CHEM 1364 Test 3 Fall 1999
1. _______________________ radiation is a term that covers the type of radiation emitted from TV towers, microwaves, and light bulbs.
2. A(n) _______________ is a 'particle' of the radiation described above.
3. The _______________________ effect was explained by Einstein, using Planck's concept of quantized energy packets of light.
4. A(n) ______________ spectrum emits only discrete frequencies of light, as opposed to all of the frequencies that are possible.
5. Heisenberg's _______________ principle states that we cannot know both the position and the momentum of an object.
6. Schrodinger manipulated equations describing ___________ to explain the quantized energy levels that are observed in atoms.
7. A(n) _______________ is the name for the probability function of an electron 'around' an atom.
8. The _______________ Exclusion Principle states that no electron may have the same set of four quantum numbers.
9. Although the elements in the periodic table were grouped based on similar chemical and physical properties, we now believe the ______________ electronic structures are the same for these elements.
10. Atomic radii _________________ (increase/decrease) as we go from left to right across a period on the Periodic Table.
11. _____________________________ is the energy required to remove an electron from an atom in the gas phase.
12. _____________________________ is the energy required to add an electron to an atom in the gas phase.
13. ________________ are elements that are in transition from metals to non metals.
14. Nonmetal oxides are __________________ (acidic/basic).
15. ____________________ are different forms of the same element, such as O2 and O3 are both elemental forms of oxygen.
16. The first ionization energy for Rb is 403 kJ/mol. Calculate the wavelength and frequency of light required to just remove an electron from Rb. What region of the EM spectrum is this light?
17. Calculate the frequency, wavelength, and energy of the photon that is emitted when an electron falls from the n = 5 to the n = 2 orbit in hydrogen.
18. Show the electronic configuration for the following elements:
N, Ni, Cd, Eu, Uun
19. Arrange the following atoms in order of increasing atomic size:
At, Br, Cl, I
As, Br, Ca, Ga
Ba, Ge, Ne, S
20. Explain why the first ionization energy of nitrogen is greater than the first ionization energy of oxygen, and why the electron affinity of nitrogen is greater than zero, while all other non metals (and most metals) show an electron affinity that is less than zero.