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What is the maximum number of electrons that can be identified with the following set of quantum numbers
n = 6
l = 1
ml = -1
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To determine the maximum number of electrons that can be identified with a given set of quantum numbers, you need to use the following rules:
1. The principal quantum number, denoted as "n", represents the energy level or shell of an electron. It can have values from 1 to infinity.
2. The azimuthal quantum number, denoted as "l", determines the shape of the electron's orbital. It can have values ranging from 0 to (n - 1).
3. The magnetic quantum number, denoted as "ml", specifies the orientation of the orbital in space. It can have integer values between -l and +l.
To find the maximum number of electrons, you need to consider the values of "n", "l", and "ml" and apply the rules.
In this case, the given values are:
n = 6
l = 1
ml = -1
Here's how you can find the maximum number of electrons:
1. Determine the maximum value of "ml" based on the value of "l":
- Since l = 1, ml can have values of -1, 0, and 1.
2. Use the formula to calculate the maximum number of electrons:
max electrons = 2(2l + 1)
3. Substitute the value of "l" into the formula:
max electrons = 2(2 * 1 + 1) = 2(3) = 6
Therefore, the maximum number of electrons that can be identified with the given set of quantum numbers (n = 6, l = 1, ml = -1) is 6.