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Unit 3: Atomic Structure
Name: _________________________
Text Questions from Corwin
Ch. 5
1. How did the views of Democritus and Aristotle disagree with regard to matter?
5.1
2. What did Dalton offer for his ideas about the atom, which set him apart from the Greek thinkers?
3. Besides Boyle’s experiments, what two other principles did Dalton employ in his model of the atom?
4. Of Dalton’s five statements about the atom, which two do we NOT believe in today? State those two.
5.2
5. Thomson’s model of the atom was of a positively charged atom containing…
6. What were two popular names given to Thomson’s model?
5.3
7. What did Rutherford conclude about WHY most of the alpha particles passed through the foil?
8. What two things did Rutherford reason about the nucleus?
9. Describe the model of the atom that Rutherford proposed in 1911.
10. The size of an atom compared to the size of its nucleus is similar to…
11. About how many years passed between Rutherford’s work and the discovery of the neutron?
5.4
12. What is the difference between the atomic number and the mass number?
13. Write out a generic atomic notation, and identify all of the terms.
14. What are isotopes?
5.5
15. What is an atomic mass unit equal to?
16. Define atomic mass.
17. What two things are needed to calculate an element’s atomic mass?
18. The atomic mass of carbon is ______ amu, but no carbon atom weighs this amount. A carbon atom
weighs either ________ amu or ________ amu. The atomic mass of carbon represents the mass of a
____________________ average carbon atom.
19. From the periodic table, how can you identify the elements that are radioactive?
5.6
20. Wavelength refers to…
21. Frequency refers to…
22. What is the relationship between frequency and wavelength?
23. What is the relationship between frequency and energy?
24. What is the range of wavelengths that constitutes the visible spectrum?
25. How do the wavelengths of ultraviolet radiation and infrared radiation compare to visible wavelengths?
26. The continuous spectrum is also called the…
27. List at least four types of radiant energy that make up the continuous spectrum.
5.7
28. What did Max Planck propose in 1900?
29. Although radiant energy has a ________ nature, it also has a _____________ nature.
30. What is a photon?
31. With reference to Figure 5.10… The quantum concept of energy is analogous to the ball losing potential
energy as it travels down the _________.
5.8
32. Bohr proposed that electrons orbit the nucleus just as…
33. What two things did Bohr suggest about electron orbits?
34. According to Bohr, an energy level is…
35. According to Bohr, electrons could be found only in ________ energy levels and __________ ______.
36. The paper that Bohr received: What did it show?
37. An __________ spectrum is emitted when a gas is excited by an electrical ________. The gas, which is
sealed in a ____________ tube, emits light that can be separated into a ________ of narrow _____
when passed through a ________.
38. Bohr realized that the emission spectrum of hydrogen was experimental _____________ to support his
model of the atom.
39. In a hydrogen discharge tube, excited H atoms have electrons in a _____ energy orbit. Because this is
an _________ state, the electron _______ to a lower level. In doing so, the electron ______ a definite
amount of energy; this corresponds to a ________ of light energy. The energy of the ________ is
_________ to the energy ______ by the electron as it ________ to a lower energy level.
40. How many photons are emitted when a single electron drops to a lower energy level?
41. What did the further study of emission spectra reveal?
42. This “atomic fingerprint” indicated that…
43. In 1895 – 27 years after it was discovered to exist in the Sun – where ELSE was helium found?
5.9
44. Could Bohr explain the spectra of other elements, besides hydrogen?
45. Within a main energy level, Bohr suggested the idea of…
46. Write the designations – AND what the designations stand for – for the four types of energy sublevels.
47. The type of sublevel determines what?
48. How many electrons can the following sublevels hold?
s
p
d
49. Compared to those closer to the nucleus, electrons farther from the nucleus occupy…
f
5.10
50. List the first twelve sublevels, in order of increasing energy.
51. What is an electron configuration?
52. First, the __________ is written, followed by _____________ indicating…
53. For a given element, WHAT corresponds to the number of electrons in a neutral atom?
54. For neutral atoms, the ____ of the _______________ equals the ________ _________ of the element.
5.11
55. Why was it desirable that a more powerful atomic theory emerge in the 1920s?
56. What did Heisenberg state, in his uncertainty principal?
57. The more accurately the position of an electron is known…
58. Following Bohr’s model, the quantum mechanical model retained WHAT, but incorporated what ELSE?
59. How is the energy of an electron described, in the quantum mechanical model?
60. What is an orbital?
61. The shape of an s orbital is that of a _________. A p orbital is shaped like a __________.
62. Although all s orbitals are _____________, they are NOT all the same _____. Similarly, all of the
___________-shaped p orbitals are NOT the same _____.