question arrange the electrons in the sulfur atom in the orbital diagram. use the periodic table to…

Explanation:

Step1: Determine sulfur's atomic number

Sulfur (S) has an atomic number of 16, so it has 16 electrons.

Step2: Fill electrons in orbitals

• Fill the 1s orbital first. The 1s orbital can hold 2 electrons, so we put two spin - paired electrons ($\uparrow\downarrow$) in the 1s box.
• Then fill the 2s orbital. The 2s orbital can also hold 2 electrons, so we put two spin - paired electrons ($\uparrow\downarrow$) in the 2s box.
• Next, fill the 2p orbitals. The 2p sub - shell has 3 orbitals and can hold 6 electrons. We fill them one electron at a time (Hund's rule) first and then pair them up. So we put 6 electrons in the 2p orbitals as $\uparrow\downarrow\uparrow\downarrow\uparrow\downarrow$.
• Then fill the 3s orbital. The 3s orbital can hold 2 electrons, so we put two spin - paired electrons ($\uparrow\downarrow$) in the 3s box.
• Finally, fill the 3p orbitals. We have 4 remaining electrons for the 3p sub - shell. According to Hund's rule, we first put 3 unpaired electrons in the 3 p orbitals and then pair up the fourth electron. So we have $\uparrow\downarrow\uparrow\uparrow$ in the 3p orbitals.

Answer:

1s: $\uparrow\downarrow$ 2s: $\uparrow\downarrow$ 2p: $\uparrow\downarrow\uparrow\downarrow\uparrow\downarrow$ 3s: $\uparrow\downarrow$ 3p: $\uparrow\downarrow\uparrow\uparrow$