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1. Which of the following is the correct electron configuration for Zn2+?
2. Which of the following quantum number sets is possible?
3. What is the maximum number of electrons allowed in a single atomic energy level in terms of the principal quantum number n?
4. Which of the following equations describes the maximum number of electrons that can fill a subshell?
5. Which of the following atoms only has paired electrons in its ground state?
6. An electron returns from an excited state to its ground state, emitting a photon at λ = 500 nm. What would be the magnitude of the energy change if one mole of these photons were emitted? (Note: h = 6.626 × 10-34 J·s)
7. Suppose an electron falls from n = 4 to its ground state, n = 1. Which of the following effects is most likely?
8. Which of the following isotopes of carbon is LEAST likely to be found in nature?
9. Which of the following best explains the inability to measure position and momentum exactly and simultaneously according to the Heisenberg uncertainty principle?
10. Which of the following electronic transitions would result in the greatest gain in energy for a single hydrogen electron?
11. Suppose that an atom fills its orbitals as shown:
Such an electron configuration most clearly illustrates which of the following laws of atomic physics?
12. How many total electrons are in a 133Cs cation?
13. The atomic weight of hydrogen is 1.008 amu. What is the percent composition of hydrogen by isotope, assuming that hydrogen's only isotopes are 1H and 2D?
14. Consider the two sets of quantum numbers shown in the table, which describe two different electrons in the same atom.
Which of the following terms best describes these two electrons?
15. Which of the following species is represented by the electron configuration 1s22s22p63s23p64s13d5?
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