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Chemistry CPA Quarterly 2 Review 2013-2014 School Year
Name: _______________________________ Teacher: _____________________
Atomic Structure:
1. Consider the four postulates of Dalton’s Atomic Theory and determine how each
one compares to the atomic theory we believe is true today.
2. Describe the gold foil experiment and what it accomplished below.
3. Compare and contrast the atom’s size and density with that of its nucleus.
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4. Name the three major sub-atomic particles and give mass, charge and location in
the atom.
Particle
Mass
Charge
Location
5. Identify the following elements: atomic #’s 12,8,17,9
6. What makes it possible to identify elements from only their atomic number?
7. How many protons, neutrons, and electrons are in a neutral atom of argon?
8. For the atom represented by Be-9, indicate:
a. Atomic #
b. Mass #
c. Number of electrons
d. Number of neutrons
9. What is an isotope?
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10. Complete the following table:
Isotope Atomic # Mass #
Protons
H
2
Li
7
14
F-1
neutrons
electrons
Cation/Anion
Neutral?
cation
2
7
7
12
10
19
24
11. Calculate the average atomic mass for the following element:
Sulfur:
S-32, 95% abundant
S-33, 0.76% abundant
S-34, 4.22% abundant
S-36, 0.014% abundant
12. Potassium has 2 isotopes: K-39 and K-41. Which isotope is most abundant in
nature? How do you know?
The Electron
13. Illustrate the shape and energy of the four electron orbitals.
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14. For all of the following elements:
 Write the electron configuration
 Draw the Lewis dot notation for each
 draw the arrows that represent the electrons in each element
 Determine how many valence electrons each element has.
a. Oxygen
b. Fluorine
c. Sodium
d. Aluminum
e. Phosphorus
f. Calcium
15. What are the four sublevel blocks of the periodic table?
16. What sublevel block do we find the halogens and the noble gases? The transition
elements? The alkali and alkaline earth metals?
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17. Give an example of an electron transition that would absorb energy into the atom.
How is this transition different from one that would release energy from the
atom?
Periodic Table:
18. Describe Mendeleev’s contribution to the organization of the PT.
19. What convinced other scientists that Mendeleev’s PT was valid?
20. How is our modern PT organized?
21. What do we call a vertical column of elements on the PT?
22. What do elements in the same vertical column all have in common?
23. Where are the metals located on the PT?
24. Describe the physical properties of metals.
25. Where are the nonmetals located on the PT?
26. Describe the physical properties of nonmetals.
27. What do we call the elements that lie between the metals and the nonmetals,
having some properties of each?
28. Give two examples of those types of elements.
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29. Where are the noble gases found on the PT?
30. What is special about the noble gas family?
31. In which group are the halogens located?
32. Which is the most active halogen?
33. Which is the least active halogen?
34. In which group would the most active metals be found?
35. In which sublevel block of the PT are the most active metals found?
36. Which metal in the alkali family is most active? Why?
37. What happens to the size (radius of an atom as one goes from top to bottom in the
same group of the PT? Explain.
38. What size are the more reactive metals? Why?
39. What size are the more reactive nonmetals? Why?
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40. What do we call an atom that has either gained or lost electrons?
41. What is the name given to a positive ion?
42. How does a positive ion form?
43. What is the name given to a negative ion?
44. How does a negative ion form?
Nuclear Chemistry:
45. Define the following
a. Fission:
b. Fusion:
c. Nuclear Decay:
46. How are fission and fusion alike?
47. How are fission and fusion different?
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48. Complete the following table regarding nuclear radiation types
Symbol(s)
charge
Strength
Alpha
Beta
gamma
49. Write a reaction for the alpha decay of 238U.
50. Write a reaction for the beta decay of 16P.
51. What element is harmful to humans and forms during the natural decay cycle of
the element Uranium?
52. How does this element cause trouble for humans?
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Laboratory Questions: Flame Tests and Atomic Emission Spectra lab
1. Explain how the colors in the flame test were produced. Be sure to include what
parts of the atom are involved and how they behave.
2. How are flame tests used to identify elements?
3. How do astronomers use light data to identify elements in far away stars and
galaxies?
4. What does each line in an atomic emission spectrum represent?
5. How is the color of light related to its energy?
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Here is some Bright-line spectra data. Examine each individual element and
predict what the bright-line spectra would look like if helium and hydrogen were
mixed together and analyzed. Draw the resulting spectrum for that mixture in the
empty box below.