Question

Which of the following is not a valid set of quantum numbers? A) n = 3, l = 0, ml = 0, and ms = 1/2 B) n = 2, l = 1, ml = -1, and ms = -1/2 C) n = 3, l = 2, ml = 3, and ms = 1/2 D) n = 2, l = 1, ml = 0, and ms = -1/2

Answer 1

Answer:

C) n = 3, l = 2, ml = 3, and ms = 1/2

Explanation:

• n = The principal quantum number. It gives the electron shell, or energy level, of an electron. The value of n ranges from 1 to the shell containing the valence electron of that atom

• l = The angular momentum quantum number. It gives the subshell and gives the magnitude of the orbital angular momentum through the relation. The value of l ranges from 0 to (n-1

        n= 3 hence l can take 0,1,2. Thus 2 is a valid number

• ml = The magnetic quantum number. It gives the specific orbital within that subshell and gives the projection of the orbital angular momentum along a specified axis. The value of ml can range from (-l) to ((+l)

Here ml can take values of -2,-1,0,1,2. hence m= 3 is not valid quantum        number for l= 2

• ms = The spin quantum number. It gives the intrinsic spin angular momentum of the electron within each orbital and describes the projection of the spin angular momentum along the specified axis. It can the values of +(1÷2) or -(1÷2)