Download Chapter 8 and 10: Structure of the Atom

Unit 2 Form and Function Problem Sets
1.
How did Aristotle and Democritus describe matter in ancient Greek times? How were their descriptions of
matter different? Explain why Aristotles ideas were more popular, even though they were later proven to be
wrong (approximately 2000 years later!).
2. Explain the experiments performed by John Dalton in the early 1800’s and the inductive reasoning he used in
formulating his model of the atom.
3. Clearly describe what you observed in a Crookes tube and explain what information this provides and the
inductive reasoning used in the development of the structure of the atom.
4. What specific information did Thompson include in his model of the atom that was different from Dalton?
5. Describe Millikan’s oil-drop experiment, the observations he made and the inductive reasoning he used to
further the developing model of the atom.
6. Describe Rutherford’s gold foil experiment. Explain the observations he made and the inductive reasoning he
used to further the developing model of the atom.
7. What specific information did Rutherford include in his model of the atom that was different from Thompson?
8.
What differentiates two elements from each other?
9. Using each of the four models of the atom, sketch or describe what an oxygen atom would be like in each
theory.
a. Dalton
b. Thompson
c. Rutherford
d. Bohr
10. Describe what you observed in the gas discharge tube for hydrogen gas. What inductive reasoning was made
by Bohr when he made these observations and how did that further the developing model of the atom?
11. What specific information did Bohr include in his model of the atom that was different from Rutherford?
12. If an atom was blown up to the size of the dome of the capitol building, an atom’s nucleus would be the size of
a.
A grain of salt
b. an orange
d. a basketball
d. the dome
In this model of an atom, what would be size of the electrons be?
13. Why was it so difficult to detect and identify the neutron?
14. Where is most of the mass of an atom located? Explain.
Average Atomic Mass
15. Rubidium has two common isotopes, 85Rb and 87Rb. If the abundance of 85Rb is 72.2% and the abundance of
87
Rb is 27.8%, what is the average atomic mass of rubidium?
16. Uranium has three common isotopes. If the abundance of 234U is 0.01%, the abundance of 235U is 0.71%, and the
abundance of 238U is 99.28%, what is the average atomic mass of uranium?
17. Titanium has five common isotopes: 46Ti (8.0%), 47Ti (7.8%), 48Ti (73.4%), 49Ti (5.5%), 50Ti (5.3%). What is the
average atomic mass of titanium?
18. Explain why atoms have different isotopes. In other words, how is it that helium can exist in three different
forms?
15. Complete the following table:
Element
Protons
Neutrons
a.
Te
b.
c.
52
120
52
75
Electrons
Mass #
54
Lu
176
5
Ce
g.
83
12
+3
33
0
15
0
Zn
j.
1
k.
1
C
m.
Th
n.
142
Ca
20
p.
Te
76
q.
45
r.
66
+2
2
+1
13
0
59
+2
55
+6
8
0
s.
18
32
-2
t.
38
88
+2
u.
23
He
0
58
9
4
92
28
o.
Xe
1
1
l.
132
56
h.
i.
+2
0
e.
Symbol
0
d.
f.
Charge
18
+3
19. What are the major parts of the electromagnetic spectrum?
20. What is the energy of a quantum of light with a frequency of 4.31 x 10 14 Hertz? What is the wavelength of
this light?
21. What is the energy of a quantum of light with a frequency of 6.8 x 1018 Hertz? What is the wavelength of this
light?
22. What is the energy of a quantum of light with a frequency of 9.5 x 10 15 Hertz? What is the wavelength of this
light?
23. A certain green light has a frequency of 6.26 x 10 14. What is its wavelength?
24. A certain violet light has a wavelength of 413 nm. What is the frequency of the light?
25. A certain green light has a wavelength of 486 nm. What is the frequency of the light? What is the energy of
light with wavelength 662 nm. First find the frequency in hertz of this wavelength of light.
26. Draw an s orbital.
27. Draw the 3 p orbitals.
28. How many d orbitals are there in each sublevel? How many f orbitals in each sublevel?
29. Which set of orbitals has the higher energy?
a. 3p or 4p
b. 3d or 4p
c. 5p or 6s
d. 4d or 5p
e. 4f or 6s
30. What is the maximum number of elextrons in an s orbital, p subshell, d subshell, and f subshell?
31. Why are there 10 members of each transition series?
32. Which subshell is filled next after the following subshells are filled?
33. Write electron configurations for the following:
a. Be
b. Mg
c. Ca
d. Sr
What is the similarity in the configurations of these elements?
34. Write electron configurations for the following:
a. Sc
b. Ti
c. Ni
d. Zn
Which sublevel is changing in these configurations?
35. Write using orbital notation the electron arrangement for copper.
36. Write ground state electron configurations for the following elements:
a. Ti
b. Mo
c. S
d. Zn
e. Ag
37. Determine the neutral atom whose ground state electron configuration is:
a. 1s22s22p63s23p64s23d8
b. 1s22s22p63s23p64s23d104p65s24d10
c. 1s22s22p63s23p4
38. Given the following, what neutral atom is represented?
1s
2s
2p
39. Write the complete orbital notation for the following:
a. Mg
b. Cr
c. Al
d. Xe
e. He
40. What is the last term in the electron configuration for the following:
a. Ba
b. Sc
c. Fe
d. C
e. Se
f. Ne
41. What is the most stable ion for the following:
a. Ca
b. Na
c. Al
d. S
e. N
f. Cl
42. Write electron configurations for the following ions:
a. O-2
b. Mg+2
c. Cl-1
d. Sc+2
e. Cd+2
f. As-3
g. Te
Which element do the electron configurations of these ions resemble? Why?
43. Using electron configurations, explain why aluminum forms a stable +3 ion.
44. For each of the following electron configurations of neutral atoms, determine the element listed and if the
configuration is a ground state configuration or an excited state.
a. 1s22s22p6
b. 1s22s22p53s2
c. 1s22s22p63s23p64s23d3
d. 1s22s22p63s25s1
45. What ions could have the following electron configuration (list at least 4)?
1s22s22p63s23p6
46. Give an example of the following:
a. two ions of the same atom.
b. two ions isoelectronic to each other
c. two atoms which are isotopes of the same element
47. Write one possible notation for excited Al.
48. Write the electron configuration for the following: (long method)
a. C
b. Ar
c. Zn
d. Ga
49. Write the last term of the electron configuration for each of the following:
a. N
b. Ca
c. Ge
d. Nd
e. Mo
50. Write the electron configuration for the following: (using the last noble gas)
a. Na
b. Cl
c. V
d. Sb
e. N
51. Write the electron configuration for the following ions:
a. Cl-1
b. O-2
c. Ca+2
d. Ni+2
e. V+2
52. Name three elements with an incomplete d orbital.
53. Why are the noble gases considered to be stable?
54. Explain clearly the difference between an orbital and a sublevel.
55. Briefly explain why the 4s orbital “fills” before the 3 d orbitals, and why electrons are lost from the 4s orbital
before the 3d orbital.
56. Name three ions isoelectronic to Kr.
57. Draw an orbital diagram for:
a. Ca
b. Ca+2
c. Ca+1
d. V
e. V+1
58. Write the electron configuration for the following:
a. Na
b. Na+1
c. Ca+2
d. O-2
e. Mn
59. What ion would be most stable for the following atoms:
a. Mg
b. Sc
c. Cl
d. N
e. S
f. V+2
g. V+3
f. Li
60. Explain how a negative ion is formed. Explain how a positive ion is formed.
61. The element barium has an atomic number of 56, and a selected Ba +2 ion has a mass number of 137. How many
protons, neutrons, and electrons are in the Ba+2 ion?
62. What are the three isotopes of hydrogen and what is the difference between them?
63. Draw a picture which shows the formation of a Cl-1 ion from a neutral Cl atom?
64. What is the difference between a 1s orbital and a 2s orbital?
65. Which sublevel has the highest energy (of the sublevels that actually fill in ground state notations of atoms
from the periodic table)?
66. Which orbital has the lowest energy?
67. What is the order of filling orbitals through the 5p orbitals.
68. Write complete electron configuration for the following:
a. Ne
b. K
c. I
d. Au
e. B+3
69. What is the last tem in the electron configuration for the following:
a. Li
b. S
c. Al
d. U
e. Ag
f. Si+2
g. Br-1
f. Th
70. Clearly explain how neutral isotopes of the same element are similar and different. Be sure to include
electrons, protons, neutrons, mass number, and atomic numbers.
71. What are the major groups on the periodic table? What are the properties of each group?
72. How does the number of valence electron affect the properties of the different groups of atoms?
73. What happens to atomic size, radius, ion size, ionization energy, and electronegativity as you go across a row on
the periodic table? As you go down a row on the periodic table?