Which set of quantum numbers is not possible

In summary, the four quantum numbers (n, l, ml, and ms) are used to describe an electron's energy level, sublevel, orbital orientation, and spin direction. A possible set of quantum numbers must follow certain restrictions, such as the exclusion principle and the Pauli exclusion principle. Each electron can only have one unique set of quantum numbers. The azimuthal quantum number (l) determines the shape of an electron's orbital, with different sublevels having different shapes. There are limits to the possible values for each quantum number, with n being any positive integer, l ranging from 0 to (n-1), ml ranging from -l to +l, and ms only having values of +1/2 or -1
  • #1
Reptarous
1
0
Which set of quantum numbers is not possible?
a. N = 5, l =3 , ml = 0 , ms = -1/2
b. N = 1, l = 0, ml = 0 , ms = 1/2
c. N = 3 ,l = 2, ml = 1, ms = 1/2
d. N = 4, l = 3, ml = -3, ms = 1/2
e. N = 5, l = 2, ml = 0, ms = -1/2

They all look possible to me and there is no none of the above option in the question
 
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  • #2
i think the question is wrong :P
 
  • #3
Taken verbatim all these answers are perfectly correct sets of quantum numbers.

Perhaps what the question is trying to ask is "which of these do appear in the ground states of known elements". But I am just guessing/speculating.
 

Related to Which set of quantum numbers is not possible

1. What are the four quantum numbers and how are they used to describe an electron?

The four quantum numbers are the principal quantum number (n), the azimuthal quantum number (l), the magnetic quantum number (ml), and the spin quantum number (ms). These numbers are used to describe the energy level, sublevel, orbital orientation, and spin direction of an electron, respectively.

2. What is meant by a "possible" set of quantum numbers?

A possible set of quantum numbers refers to a combination of values for n, l, ml, and ms that are allowed according to the rules of quantum mechanics. These values must follow certain restrictions, such as the exclusion principle and the Pauli exclusion principle, in order to accurately describe the properties of an electron.

3. Can there be more than one set of quantum numbers for a single electron?

No, each electron in an atom can only have one unique set of quantum numbers. This is because each electron has its own specific energy level, sublevel, orbital orientation, and spin direction, and these properties cannot be shared by multiple electrons.

4. How do the quantum numbers determine the shape of an electron's orbital?

The azimuthal quantum number (l) determines the shape of an electron's orbital. This number corresponds to the different sublevels (s, p, d, f) in an energy level, which have different shapes. For example, the s sublevel is spherical, while the p sublevel is dumbbell-shaped.

5. Is there a limit to the possible values for each quantum number?

Yes, there are limits to the possible values for each quantum number. The principal quantum number (n) can have any positive integer value, while the azimuthal quantum number (l) can have values from 0 to (n-1). The magnetic quantum number (ml) can have values from -l to +l, and the spin quantum number (ms) can only have values of +1/2 or -1/2.

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