7. Calculate the energy (J) of a pure elemental sample weighing 0.5 g. 8. Determine the mass (g) of a sample with an energy of 1.78 eV.
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- Which of these expressions would yield the wavelength of light in meters emitted when an electron drops from orbit n = 3 to n = 2 in a Bohr hydrogen atom? Given h = 4.14 x 10-15 eVs and c = 3.00 x 108 m/s. a. 1.89/hxc b. hc/1.89 c. 1.89 x h x c d. (1.51 + 3.4)/hc e. hc/3.41. Enumerate the microstates of p3. Determine the MS and ML values for each microstate. 2. On a table of possible MS and ML values, tally the microstates in no. 1 for a particular combination of MS and ML 3. Based on the table in no. 2, determine the atomic term symbols for the allowed atomic states of p3 resulting from the coupling of orbital and spin angular momentums. 4. Arrange the term symbols in no. 3 according to increasing energy.1. The equation q = ne tells us that charge is quantized in the form of small packets. Note that q is charge in coulomb (C), e is the charge of the electron, and n is the number of electrons. Using this equation, calculate the number of electrons that make up a charge of +24mC.
- 7. For the 3p and 3d states of hydrogen, show that (-) avg =1/1290. ao. n²1. Differentiate the three quantum numbers for an electron in the hydrogen atom and justify why the idea of an electron orbiting a proton has been abandoned.4. In each of the following equations, determine the emitted particle(s) in each case. 141 La → 57 a. b. C. d. 222 Rn → 86 238 U → 92 34 226 88 218 Po + ? 84 234 Th + ? 90 34 CI→ ³4S + ? 16 Ra → 222 Rn + ? 86 e. f. g. h. 138 Nd → 60 212 Pb → 82 215 Po 84 141 Ce + ? 58 138 Pr + ? 59 212 23Bi + ? 83 211Pb + ? 82