Easy
For a given azimuthal quantum number $(l)$,the total number of magnetic quantum numbers $(m)$ is given by:
- A$l = \frac{(m + 1)}{2}$
- B$l = \frac{(m - 1)}{2}$
- C$l = \frac{(2m + 1)}{2}$
- D$l = \frac{(2m - 1)}{2}$
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Similar Questions
Which of the following explains the sequence of filling the electrons in different shells?
If the magnetic quantum number of a given orbital is represented by $-3$,then what will be the minimum possible value of its principal quantum number $(n)$?
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View SolutionWhich of the following orbitals has/have zero probability of finding the electron in the $xy$ plane?
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View SolutionMatch the items in List-$A$ with the items in List-$B$ and select the correct option.
List-$A$ List-$B$ $(1)$ Principal quantum number $(A)$ Shape of the orbital $(2)$ Azimuthal quantum number $(B)$ Spin of the electron $(3)$ Magnetic quantum number $(C)$ Orientation of the orbital in space $(4)$ Spin quantum number $(D)$ Size of the orbital
| List-$A$ | List-$B$ |
| $(1)$ Principal quantum number | $(A)$ Shape of the orbital |
| $(2)$ Azimuthal quantum number | $(B)$ Spin of the electron |
| $(3)$ Magnetic quantum number | $(C)$ Orientation of the orbital in space |
| $(4)$ Spin quantum number | $(D)$ Size of the orbital |
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View SolutionWhich of the following rules describes the order in which electrons fill various orbitals?
Medium
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