(A) The magnetic quantum number $m_l$ depends on the azimuthal quantum number $l$,where $m_l$ ranges from $-l$ to $+l$.For an $s$-orbital,$l = 0$,so $

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(A) The magnetic quantum number $m_l$ depends on the azimuthal quantum number $l$,where $m_l$ ranges from $-l$ to $+l$.For an $s$-orbital,$l = 0$,so $m_l$ can only be $0$.Since the given value is $m_l = -1$,it is impossible for an electron to be in an $s$-orbital because $m_l$ cannot be $-1$ when $l = 0$.Therefore,the correct option is $A$.

Class 11 Chemistry Structure of Atom Quantum number, Electronic configuration and Shape of orbitals

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For an electron with quantum numbers $s = +1/2$ and $m_l = -1$,which of the following orbitals is not possible?

A
$s$
B
$p$
C
$d$
D
$f$

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Class 11 Questions

Class 11

Chemistry Questions

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Structure of Atom

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Quantum number, Electronic configuration and Shape of orbitals

The correct set of quantum numbers for the unpaired electron of $Cu$ atom is

MediumKVPY 2020

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In an atom, the order of increasing energy of electrons with quantum numbers $(i)$ $n=4, l=1$, (ii) $n=4, l=0$, (iii) $n=3, l=2$, and (iv) $n=3, l=1$ is:

MediumAP EAMCET 2014

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Which of the following is the correct electronic configuration of $Cr$ (Chromium)?

Easy

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How many orbitals is/are possible with $n=3$,$l=1$ and $m_l=-1$ values?

EasyAP EAMCET 2019

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Which of the following electronic configurations is not possible according to Hund's rule?

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For an electron with quantum numbers $s = +1/2$ and $m_l = -1$,which of the following orbitals is not possible?

Similar Questions

The correct set of quantum numbers for the unpaired electron of $Cu$ atom is

In an atom, the order of increasing energy of electrons with quantum numbers $(i)$ $n=4, l=1$, (ii) $n=4, l=0$, (iii) $n=3, l=2$, and (iv) $n=3, l=1$ is:

Which of the following is the correct electronic configuration of $Cr$ (Chromium)?

How many orbitals is/are possible with $n=3$,$l=1$ and $m_l=-1$ values?

Which of the following electronic configurations is not possible according to Hund's rule?

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