How many electrons in an atom can have each of the following quantum number or sublevel designations?
1. n=4, l=3
To determine the number of electrons in an atom with quantum number or sublevel designations, you need to use the formula 2(2l + 1).
For n = 4 and l = 3:
The quantum number n represents the principal energy level, and in this case, it is 4.
The quantum number l represents the azimuthal quantum number or the sublevel designation, which can range from 0 to (n-1). In this case, l = 3.
Using the formula: 2(2l + 1):
2(2 * 3 + 1) = 2(6 + 1) = 2(7) = 14
Therefore, the sublevel designation with n = 4 and l = 3 can hold a maximum of 14 electrons.
To determine the number of electrons that can have a certain set of quantum numbers, you need to use the following formula:
Number of Electrons = 2(2l + 1)
In this case, the quantum numbers are n=4 and l=3.
Using the formula, plug in the value of l into the equation:
Number of Electrons = 2(2(3) + 1)
= 2(6 + 1)
= 2(7)
= 14
Therefore, in an atom with n=4 and l=3, there can be a maximum of 14 electrons.