Question

How many total electrons can occupy the following orbitals: s= ___ , p= ___ , d=, f=.

a) s= 2, p= 6, d= 10, f= 14.
b) s= 4, p= 8, d= 18, f= 32.
c) s= 1, p= 3, d= 5, f= 7.
d) s= 0, p= 2, d= 4, f= 6.

Answer 1

The s subshell holds 2 electrons, the p subshell holds 6, the d subshell holds 10, and the f subshell holds 14, making option a) the correct answer.

Step-by-step explanation:

The total number of electrons that can occupy the s, p, d, and f orbitals are as follows: an s subshell can accommodate 2 electrons, a p subshell can accommodate 6 electrons, a d subshell can accommodate 10 electrons, and an f subshell can accommodate 14 electrons.

Each orbital within these subshells can hold a maximum of two electrons with opposing spins, according to the Pauli exclusion principle and Hund's rules. The correct total electron capacities for the orbitals are therefore: s= 2, p= 6, d= 10, f= 14, which corresponds to option a).