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Hello,
Just a question regarding the magnetic quantum number. Assuming for a second that we are referring to the d-subshell (which contains 5 orbitals), the magnetic quantum number describing an electron can be defined as any one of 5 possible values (-2, -1, 0, 1, or 2). By convention, we number the orbitals within any given subshell in increasing order (as I just showed). However, other sources claim that the electron we are describing can be defined by any number ranging from -2 to 2. For instance lets say I am describing this electron in a d-orbital.
__ __ _l_ __ __
By convention (according to TBR), this electron would have a a magnetic quantum number of 0. However, other sources claim that this electron can be represented by any number ranging from -2 to 2. It can be 1, 0, 2, -2, or -1.
Does the MCAT follow convention or should I expect that they wouldn't?
Just a question regarding the magnetic quantum number. Assuming for a second that we are referring to the d-subshell (which contains 5 orbitals), the magnetic quantum number describing an electron can be defined as any one of 5 possible values (-2, -1, 0, 1, or 2). By convention, we number the orbitals within any given subshell in increasing order (as I just showed). However, other sources claim that the electron we are describing can be defined by any number ranging from -2 to 2. For instance lets say I am describing this electron in a d-orbital.
__ __ _l_ __ __
By convention (according to TBR), this electron would have a a magnetic quantum number of 0. However, other sources claim that this electron can be represented by any number ranging from -2 to 2. It can be 1, 0, 2, -2, or -1.
Does the MCAT follow convention or should I expect that they wouldn't?