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美女与野兽―*宇宙 骑士*
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CHEM 1101D First review Questions January 2005
# Question
1 What special properties do elements have compared to all other materials?
2 Why did the early Greeks think matter was made up of atoms?
3 Why did the misunderstanding of gases lead to the idea of “phlogiston（燃素）”?
4 Describe how Boyle’s measurement of gas density in the 1780's fixed this problem.
5 Explain why Lavoisier’s use of balanced chemical equations allowed him to be the first person to calculate the power of gun powder.
6 Explain the meaning of the Law of Multiple (or Combining) Proportions
7 How did Dalton in 1810 use the Law of Multiple Proportions to update the
Greek Atomic Theory of matter?
8 Why was element Hydrogen used as the beginning of the Atomic Weight scale?
9 Why was this calibration (校准) wrong by a factor of 2?
10 Explain how putting elements in order of their increasing atomic weights allowed the phenomenon of the “periodic properties” of elements to be recognized.
11 How was the linear sequence(次序) of elements converted to the 2 dimensional Periodic Table?
12 Explain how the existence of Gallium (镓) and Germanium (锗) was predicted in 1870.
13 What other complete groups or periods of elements were found later for the same reason?
14 Why did Moseley replace atomic weight with atomic number as the basis of the periodic table in 1913?
15 Explain how Bohr used Coulomb’s law of electrical attraction to set up the orbit theory of atomic structure in 1913.
16 Explain why the fundamental error of mechanical measurement (Planck’s constant) makes Bohr’s Newtonian model unusable in these extremely small atomic systems
17 How was the orbit model of atoms modified to allow for this measurement error?
18 What are the probability shapes of s, p and d orbitals?
19 What are the 3 main differences between a metal and a non-metal element?
20 Where are these types of elements in the Periodic Table?
21 What special properties do semi-metals have?
22 Define the electron affinity (吸引力) of an atom
23 Define the ionization (电离) potential of an atom
24 Define the electronegativity using electron affinity and ionization potential
25 Also define Hardness with electron affinity and ionization potential
26 How do Electronegativity and Hardness vary down groups and across periods of the Periodic Table?
27 What is the First Order force controlling orbital energies in atoms?
28 On an energy level graph show the order of orbital energies of an atom in a column.
29 In the next column of this graph show the energy change due to the Second Order Force.
30 Explain this change in orbital energies by the “Shielding Effect”
31 Define the Aufbau Principle (构造原理) for describing atoms of elements in their ground state.
32 What limitation to Aufbau is described by the Pauli paring Principle (泡利不相容原理)?
33 In Group 1A give the electronic configuration (构造) of element K.
34 Explain using Shielding why the last electron of K has a very low ionization potential.
35 In Group 2A, use Shielding to explain why the Stable Oxidation Number is 2+.
36 In Group 3A Compare the electron configurations of Boron (硼) and Aluminum to explain why Boron is a nonmetal but Aluminum is a metal.
37 In Group 4A, explain why Carbon can have Stable oxidation Numbers from +4 to -4.
38 Use Shielding to explain why the ionization potential of Silicon (Si) and the following elements are much smaller than for Carbon.
39 Explain the naming system for straight chain Carbon compounds with Hydrogen
40 How are such compounds with branches numbered and named?
41 What changes are needed for Carbon compounds with “multiple” bonding?
42 Define the two conformations of cyclohexane ( ).
43 What special bonding occurs in aromatic (芳香的) compounds?
44 Starting with benzene give three examples with names of aromatic compounds
45 Why is graphite (石墨) the ultimate aromatic substance?
# Question
1 What special properties do elements have compared to all other materials?
2 Why did the early Greeks think matter was made up of atoms?
3 Why did the misunderstanding of gases lead to the idea of “phlogiston（燃素）”?
4 Describe how Boyle’s measurement of gas density in the 1780's fixed this problem.
5 Explain why Lavoisier’s use of balanced chemical equations allowed him to be the first person to calculate the power of gun powder.
6 Explain the meaning of the Law of Multiple (or Combining) Proportions
7 How did Dalton in 1810 use the Law of Multiple Proportions to update the
Greek Atomic Theory of matter?
8 Why was element Hydrogen used as the beginning of the Atomic Weight scale?
9 Why was this calibration (校准) wrong by a factor of 2?
10 Explain how putting elements in order of their increasing atomic weights allowed the phenomenon of the “periodic properties” of elements to be recognized.
11 How was the linear sequence(次序) of elements converted to the 2 dimensional Periodic Table?
12 Explain how the existence of Gallium (镓) and Germanium (锗) was predicted in 1870.
13 What other complete groups or periods of elements were found later for the same reason?
14 Why did Moseley replace atomic weight with atomic number as the basis of the periodic table in 1913?
15 Explain how Bohr used Coulomb’s law of electrical attraction to set up the orbit theory of atomic structure in 1913.
16 Explain why the fundamental error of mechanical measurement (Planck’s constant) makes Bohr’s Newtonian model unusable in these extremely small atomic systems
17 How was the orbit model of atoms modified to allow for this measurement error?
18 What are the probability shapes of s, p and d orbitals?
19 What are the 3 main differences between a metal and a non-metal element?
20 Where are these types of elements in the Periodic Table?
21 What special properties do semi-metals have?
22 Define the electron affinity (吸引力) of an atom
23 Define the ionization (电离) potential of an atom
24 Define the electronegativity using electron affinity and ionization potential
25 Also define Hardness with electron affinity and ionization potential
26 How do Electronegativity and Hardness vary down groups and across periods of the Periodic Table?
27 What is the First Order force controlling orbital energies in atoms?
28 On an energy level graph show the order of orbital energies of an atom in a column.
29 In the next column of this graph show the energy change due to the Second Order Force.
30 Explain this change in orbital energies by the “Shielding Effect”
31 Define the Aufbau Principle (构造原理) for describing atoms of elements in their ground state.
32 What limitation to Aufbau is described by the Pauli paring Principle (泡利不相容原理)?
33 In Group 1A give the electronic configuration (构造) of element K.
34 Explain using Shielding why the last electron of K has a very low ionization potential.
35 In Group 2A, use Shielding to explain why the Stable Oxidation Number is 2+.
36 In Group 3A Compare the electron configurations of Boron (硼) and Aluminum to explain why Boron is a nonmetal but Aluminum is a metal.
37 In Group 4A, explain why Carbon can have Stable oxidation Numbers from +4 to -4.
38 Use Shielding to explain why the ionization potential of Silicon (Si) and the following elements are much smaller than for Carbon.
39 Explain the naming system for straight chain Carbon compounds with Hydrogen
40 How are such compounds with branches numbered and named?
41 What changes are needed for Carbon compounds with “multiple” bonding?
42 Define the two conformations of cyclohexane ( ).
43 What special bonding occurs in aromatic (芳香的) compounds?
44 Starting with benzene give three examples with names of aromatic compounds
45 Why is graphite (石墨) the ultimate aromatic substance?
