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Question

An electron has a spin quantum number +1/2 and a magnetic quantum number āˆ’1. It cannot be present in:

A
d-orbital
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B
f-orbital
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C
s-orbital
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D
p-orbital
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Solution

The correct option is C s-orbital
Explanation:

The s subshell contains a single s orbital, so the magnetic quantum number, which tells you the orientation of the orbital that holds a given electron, can only take 1 possible value.s orbital cannot be described by a magnetic quantum number equal to 1.

For l=0, m value should be 0 indicates s orbital.
For l=1, m value should be 1,0,+1 indicates s,p orbitals.
For l=2, m value should be 2,1,0,+1,+2 indicates s,p,d orbitals.
For l=3, m value should be 3,2,1,0,+1,+2,+3 indicates s,p,d orbitals.

For l value 1 the electron may present in p or d or f orbital it cannot be in s orbital.

Hence the correct answer is option (C)





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