CHEM 111 FA 2002 Exam 4 Name _______________________ C ONSTANTS A ND E QUATIONS : c = 2.998 x 10 8 m/s h = 6.626 x 10 34 J . s R = 1.0974 x 10 7 m 1 R H (from your textbook) = (R)(h)(c) = 2.18 x 10 18 J = c/ E = h n 2 n Rhc Multiple Choice Questions . 5 points each. Partial credit may be given if some work is shown in margin. 1. What is the energy of one photon of light having a wavelength of 978 nm? a) 3.07 x 1014Jb) 3.07 x 105Jc) 2.03 x 1019Jd) 1.22 x 10 19 J 2. The Heisenberg Uncertainty Principle "says" which of the following: 3. Which group below represents a set of isoelectronic species? Ar, Ca 2+ 4. Which of the following orbital designations ISallowed by quantum mechanics? = 1 m l = 1 5. Which of the following particles is the most paramagnetic? a) Krb) Mn2+c) Cu2+d) Ase) Co 2+ 6. Which of the following bonds is the most polar? (A table of electronegativities is provided) Cs-Cl 7. Calculate energy of the photon released when an electron makes the transition from level n = 5 to n=1 18 J
8. Which atom or ion has the ground state electron configuration illustrated below, for its outer shell electrons? 4s 3d 2+ 9. Fluorine is very likely to gain an electron, and sodium is very likely to lose an electron, when forming their ions. The best explanation for this is: a) fluorine is a larger atom than sodiumb) outer shell electrons on fluorine are more shielded from the nucleus charge than outer shell electrons on sodium.c) both atoms gain an inert gas, filled-shell configuration when they form their most common ions.d) sodium is more reactive than fluorine. 10. Which electron configuration below would represent an element with chemical properties similar to fluorine? (All of the configurations are quantum mechanically allowed and are correct for some element.) 2
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