1. proton
    2. electron
    3. neutron
    4. atomic mass number
    5. photon

14. Which of the following is not a type of electromagnetic radiation?
    1. red light
    2. sound waves
    3. x-rays
    4. photon
    5. ultraviolet radiation

15. By use of a suitable filter, the green mercury emission line can be isolated. This line has a wavelength of 546.1 nm. What is the frequency? [1 Hz = 1 s^-1]
    1. 5.490 x 10¹⁴ Hz
    2. 1.820 x 10⁴ Hz
    3. 1.640 x 10² Hz
    4. 5.461 x 10^-7 Hz
    5. 1.820 x 10^-13 Hz

16. When you sunbathe, it is important to use sunscreen to protect you from the harmful cancer causing ability of ultraviolet light waves. Yet, many home bathrooms have infrared light fixtures to help warm the room, and this light is not cancer causing. In class, we discussed that this is the case because:
    1. the amplitudes of these two types of waves are different.
    2. the frequency of infrared light is higher.
    3. the wavelength of UV light is longer.
    4. the energy of UV light is greater.
    5. the temperature of the IR light.

17. Thompson's raisin pudding model (or plum pudding) of the structure of atoms was not an adequate description because:
    1. it did not account for the existence of electrons.
    2. it did not account for the existence of protons.
    3. it required electrons to move in fixed circular orbits.
    4. it said that atoms were spheres of positive charge with electrons embedded.
    5. all of the above.

18. Which of the following is a postulate of the Bohr model of the atom that the Schroedinger model refutes?
    1. The energy of an electron is quantized, in other words there are only certain allowed energies for an electron.
    2. The electron in a hydrogen atom travels around the nucleus in a circular orbit.
    3. All electrons have exactly the same amount of energy at constant temperature.
    4. Schroedinger agreed with all of the above Bohr postulates.

19. The shape of a 2s orbital resembles:
    1. a hockey puck.
    2. an (American) football.
    3. an ellipse.
    4. a sphere.
    5. a square.

20. Which orbital of the following has a principal quantum number of 3 and an angular momentum quantum number of 2?
    1. 3s
    2. 3d
    3. 4f
    4. 3f
    5. 2p

21. Which of the orbitals in the previous question cannot exist?
    1. 3s
    2. 3d
    3. 4f
    4. 3f
    5. 2p

22. What is the maximum number of electrons that can be placed in the 3d subshell?
    1. 5
    2. 2
    3. 3
    4. 1
    5. 10

23. The shape of a 2p orbital resembles:
    1. a hockey puck.
    2. two (American) footballs, placed end-to-end.
    3. a circle.
    4. a sphere.
    5. a square.

24. Which orbital of the following has a principal quantum number of 2 and an angular momentum quantum number of 1?
    1. 2s
    2. 2d
    3. 4f
    4. 3d
    5. 2p

25. Which of the orbitals in the previous question cannot exist?
    1. 2s
    2. 2d
    3. 4f
    4. 3d
    5. 2p

26. What is the maximum number of electrons that can be placed in the 4d subshell?
    1. 5
    2. 2
    3. 3
    4. 1
    5. 10

27. Calculate the wavelength of light that corresponds to the radiation that is given off during the transition of an electron from the n = 2 to n = 5 of the state of the hydrogen atom.
    1. 434 nm
    2. 305 nm
    3. 275 nm
    4. 183 nm
    5. not enough info is given

28. Which of the following has the highest energy?
    1. gamma rays
    2. X-rays
    3. ultra-violet radiation
    4. infrared radiation
    5. radio waves

29. Which of the following sets of quantum numbers specify a valence electron in the Br atom?

    	n	l	ml	ms
    (a)	4	0	0	+1/2
    (b)	4	1	-1	+1/2
    (c)	4	1	0	-1/2
    (d)	4	1	1	+1/2
    (e)	all of the above

30. Which most closely represents the shape of a 3p orbital?
    

31. Which of the following atoms has an electron with the following quantum numbers when the atom is in its lowest energy configuration?
    n = 2, l = 2, m_l = 1, m_s = -1/2
    1. He
    2. Li
    3. C
    4. Si
    5. none of the above

32. The electron in an excited hydrogen atom emits a photon of wavelength 9.72 x 10^-8 m when it relaxes to its ground state (n=1). What is the electron's assigned energy level in that excited state?
    1. 2
    2. 3
    3. 4
    4. 6
    5. 8

33. It takes 495.8 kJ/mol of energy to ionize sodium. What frequency (s^-1) and wavelength (nm) of light would be required to ionize sodium?

    	frequency (s-1)	wavelength (nm)
    (a)	7.48 x 1038	241
    (b)	1.24 x 1015	2.41 x 104
    (c)	1.24 x 1015	241
    (d)	7.48 x 1038	3.95 x 10-22
    (e)	none of the above

34. A hydrogen atom in an excited state emits 950.4 Angstrom radiation as its electron returns to the ground state. In which excited state was the electron?
    1. first excited state
    2. second excited state
    3. third excited state
    4. fourth excited state
    5. fifth excited state

35. Below are several principles or concepts and matching descriptions. Which answer correctly matches the entries in the two columns?

    principle	description
    1. Heisenberg Uncertainty Principle	a. Bodies can lose energy only in quantized amounts.
    2. Pauli Exclusion Principle	b. It is impossible to determine simultaneously the position and speed of a particle with extreme accuracy.
    3. Hund's Rule	c. The electrons in a given atom must differ in the value of at least one of their 4 quantum numbers.
    4. Planck's Hypothesis	d. Electrons fill orbitals with the same energy so that one e- occupies a different orbital before any orbital is occupied by 2 e-.

    1. 1-a, 2-b, 3-c, 4-d
    2. 1-b, 2-c, 3-d, 4-a
    3. 1-b, 2-d, 3-a, 4-c
    4. 1-c, 2-d, 3-a, 4-b
    5. 1-d, 2-c, 3-b, 4-a

36. What is the maximum number of electrons that the shell with n=3 can accommodate?
    1. 8
    2. 16
    3. 18
    4. 24
    5. 32

37. A big success of the Bohr Model was that it explained exactly the frequencies of the four visible lines in the spectrum of hydrogen. These frequencies were known to fit one of the following formulas, in which C was a constant. Which one?
    

38. Which of the following statements about atomic orbitals is false?
    1. There are 3 p-type orbitals.
    2. For s orbitals, there is a high probability that the electron will be found at the nucleus.
    3. A node is where the electron density goes to zero.
    4. All d orbitals have 4 lobes and look like "four leaf clovers".
    5. According to the Pauli principle, all orbitals can hold up to two electrons.

39. The absorption of visible light involves which of the following processes?
    1. protons converted to neutrons
    2. molecules gaining kinetic energy
    3. electrons making the transition from the ground state to a higher energy level
    4. atomic orbitals being hybridized
    5. electrons returning from excited states to the ground state

40. Various values of the quantum numbers ( n, l , m_l , m_s ) are listed below. Which is a possible set of values for one of the d electrons in a Fe atom in its ground state?
    1. (1, 1, 0, 1/2 )
    2. (4, 0, 1, 1/2 )
    3. (4, 1, 0, -1/2 )
    4. (3, 2, 1, -1/2 )
    5. Both (c) and (d) are possible sets.

41. A hydrogen atom in an excited state emits 973.2 Angstrom radiation as its electron returns to the ground state. In which excited state was the electron?
    1. first excited state
    2. second excited state
    3. third excited state
    4. fourth excited state
    5. fifth excited state

42. Which of the following sets of quantum numbers are not allowed for an electron in an atom?
    1. n=1 ; l=1 ; ml=0
    2. n=2 ; l=1 ; ml=+1
    3. n=3 ; l=2 ; ml=0
    4. n=4 ; l=0 ; ml=0
    5. n=7 ; l=6 ; ml=+5

43. How many orbitals are allowed for principal quantum number (n) of 3?
    1. 9
    2. 8
    3. 6
    4. 4
    5. 3

44. Which of the following electron diagrams represent a correct ground state?
    
    1. A
    2. B
    3. C
    4. D
    5. E

45. What feature distinguishes the three degenerate p orbitals?
    1. They can accept different numbers of electrons.
    2. They have different origins.
    3. They have different shaped lobes.
    4. Each lobe points along either the x, y or z axis.

46. Which of the following subshells can accept a maximum of 10 electrons?
    1. 2p
    2. 4f
    3. 3d
    4. 3s
    5. 5f

47. Which of the following orbitals are degenerate in a multielectron atom?
    1. 3d subshell
    2. 3s, 3p, 3d
    3. 1s, 2s
    4. 2d subshell
    5. none of these

48. The quantum number that specifies the way the orbital is oriented in space is:
    1. the electron spin quantum number.
    2. the magnetic quantum number.
    3. the angular momentum quantum number.
    4. the principal quantum number.
    5. Hund's Rule.

49. What is the frequency of yellow light which has a wavelength of 580 nm?
    1. 5.17 x 10^-2 s^-1
    2. 174 s^-1
    3. 2.998 x 10⁸ s^-1
    4. 5.17 x 10¹⁴ s^-1
    5. 1.74 x 10¹⁸ s^-1

50. If it takes 243.4 kJ of energy to break bonds in a Cl₂ molecule, what is the frequency of the energy used to break the bonds?
    1. 3.673 x 10³⁸ s^-1
    2. 2.727 x 10²⁹ s^-1
    3. 3.673 x 10³⁵ s^-1
    4. 8.174 x 10^-31 s^-1
    5. 6.626 x 10^-34 s^-1

51. Which of the following has the largest wavelength?
    1. visible light
    2. x-rays
    3. infrared light
    4. ultraviolet radiation

52. Which of the following statements concerning 2p orbitals is incorrect?
    1. There are 3 degenerate orbitals of different energy.
    2. Each lobe points along either the x, y, or z axis.
    3. They have smaller lobes than the 3p orbitals.
    4. They have the same shape as 3p orbitals.
    5. They can each hold two electrons.

53. Calculate the energy of a photon emitted with a wavelength of 645 nm.
    1. 3.08 x 10^-19 J
    2. 3.08 x 10^-28 J
    3. 4.65 x 10¹⁴ J
    4. 4.65 x 10⁵ J
    5. 4.28 x 10³¹ J

54. Which orbital of the following has a principal quantum number of 3 and an azimuthal quantum number of 2?
    1. 3s
    2. 3d
    3. 4f
    4. 3f
    5. 2p

Answers

1. D
2. A
3. E
4. D
5. B
6. B
7. C
8. C
9. C
10. C
11. A
12. B
13. B
14. B
15. A
16. D
17. D
18. B
19. D
20. B
21. D
22. E
23. B
24. E
25. B
26. E
27. A
28. A
29. E
30. B
31. E
32. C
33. C
34. D
35. B
36. C
37. B
38. D
39. C
40. D
41. C
42. A
43. A
44. D
45. D
46. C
47. A
48. B
49. D
50. A
51. C
52. A
53. A
54. B