Download 6.9: electron configuration and the periodic table

NAME:
HONORS CHEMISTRY GUIDED READING ASSIGNMENT
CHAPTER 6
25 points
DIRECTIONS: Complete this packet and hand it in on the day of the chapter 6 test (due at the
time the test is given). It is suggested that you work on a portion of it each night. You can use
this packet during class when notes are being given, but completing the packet does not
replace the action of taking notes in class. It is expected that you will take notes during class,
even if it is just adding to the material in this packet. Remember, the class notes are the
primary source for test material.
6.1: THE WAVE NATURE OF LIGHT
1. What is electromagnetic radiation?
2. List 3 examples of electromagnetic radiation:
a.
b.
c.
3. Label the diagrams below and define each of the measurable characteristics of the wave.
Characteristic 1:
Characteristic 2:
Characteristic 3:
4. At what speed does electromagnetic radiation move?
5. What is the equation used to relate frequency and wavelength? What is the value for c? Solve the equation for
frequency then solve it for wavelength.
6. What is the relationship between frequency and wavelength?
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7. What are the units for frequency and wavelength?
8. Label the following diagram with the types of electromagnetic radiation:
9. Using the diagram above to explain why the colors of a rainbow are always arranged ROYGBIV.
10. Using the diagram above, explain why gamma rays are very harmful.
Solve problem # 7 on P. 230.
6.2: QUANTIZED ENERGY AND PHOTONS
1. List the three phenomena associated with light that wave theory of light can’t explain:
1.
2.
3.
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2. What relationship were physicists in the 1800’s trying to understand?
3. Explain Planck’s assumption.
4. What equation was proposed to explain Plank’s assumption? What is the value for h? Solve the equation for
frequency.
5. What is the relationship between frequency and energy?
6. What are the units for frequency and energy?
7. Explain how the model of the steps on P. 203 is appropriate for Planck’s work.
8. Briefly explain the photoelectric effect.
9. Label the photoelectric effect diagram below.
10. Explain the significance of the photon to Planck’s theory.
Solve problems 13, 17, 19 on P. 231.
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6.3: LINE SPECTRA AND THE BOHR MODEL
1. How is a spectrum produced?
2. What is the difference between a continuous spectrum and a line spectrum?
3. What is the Rydberg equation? What is it used to calculate? Define each of the variables.
4. Describe the Rutherford model of the atom
5. Describe the Bohr model of the atom.
6. What is a major shortcoming of the Bohr model? What does Bohr assume to justify his model of the atom?
7. State the 3 postulates of Bohr’s model.
1.
2.
3.
8. Describe the first orbit in the Bohr model of an atom.
9. How does the Rydberg equation justify Bohr’s model of the atom?
10. What are the limitations of the Bohr model of the atom?
Solve problems 21, 27, 29 and 31 on P. 231.
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6.4: THE WAVE BEHAVIOR OF MATTER
1. What concept did deBroglie add to atomic theory?
2. What is the deBroglie equation? Solve the equation for mass and then for velocity. What is the value of h?
3. State Heisenberg’s Uncertainty principle. What are its implications for the study of the atom?
6.5: QUANTUM MECHANICS AND ATOMIC ORBITALS
1. What was Erwin Schrodinger’s contribution to atomic theory?
2. What does the solution to Schrodinger’s equation for a hydrogen atom produce?
3. What is the difference between an orbit and an orbital?
4. What are quantum numbers?
5. List at least two pieces of information about the following quantum numbers:
1. Principle quantum number
2. Azimuthal quantum number
3. Magnetic quantum number
6. Which quantum number(s) indicate(s) the energy level (shell) of an electron?
7. Which quantum number(s) indicate(s) the energy sublevel (subshell) of an electron?
8. What is the acceptable range of values for n? Why?
9. What is the acceptable range of values for l? Why?
10. What is the acceptable range of values for ml? Why?
11. How can one quickly determine the total number of orbitals in an energy level (shell)?
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12. Explain the following diagram (and what about the cartoon???)
Solve problems # 41, 43 and 45 on P. 232
6.6: REPRESENTATIONS OF ORBITALS
1. Explain why the s orbital in the diagram below gets larger with increasing principle quantum number.
2. Describe the shape of a p orbital.
3. Using the diagram below, explain why there are 3 p orbitals for each energy level (shell) beginning with the second
energy level (shell).
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4. In which energy levels are d orbitals found? What is the azimuthal quantum number for the d orbital?
5. Using the diagram below, explain why there are 5 d orbitals for each energy level (shell) beginning with the third
energy level (shell).
6. In which energy levels are f orbitals found? How many f orbitals are found in each energy level (shell) beginning with
the fourth energy level (shell).
7. After reviewing the material in this section, explain why these values are recorded for each column in the following
table:
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6.7: MANY ELECTRON ATOMS
1. How does the energy of an orbital change with an increase in the value of l?
2. Explain why the orbitals are staggered in the following diagram:
3. What does the spin quantum number reveal about an electron? What is its notation?
4. State the Pauli Exclusion Principle.
Solve problem # 55 on P. 233
6.8: ELECTRON CONFIGURATIONS
1. What is Hund’s rule and how does it affect an electron configuration?
2. Draw an orbital electron configuration for an element of your choice.
3. Draw an electron configuration (using standard electron configuration notation) for an element of your choice.
4. Draw a condensed electron configuration (noble gas electron configuration) for an element of your choice.
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6.9: ELECTRON CONFIGURATION AND THE PERIODIC TABLE
1. What are valence electrons?
2. In which groups on the periodic table are the valence electrons of the atoms in filling the s orbitals?
3. In which groups on the periodic table are the valence electrons of the atoms in filling the p orbitals?
4. In which groups on the periodic table are the valence electrons of the atoms in filling the d orbitals?
5. In which groups on the periodic table are the valence electrons of the atoms in filling the f orbitals (add more specifics
as necessary)?
6. Why are there some electron configurations that do not follow the expected pattern for d block elements? Where on
the periodic table do these exceptions occur?
Try to do electron configurations (3 types) for some of the s, p and d block elements.
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