1. Electron Structure and Periodic Trends

2. 1. Wavelength is… A. the height of the wave
B. the length of the entire wave as it travels through space
C. the distance between two adjacent points on the wave
D. Number of waves that pass a point in 1 second.
E. large when the frequency of a wave is large.

3. 2. Which of the following forms of light has the longest wavelength?
A. Microwaves
B. UV
C. Radio
D. Infrared
E. Visible

4. 3. Which of the following forms of light has the highest frequency?
A. Micro
B. UV
C. Radio
D. Infrared
E. Visible

5. 4. What color of visible light has the longest wavelength?
A. Violet
B. Blue
C. Green
D. Yellow
E. Red

6. 5. At which point on the wave below is the frequency the highest?

7. 6. Arrange the following in order of DECREASING wavelength:
A. X-ray, Infrared, UV, radio
B. Radio, UV, Infrared, X-ray
C. UV, Infrared, Radio, X-ray
D. Radio, X-ray, Infrared, UV
E. Radio, Infrared, UV, X-ray

8. 7. What color of visible light has the highest frequency?
A. Violet
B. Blue
C. Green
D. Yellow
E. Red

9. 8. When white light passes through a prism/ diffraction grating…
A. it tends to speed up faster than 3 x 108 m/s.
B. it splits into a continuous range of colored wavelengths making up visible light.
C. it splits into distinct bands of light.
D. it splits into all forms of light EXCEPT visible light.
E. it remains white because the prism can’t affect light.

10. 9. A line emission spectrum for an excited element…
A. consists of lines of different colors.
B. is different for each element.
C. occurs because photons of certain wavelengths are released by the atoms.
D. Indicates that electrons in atoms can make specific energy-level jumps and falls.
E. All of the above

11. 10. When do excited electrons emit light?
A. when they jump from ground state to excited state
B. when they fall from excited state back to ground state

12. 11. When an excited electron falls back to its original energy level, what is given off?
A. A proton
B. A neutron
C. A photon
D. An electron
E. A sublevel

13. 12. Draw the orbital diagram of nitrogen
___ ____ ___ ___ ___ ___ ___ ___ ___ 1s 2s 2p 3s 3p

14. 13. Which sublevel can hold the LEAST number of electrons?
B. p
C. d
D. f

15. 11. An electron can form a spherical shaped region when it is a/an ___ orbital.
A. d
B. p
C. s
D. f

16. 12. The number of orbitals in any p sublevel is…
C. 3
D. 4

17. 13. The maximum number of electrons that any d sublevel can hold is…

18. 14. The electron configuration for Al is
A. 1s22s22p9
B. 1s22s22p63p5
C. 1s22s22p63s23p1
D. 1s22s22p83p1
E. 1s22s22p63p3

19. 15. The electron configuration for Si is
1s22s22p63s4
1s22s22p63s23p4
1s22s22p63s23p2
1s22s22p63p4
1s22s22p63s24p2

20. 16. The electron configuration for O is
2s22p4
1s22s22p23s2
1s22s42p4
1s22s22p4
1s22s6

21. 17. 4p3 would be the sublevel notation for which element?
A. As
B. Rb
C. Na
D. N
E. Xe

22. 18. Final configuration for 5s1?
A. As
B. Rb
C. Na
D. N
E. Xe

23. 19. Final configuration for 3s1?
A. As
B. Rb
C. Na
D. N
E. Xe

24. 20. Final configuration for 5p6?
A. As
B. Rb
C. Na
D. N
E. Xe

25. 21. [Ar] 4s23d6 is which element?
A. Chromium
B. Iron
C. Krypton
D. Calcium
E. Zinc

26. 22. The element that begins filling the 6s sublevel is
A. lithium
B. Rubidium
C. Cesium
D. Scandium
E. Barium

27. 23. What is the maximum number of electrons the d sublevel can hold?

28. 24. What’s wrong with this configuration
24. What’s wrong with this configuration? Explain AND choose… 1s22s22p63s33p4
Aufbau
Pauli Exclusion Principle
Hund’s Rule
Roy G. Biv Principle

29. 25. What are the trends? (increases or decreases)
AR=______________ AR= ______________

30. 26. What are the trends? (increases or decreases)
IE = _______________ IE = ________________

31. 27. What are the trends? (increases or decreases)
EN= ____________ EN = ____________________

32. 28. The atomic radius of oxygen is larger than that of
A. Li
B. S
C. F
D. B

33. 29. Which has the greatest ionization energy?
A. C
B. Si
C. Ge
D. Sn
E. Pb

34. 30. Which has the smallest electronegativity?
A. C
B. Si
C. Cl
D. F
E. Rb

35. 31. Elements in Group 17 will have how many valence electrons?8 9
It varies depending on the element.

36. 32. How many valence electrons does gallium (Ga) have?1 13 2 31 3

37. 33. Blue light has a wavelength of 453 nm
33. Blue light has a wavelength of 453 nm. Which wavelength best represents red light?
A nm
B nm
C nm

38. 34. What group has the highest ionization energy?
B. 2
C. 16
D. 17
E. 18

39. 35. Draw a Lewis Dot structure for phosphorus:

40. 36. Draw a Lewis Dot structure for carbon:

41. 37. T or F?
Orbitals can hold more than 2 electrons.

42. 38. T or F?
Electrons spin in the same direction in each orbital.

43. 39. T or F?
Large atoms are easy to take electrons from.

44. 40. T or F?
Pauli Exclusion Principle tells us that 2 electrons can fit in an orbital but must have opposite spin.

45. 41. T or F?
Blue flames from a bunsen burner have less energy than the yellow luminous flames of a camp fire.

46. 42. T or F?
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