Final answer:
The electron configurations 2p^3, 4d^9, and 3s^1 are correctly identified as shell 2 p subshell with 3 electrons, shell 4 d subshell with 9 electrons, and shell 3 s subshell with 1 electron respectively. The configuration 5g^16 is not allowed as the 'g' subshell does not exist in the current understanding of chemsitry.
Step-by-step explanation:
When identifying the shell, subshell, and number of electrons in atomic orbitals, we follow certain principles in Quantum Chemistry. The principal quantum number (n) indicates the shell, the angular momentum quantum number (l) indicates the subshell (s, p, d, f), and the superscript indicates the number of electrons in that subshell. However, it's important to note that there is no 'g' subshell in currently known chemistry. Here are the correct identifications:
- (a) Shell: 2, Subshell: p, Number of electrons: 3
- (b) Shell: 4, Subshell: d, Number of electrons: 9
- (c) Shell: 3, Subshell: s, Number of electrons: 1
- (d) The notation '5g^{16}' is not allowed since the 'g' subshell does not exist with the current understanding of chemistry.
The Pauli Exclusion Principle also states that no two electrons can have the same set of quantum numbers within a single atom, which explains the limitations on the number of electrons within subshells.