Final answer:
The subshells present in the n = 5 shell are 5s, 5p, 5d, and 5f. There are five subshells for n = 5, representing different angular momentum values denoted by the quantum number l. The spectroscopic notation for these subshells uses the principal quantum number followed by the letter representing the subshell.
Step-by-step explanation:
The subshells present in the n = 5 shell include the s, p, d, and f subshells. In quantum mechanics, the principal quantum number n corresponds to the energy level of the electron in an atom. For any given value of n, there are n subshells. Since we are considering n = 5, there are five subshells present: 5s, 5p, 5d, and 5f. The fifth, 5g, theoretically exists but is not occupied in elements currently known.
The spectroscopic notation for these subshells would be 5s for l = 0, 5p for l = 1, 5d for l = 2, and 5f for l = 3. Remember that each subshell can hold a different number of electrons: the s can hold 2, p can hold 6, d can hold 10, and f can hold 14 electrons.