Final answer:
The number of orbits present in the s, p, d, and f subshells are 1, 3, 5, and 7 respectively. The maximum number of electrons that each subshell can hold is 2, 6, 10, and 14 correspondingly. For the shells or periods, the maximum number of electrons that can be in each is governed by the formula 2n², resulting in maximums of 2, 8, 18, and 32 for the first four shells.
Step-by-step explanation:
When studying subshells within an atom, the number of orbits or orbitals present corresponds to different types of subshells. The s-subshell has one orbital, the p-subshell has three orbitals, the d-subshell has five orbitals, and the f-subshell has seven orbitals. Therefore, the answer to the number of orbits present in the subshells A) s, B) p, C) d, D) f is A) 1, B) 3, C) 5, and D) 7, respectively.
The maximum number of electrons that can occupy each subshell is dictated by the formula 2(2l + 1), where l is the angular momentum quantum number associated with each subshell. For the s, p, d, and f subshells, the values of l are 0, 1, 2, and 3 respectively. This equation gives us the maximum of 2 electrons for the s-subshell, 6 for the p-subshell, 10 for the d-subshell, and 14 for the f-subshell. Thus, the answer for the subshells A) s, B) p, C) d, D) f in terms of the maximum number of electrons is B) 2, 6, 10, 14.
In terms of quantum numbers or periods of an atom, the maximum number of electrons that can be in each shell is determined by the formula 2n², where n is the principal quantum number of the shell. Using this formula, we find that the maximum number of electrons in the first four shells (n=1 to n=4) is A) 2, 8, 18, 32, which correlates to each period's maximum electron capacity.