(Polar molecules, Non-polar molecules, etc.)
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The magnetic quantum number can range from -l to +l. One thing to note, however, is that only integer values are allowed for the magnetic quantum number. For instance, if l=2, the magnetic quantum number could be -2, -1, 0, 1, or 2.
Hi, I don't believe there is a way for us to determine the magnetic quantum number (ml) a specific electron has without doing an experiment. Thus, we will most likely not be asked about a specific ml number. Rather it is more likely that we will be asked about the range such as on the previous quiz. Hope this helps!
804899546 wrote:Is there any way for us to tell exactly what magnetic quantum number an electron would have within an orbital without doing an experiment? Will we ever be asked which magnetic quantum number an electron has?
By convention, the first half of any orbital (d1 - d5) has +1/2 spins while the latter half (d6 - d10) has -1/2 spins.
Also, notice how there are 5 elements in the first half of a d orbital and 5 elements in the latter half - 10 elements in each d orbital in total. This corresponds to magnetic quantum numbers -2 for the first element, -1 for the second element, 0 for the third element, 1 for the fourth element and 2 for the fifth element of each half.
The Principal quantum n would usually be given to you for you to solve. To find l you subtract n-1 which could take on the values 0,1,2,3,4..... and remember that l is also the subshell in which 0=s, 1=p, 2=d, 3=f. The value of m sub l is what ever l is such as l=2 m sub l equal both the negative and positive integer of that number and all those numbers between it such as l=2 m sub l = -2, -1, 0, 1, 2 and m sub s is also equal to plus or minus one half.
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