Quantum Numbers

[Natalie Flores 1F]

Hi! I'm having a hard time with quantum numbers but more so with ml for orbitals. Why are the numbers for it -2,-1,0,1,2 or -1,0,1 and where did they come from? Thank you!!

[Lauren Woodward 1I]

Ml is the magnetic quantum number and is essentially a range of numbers that is given by the value of l. The allowed values of ml range from l to -l, so if l=2, the range would be +2, +1, 0, -1, -2. It also describes the number of orbitals in each subshell. The range of p is +1, 0, -1, meaning that the p subshell has 5 orbitals. Hope this helps at least a little!

[Preethika Praveen 2G]

Hi! The number of orbitals are determined from the angular momentum quantum number, l. l is the number of subshells per principal energy level determined by l=n-1. ml is the magnetic quantum number and can be determined by ml=2l+1. The possible values of ml range from -l to +l. Therefore, for l= 1, there are three possible orientations (-1, 0, 1) and for l=2, there would be five possible orientations (-2,-1,0,1,2)

[LaurenAkason2A]

Hey!! I was having a really hard time with quantum numbers too and then I watched the organic chemistry tutor youtube video called " maximum number of electrons" and it was sooo helpful! I highly recommend watching this video if you're struggling with this concept. Hope this helps!!!

[Alice Guey 1B]

The numbers for each of the four quantum numbers are just a convention. For the magnetic quantum number of an atom, specifically, it is easier to remember that its absolute value will not exceed the angular momentum quantum number. If an atom has an angular momentum quantum number of 2, then its range of possible magnetic quantum numbers spans from -2 to 2.