Determine the maximum number of electrons that each of the following orbitals (sublevels) can hold. Consider only the electrons needed to fill the orbitals indicated. a) 6s b) 5p c) 4d d) 5f
The Correct Answer and Explanation is:
Here are the maximum numbers of electrons that each of the given sublevels can hold:
a) 6s → 2 electrons
b) 5p → 6 electrons
c) 4d → 10 electrons
d) 5f → 14 electrons
Explanation:
Each electron in an atom is described by four quantum numbers: the principal quantum number (n), the angular momentum quantum number (l), the magnetic quantum number (ml), and the spin quantum number (ms). The sublevel or orbital type (s, p, d, f) corresponds to a particular value of l, which determines the shape of the orbital and the number of orbitals it contains.
- s sublevel (l = 0): Has 1 orbital. Each orbital can hold a maximum of 2 electrons (one with spin up, one with spin down). So, the 6s sublevel holds 2 electrons.
- p sublevel (l = 1): Has 3 orbitals (ml = −1, 0, +1). Each can hold 2 electrons. So, the 5p sublevel holds 6 electrons.
- d sublevel (l = 2): Has 5 orbitals (ml = −2, −1, 0, +1, +2). Each orbital holds 2 electrons, so the 4d sublevel holds 10 electrons.
- f sublevel (l = 3): Has 7 orbitals (ml = −3 to +3). Each can hold 2 electrons. So, the 5f sublevel holds 14 electrons.
These values are consistent across all energy levels, meaning any s sublevel holds 2 electrons, any p sublevel holds 6, any d sublevel holds 10, and any f sublevel holds 14. The energy level number (the number in front, such as 4d or 5f) does not change the maximum capacity of the sublevel, but it does affect its energy and the distance from the nucleus.
