General Chemistry I (Casanova)
Assignment 6: Chapter 6
Name: _____________________________________________
1. Define the following terms: a) Electromagnetic radiation – b) Frequency ( ) – c) Wavelength (λ) – d) Speed of light (c) – e) Amplitude – f) Electromagnetic spectrum – g) Photon – h) Ground state – i) node – j) Paramagnetic – k) Diamagnetic - M/W or T/R ? Setup of each problem must be shown when performing ANY CALCULATION from this point on. Attention
should be given to significant figures. 2. Label the following diagram of a wave:
A
A)_______________________________________ B)_______________________________________ B C 3. C)_______________________________________ C Explain the relationship between , and E. 4. Given the diagram of the Double Slit Experiment explain what conclusions were made concerning the
nature of the electron. (Review Chapter 7 and 8 PowerPoint presentation found on the PowerPoint
Canvas page) 5. Given the diagram of the Photoelectric Effect explain what conclusions were made concerning the nature
of the electron. (Review Chapter 7 and 8 PowerPoint presentation found on the PowerPoint Canvas
page) 6. Explain the significance of the Louis deBroglie’s equation, h m v . 7. Compare and contrast the orbit proposed by Niels Bohr and the orbital proposed by Erwin Schrӧdinger. 8. Explain the significance of the Heisenberg Uncertainty Principal. 9. The MRI (magnetic resonance imaging) body scanner used in hospitals operate at 400. MHz. How much
energy does this correspond to in kJ/mol? 10. What is the λ (in meters) of UV radiation with 11. What is the 12. Given: 5.5 10 Hz
15 ? of electromagnetic radiation with a λ = 4.4 μm? 1 1
1 1.10 x107 m 1 2 2 where n2 n1 n1 n2 and 1
E h c where h 6.63 x1034 J s
c 3.00 x108 m / s (a) Calculate the energy (J) of the photon released by the hydrogen electron as it returns from n = 5 to n = 2.
(b) Calculate the energy for one mole of photons in kJ/mol.
(c) Calculate the wavelength of light emitted by photon.
(d) Based on the EM spectrum shown below what region of the spectrum do they fall? 13. Give the allowable combinations of quantum numbers for each of the following electrons.
a) b) c) d) 4s 5d electron electron 3p (the electron with a -1/2 spin) 5f _ _ _ _ _ _ 14. Give the orbital designations of electrons with the following quantum numbers. (Hint: do the opposite of
question 13 c or d)
a) b) n 3, l 0, ml 0, ms 1 2 n 2, l 1, ml 1, ms 1 2 15. Write the electron configurations for each of the elements using the method indicated. a) Co (Z = 27) (superscripted notation) b) I (Z = 53) (Kernel notation) c) F (Z = 9) (Line and arrow notation) 16. Given the subshells a) Has l 2 1s, 2 s, 2 p,3s, 3 p, and 3d , identify those that meet the following descriptions: ___________________________ b) Can have ml 1 ________________________ c) Is empty in a nitrogen atom________________________
d) Is full in a carbon (C) atom_________________________
e) Contains the outermost (valence) electrons in a beryllium (Be) atom____________________________
f) Can contain two (2) electrons, both with spin ms 1 2 _______________________________ 17. Explain why sodium vapor (sodium metal heated until it becomes gaseous) is found to be paramagnetic
while mercury vapor is found to be diamagnetic. 18. Explain why atomic radii increase down a group and decrease across a period. 19. Which atom in each of the following pairs has a larger radius? a) Na or K b) V or Zn c) V or Ta d) Li or Ba
20. Which would you expect to have the largest ionization energy, Na or Mg? Be sure to justify your answer! 21. The following table shows the ionization energies for each successive loss of an electron from the silicon
atom. Explain why a significant increase is shown when the 5th electron is lost forming the cation, Si5+. (Review
Chapter 7 and 8 PowerPoint presentation found on the PowerPoint Canvas page) # of e- lost
1
2
3
4
5
6
7 I.E.
(kJ/mol)
787
1577
3231
4356
16091
19784
23783

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