Quantum numbers describe the location of the outermost or valence electron. There are five quantum numbers: principal (n), angular momentum (l), magnetic (ml), and spin (ms). Following Bohr's atomic theory, electrons are believed to orbit the nucleus within defined energy levels, beginning at level 1 which is nearest to the nucleus and increasing through levels 2, 3, 4, 5, 6, and 7. These levels correspond to the principal quantum number. Each orbital contains subshells, which follow the order of increasing complexity: s, p, d, and f. The angular momentum quantum numbers correspond to these subshells as follows: s=0, p=1, d=2, and f=3. Hence, for an electron in the 5p orbital, the quantum numbers are: 5, 1. The correct matches are as follows:
In the context of NMR spectroscopy, a significant magnetic field creates an energy difference between the alpha and beta spin states, which allows nuclei to absorb RF radiation, ultimately leading to the excitation of a nucleus from a +1/2 spin state to a -1/2 spin state.
Molarity is defined as the number of moles present in one liter of solution. Given the mass of NH₃ is 2.35 g and its molar mass is 17 g/mol, the moles of NH₃ in 2.35 g can be calculated as 2.35 g / 17 g/mol = 0.138 mol. Consequently, in a 0.05 L solution, the number of moles amounts to 0.138 mol. Therefore, the concentration in 1 L is: 0.138 mol / 0.05 L x 1L = 2.76 mol. Thus, the molarity of NH₃ is 2.76 M.
