Asked by: Lashonda Monleon
science physics

What are the possible values of ML when L 2?

Last Updated: 12th February, 2020

Therefore, given l=2 , the possibleml values are −2,−1,0,1,2 . Thistells us that the d subshell contains five d orbitals, each with adifferent orientation ( dyz , dxy , dxz ,dx2−y2 , and dz2 ).

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Also question is, what values of m1 are possible for L 2?

The values of ml allowed range from -l tol, therefore a 6d sub shell would have values-2,-1,0,1, and 2 (5 values).

Subsequently, question is, what are the possible values of ML for this orbital? The values of the magnetic quantum number are thenegative and positive values of l. As described above, the ssubshell has one orientation, since it is spherical and l=0. The psubshell has three orientations, represented by ml= -1, 0,1. The d subshell has five orbitals represented byml= -2, -1, 0, 1, 2.

Accordingly, what are the possible values of the magnetic quantum number ml?

Magnetic Quantum Number (ml): ml =-l, , 0, , +l. Specifies the orientation in space of an orbital ofa given energy (n) and shape (l). This number divides thesubshell into individual orbitals which hold the electrons; thereare 2l+1 orbitals in each subshell.

What values of L are possible for n 3?

When n = 1, l= 0 (l takes on onevalue and thus there can only be one subshell) When n= 2, l= 0, 1 (l takes on two values and thusthere are two possible subshells) When n = 3,l= 0, 1, 2 (l takes on three values and thusthere are three possible subshells)

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