Question

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

• A. $d$-orbital
• B. $f$-orbital
• C. $s$-orbital
• D. $p$-orbital

Answer 1

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.

$Hencethecorrectanswerisoption\left(C\right)$