Why period 3 elements can use their d orbitals...

[LyahFitzpatrick 2E]

I realize that once an atom obtains five electrons, they are able to occupy space in each s and p orbital with at least one electron. However, how does this then enable the d orbital to be used? Shouldn't the p orbital fill first? Is this just a phenomenon that happens to make covalent bonds work out?

[Michael Vigman 2D]

Consider that for each period, the quantum number n increases.

At period 3, n=3 and the d- orbital begins which means l can be 2 and ml can be -2, -1, 0, 1, 2. With 5 different subshells (-2 thru 2), it can hold 10 electrons.

*I'm not sure if I fully understood the question but perhaps this can clear up some stuff.

[Ashley Presnell 1C]

If an atom is trying to form more bonds than electrons that are able to be fit into the s and p orbitals, period 3 elements will fill their d-orbitals. Not 100% sure if I completely understood the question, but for example Sulfur can form 6 bonds to create SO4 (2-) because it starts to fill up the 3d orbital.

[Aneesha_Nema_3C]

Period 3 elements have an n value, which means that l can be 0, 1, or 2. This means that these elements have access to s, p , and d orbitals. The p-orbital does typically fill up first for ground-state electron configurations, but elements like P, S, or Cl can form more bonds than other atoms and hold more electrons in their d-orbital.

[Ruiyu Li 3I]

n for elements in period 3 is 3, so the values of l can be 0, 1, 2, which corresponds to s, p, and d subshell. Elements in period 3 will fill the electrons in s and p orbitals first in their ground state. If there are more electrons, the elements are able to accommodate them in their d orbitals.

[Rebekah Han 2K]

Is the d orbital used when an electron is excited? So would an electron jump from the p to the d orbital?

[905715668]

The d-orbital is added to a shell in period 3. That is why the 1st d-block of elements is called 3d.