Question

18. All of the following sets of quantum numbers are allowed EXCEPT a. n = 1, = 0, = 0 b. n = 2, = 2, = +1 c. n = 3, = 1, = –1 d. n = 4, = 1, = 0 e. n = 5, = 4, = –3

Answer 1

Answer:

b

Explanation:

it is impossible for n & l to be equal

Answer 2

There are 4 quantum numbers:

1. Principal Quantum number $(n)$ specifies the energy of the electron in a shell.
2. Azimuthal Quantum number $(l)$ specifies the shape of an orbital. The value of it lies in the range of 0 to (n-1)
3. Magnetic Quantum number $(m)$ specifies the orientation of the orbital in space. The value of it lies in the range of -l to +l
4. Spin Quantum number $(s)$ specifies the spin of an electron in an orbital. It can either have a value of $+\frac{1}{2}$ or $-\frac{1}{2}$

To find the forbidden set, we need to know the following facts about quantum numbers:

• The value of $l$ will always be less than the value of $n$
• The value of $m$ and [/tex]l[/tex[ be be equal to 0 but the value of $n$ can never be equal to 0.

Thus, we can say that the option that affirms that n = 2, l = 2, m = +1 is forbidden because the value of $l$ is equal to the value of $n$.

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