An orbital is explained by the principle quantum number, #n#, the angular inert quantum number, #l#, and also the magnetic quantum number, #m_l#. An electron is described by every of these quantum numbers, v the enhancement of the electron rotate quantum number, #m_s#.

The **principle quantum number** , #n#, is the energy and also distance from the nucleus, and represents the shell.

The #3d# orbital is in the #n=3# shell, similar to the #2p# and also #2s# orbitals space in the #n = 2# shell.

The **angular momentum quantum number** , #l#, defines the form of the orbit or subshell, whereby #l=0,1,2,3...# synchronizes to #s, p, d, # and also #f# orbitals, respectively.

Therefore, a #d# orbital has actually an #l# value of #2#. The is worth noting that each shell has actually up to #n-1# types of orbitals.

For example, the #n=3# shell has orbitals that #l=0,1,2#, which method the #n=3# shell contains #s#, #p#, and #d# subshells. The #n=2# shell has actually #l=0,1#, therefore it has only #s# and #p# subshells.

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The **magnetic quantum number** , #m_l#, explains the orientation that the orbitals (within the subshells) in space. The feasible values because that #m_l# the any type of orbital (#s,p,d,f...#) is provided by any type of integer worth from #-l# come #l#.

So, for a #3d# orbital v #n=3# and also #l=2#, we deserve to have #m_1=-2,-1,0,1,2#. This tells us that the #d# orbital has actually #5# possible orientations in space.

If you"ve learned anything about group theory and also symmetry in chemistry, because that example, you can vaguely remember having actually to attend to various orientations the orbitals. Because that the #d# orbital, those room #d_(yz)#, #d_(xy)#, #d_(xz)#, #d_(x^2-y^2)#, and also #d_(z^2)#. So, we would certainly say the the #3d# subshell includes #5# #3d# orbitals (shown below).

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Finally, the **electron spin quantum number**, #m_s#, has actually only two feasible values, #+1/2 and -1/2#. As the name implies, this values explain the turn of every electron in the orbital.

Remember that there are just two electron to every orbital, and that they should have actually opposite spins (think Pauli exclusion principle). This tells us that there room two electrons per orbital, or per #m_l# value, one with an #m_s# worth of #+1/2# and also one v an #m_s# value of #-1/2#.

**(Tl;dr)** Thus, as declared above, each individual #3d# orbital have the right to hold #2# electrons. Since there are five #3d# orbitals in the #3d# subshell, the #3d# subshell have the right to hold #10# electrons full (#5*2#).