Homework: 1. Radioactive americium - 241 is used in household smoke detectors and in bone mineral analysis. a) Give the number of electrons, protons, and neutrons in an atom of americium - 241. b) Write the proper nuclide symbol. 2. What characteristics do atoms of carbon-12, carbon-13, and carbon-14 have in common? IN what ways are they different? 3. Identify the isotope that has atoms with a) 117 neutrons, 77 protons, and 77 electrons b) 30 neutrons, 28 protons, and 28 electrons 4. How did the discovery of isotopes conflict atomic theory? with Dalton’s 5. The average mass of any large number of atoms of a given element is always the same for a given element. Explain. 6. . Naturally occurring boron is 19.9% B - 10 (mass = 10.01294 u) and 80.1% B - 11 (mass = 11.0093 u). Calculate the average atomic mass. 7. Uranium has an atomic mass equal to 238.0289. It consists of two isotopes: uranium with an isotopic mass of 235.044 u and uranium-238 with an isotopic mass of 238.051 u. Calculate the % abundance of the uranium-235 isotope. 8. How did Rutherford interpret the deflection of in his gold foil experiment? α-particles Did these findings support or disprove the plum pudding model of the atom? Explain. 9. How does Bohr's model of the atom explain the existence of line spectra? How are spectral lines produced? 10. What is the energy of a photon that has a wavelength of 8.33 x 10-6 m? 11. What is the wavelength of a photon that has an energy of 5.25 × 10-19 J 12. How does the quantum model describe the location of an electron? Periodic Table
Homework: 1. Radioactive americium - 241 is used in household smoke detectors and in bone mineral analysis. a) Give the number of electrons, protons, and neutrons in an atom of americium - 241. b) Write the proper nuclide symbol. 2. What characteristics do atoms of carbon-12, carbon-13, and carbon-14 have in common? IN what ways are they different? 3. Identify the isotope that has atoms with a) 117 neutrons, 77 protons, and 77 electrons b) 30 neutrons, 28 protons, and 28 electrons 4. How did the discovery of isotopes conflict with Dalton’s atomic theory? 5. The average mass of any large number of atoms of a given element is always the same for a given element. Explain. 6. . Naturally occurring boron is 19.9% B - 10 (mass = 10.01294 u) and 80.1% B - 11 (mass = 11.0093 u). Calculate the average atomic mass. 7. Uranium has an atomic mass equal to 238.0289. It consists of two isotopes: uranium with an isotopic mass of 235.044 u and uranium-238 with an isotopic mass of 238.051 u. Calculate the % abundance of the uranium-235 isotope. 8. How did Rutherford interpret the deflection of α-particles in his gold foil experiment? Did these findings support or disprove the plum pudding model of the atom? Explain. 9. How does Bohr's model of the atom explain the existence of line spectra? How are spectral lines produced? 10. What is the energy of a photon that has a wavelength of 8.33 x 10-6 m? 11. What is the wavelength of a photon that has an energy of 5.25 × 10-19 J 12. How does the quantum model describe the location of an electron? Periodic Table
summer-review-practice-problems-2013-08-08.docx