- #1
Feodalherren
- 605
- 6
Homework Statement
Why isn't (3, -2 , 0 , 1/2) a valid quantum number?
Homework Equations
The Attempt at a Solution
n=3
so l = -2 is valid.
-l≤Ml≤l
2≤Ml≤-2
nonsensical statement. I don't know what to do...
Feodalherren said:Homework Statement
Why isn't (3, -2 , 0 , 1/2) a valid quantum number?Homework Equations
The Attempt at a Solution
n=3
so l = -2 is valid.
-l≤Ml≤l
2≤Ml≤-2
nonsensical statement. I don't know what to do...
Quantum numbers are a set of four values used to describe the energy state and spatial orientation of an electron in an atom.
This combination of quantum numbers violates the Pauli exclusion principle, which states that no two electrons in the same atom can have the same set of quantum numbers. The third number, known as the magnetic quantum number, cannot have a value of -2 as it can only range from -l to l, where l is the orbital angular momentum quantum number, which in this case is 3. Therefore, the combination is invalid.
No, each electron in an atom must have a unique set of quantum numbers. This means that while (3,-2,0,1/2) may be valid for one electron, it cannot be used to describe another electron in the same atom.
The first three quantum numbers (n, l, and ml) determine the energy level, or shell, of the electron. The fourth quantum number (ms) determines the orientation of the electron within that energy level.
No, quantum numbers only describe the probability distribution of where an electron may be located in an atom. The exact location of an electron cannot be known due to the uncertainty principle in quantum mechanics.