For which of following orbitals ,the value of magnetic quantum number is not zero
Answers
Answered by
0
The magnetic quantum number distinguishes the orbitals available within a subshell, and is used to calculate the azimuthal component of the orientation of orbital in space. Electrons in a particular subshell are defined by values of l.
The three quantum numbers (n, l, and m) that describe an orbital are integers:0, 1,2, 3, and so on. The principal quantum number (n) cannot be zero. The allowed values of n are therefore 1, 2, 3, 4, and so on. The angular quantum number (l) can be any integer between 0 and n - 1.And magnetic quantum number ranges from l to -l.
From all the given option 3s,2p
z
,3d
z
2
will have m=0 and hence option B is correct answer.
The three quantum numbers (n, l, and m) that describe an orbital are integers:0, 1,2, 3, and so on. The principal quantum number (n) cannot be zero. The allowed values of n are therefore 1, 2, 3, 4, and so on. The angular quantum number (l) can be any integer between 0 and n - 1.And magnetic quantum number ranges from l to -l.
From all the given option 3s,2p
z
,3d
z
2
will have m=0 and hence option B is correct answer.
Similar questions