Given the photoelectron spectrum above, which of the following best explains the relative positioning of the peaks on the horizontal axis? O has more valence electrons than Ti or C, so more energy is required to remove them O has more electron-electron repulsions in the 2p sublevel than Ti and C Ti atoms are present in a greater quantity than O than C in the mixture. Ti has a greater nuclear charge, but the 2p sublevel experiences greater shielding than the 1s sublevel. Given the photoelectron spectrum of Scandium above, which of the following best explains why Scandium commonly makes a 3+ ion as opposed to a 2+ ion? Removing 3 electrons releases more energy than removing 2 electrons. Scandium is in Group 3, and atoms only lose the number of electrons that will result in a noble gas electron configuration The amount of energy required to remove an electron from the 3d sublevel is close to that for the 4s sublevel, but significantly more energy is needed to remove electrons from the 3p sublevel. Removing 2 electrons alleviates the spin-pairing repulsions in the 4s sublevel, so it is not as energetically favorable as emptying the 4s sublevel completely. On the photoelectron spectrum for magnesium given above, draw the spectrum for aluminum. Answer Key
Given the photoelectron spectrum above, which of the following best explains the relative positioning of the peaks on the horizontal axis? O has more valence electrons than Ti or C, so more energy is required to remove them O has more electron-electron repulsions in the 2p sublevel than Ti and C Ti atoms are present in a greater quantity than O than C in the mixture. Ti has a greater nuclear charge, but the 2p sublevel experiences greater shielding than the 1s sublevel. Given the photoelectron spectrum of Scandium above, which of the following best explains why Scandium commonly makes a 3+ ion as opposed to a 2+ ion? Removing 3 electrons releases more energy than removing 2 electrons. Scandium is in Group 3, and atoms only lose the number of electrons that will result in a noble gas electron configuration The amount of energy required to remove an electron from the 3d sublevel is close to that for the 4s sublevel, but significantly more energy is needed to remove electrons from the 3p sublevel. Removing 2 electrons alleviates the spin-pairing repulsions in the 4s sublevel, so it is not as energetically favorable as emptying the 4s sublevel completely. On the photoelectron spectrum for magnesium given above, draw the spectrum for aluminum. Answer Key
pes_assessment.docx