Multiple Choice
In one atom, what is the maximum number of electrons that can have the principal quantum number n = 2?
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9. Quantum Mechanics
Quantum Numbers: Number of Electrons
Multiple Choice
Determine the number of electrons that can have the following set of quantum numbers:n = 3, ml = 0.
A
2 e-
B
4 e-
C
6 e-
D
3 e-
Verified step by step guidance1
Understand the quantum numbers: The principal quantum number (n) indicates the energy level, and the magnetic quantum number (ml) specifies the orientation of the orbital within a subshell.
Identify the possible values for the azimuthal quantum number (l) when n = 3. The possible values for l are 0, 1, and 2, corresponding to the s, p, and d subshells, respectively.
Determine which subshells can have ml = 0. For l = 0 (s subshell), ml = 0 is possible. For l = 1 (p subshell), ml = 0 is also possible. For l = 2 (d subshell), ml = 0 is possible as well.
Calculate the number of electrons for each subshell with ml = 0. Each orbital can hold a maximum of 2 electrons. Therefore, for each subshell (s, p, and d) with ml = 0, there can be 2 electrons.
Sum the electrons from each subshell: 2 electrons from the s subshell, 2 electrons from the p subshell, and 2 electrons from the d subshell, resulting in a total of 6 electrons that can have the given set of quantum numbers.
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