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##### Asked by: Lashonda Monleon

science physics# What are the possible values of ML when L 2?

Last Updated: 12th February, 2020

**l**=

**2**, the

**possible**m

**l values**are −

**2**,−1,0,1,

**2**. Thistells us that the d subshell contains five d orbitals, each with adifferent orientation ( dyz , dxy , dxz ,dx

**2**−y

**2**, and dz

**2**).

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

The **values** of ml allowed range from -**l** to**l**, 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 by**ml**= -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 one**value** 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)