Step-by-step explanation:
Hund's first and second rules describe how electrons are arranged in an atom's orbitals. Hund's first rule states that when electrons occupy orbitals of equal energy (such as the three p orbitals in a given shell), they will each first occupy separate orbitals before any orbital receives a second electron. This means that electrons will always try to maximize their spin, with one electron in each orbital having the same spin before any pairing occurs.
Hund's second rule states that if two or more orbitals of the same energy level are available, electrons will occupy empty orbitals before they pair up in an orbital that already has an electron.
Now, let's look at the orbital notation for sulfur. The atomic number of sulfur is 16, which means it has 16 electrons.
The orbital notation for sulfur would be:
1s² 2s² 2p⁶ 3s² 3p⁴
This indicates that sulfur has two electrons in the 1s orbital, two electrons in the 2s orbital, and six electrons in the 2p orbital, fully occupying all three 2p orbitals with two electrons in each and spinning in the same direction. Sulfur also has two electrons in the 3s orbital and four electrons in the 3p orbital, with a single electron in each of the three 3p orbitals and the fourth 3p orbital being half-filled. The half-filled 3p orbital is a consequence of Hund's rule, which predicts that electrons will fill each of the three 3p orbitals with one electron before any two orbitals receive a second electron.