The 3rd shell of an atom can hold a maximum of 18 electrons, which corresponds to 3 subshells: s, p, and d. Each subshell has a specific number of orbitals: s = 1, p = 3, d = 5. Therefore, there are a total of 9 orbitals in the 3rd shell.
Each orbital in the 3rd shell can hold a maximum of 2 electrons. This is based on the Pauli exclusion principle, which states that each orbital can only contain 2 electrons with opposite spins.
The 3rd shell can hold a maximum of 18 electrons. This is because the 3rd shell has 3 subshells (s, p, and d) which can hold a total of 18 electrons (2 in the s subshell, 6 in the p subshell, and 10 in the d subshell).
The 3rd shell can have a maximum of 3 subshells: s, p, and d. This is based on the principle that each subshell corresponds to an angular momentum quantum number (l) and in the 3rd shell, l can have values of 0, 1, and 2.
The number of orbitals in the 3rd shell (9 orbitals) is greater than the 2nd shell (4 orbitals) and less than the 4th shell (16 orbitals). This is because the number of orbitals increases with the principle quantum number (n), and for a specific n value, the number of orbitals increases with the angular momentum quantum number (l).