Answer:
In an atom, the quantum numbers n, l, and ml are used to describe the electronic configuration and distribution of electrons within the orbitals. The principal quantum number (n) represents the energy level or shell in which the electron resides. The azimuthal quantum number (l) determines the shape of the orbital, and the magnetic quantum number (ml) specifies the orientation of the orbital in space.
Given that n = 6, l = 3, and ml = 0, we can determine the number of orbitals in this particular atom.
The azimuthal quantum number (l) can have values ranging from 0 to (n-1). Therefore, for n = 6, l can take on values from 0 to 5. However, since l = 3 is specified in this case, it means that there are only orbitals with a shape corresponding to l = 3.
The magnetic quantum number (ml) can have values ranging from -l to +l. For l = 3, ml can take on values from -3 to +3. However, since ml = 0 is specified in this case, it means that there is only one orbital with an orientation corresponding to ml = 0.
Each orbital can accommodate a maximum of two electrons with opposite spins according to the Pauli exclusion principle. Therefore, the number of orbitals in an atom with n = 6, l = 3, and ml = 0 is 1.
To summarize:
- Principal quantum number (n): 6
- Azimuthal quantum number (l): 3
- Magnetic quantum number (ml): 0
- Number of orbitals: 1
Step-by-step explanation: