How many orbitals is/are possible with n=3,l= | vedclass

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(D) The symbol $n$ represents the principal quantum number (shell). The symbol $l$ represents the azimuthal quantum number (subshell),and $m_l$ repres

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$1$

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(D) The symbol $n$ represents the principal quantum number (shell). The symbol $l$ represents the azimuthal quantum number (subshell),and $m_l$ represents the magnetic quantum number (orientation of the orbital).Given $n=3$,$l=1$,and $m_l=-1$.For a given set of quantum numbers $(n, l, m_l)$,only one specific orbital is defined.Here,$n=3$ and $l=1$ corresponds to the $3p$ subshell,and $m_l=-1$ specifies one of the three $p$-orbitals (e.g.,$p_x$ or $p_y$).Thus,only $1$ orbital is possible for this specific set of quantum numbers.Therefore,option $(D)$ is the correct answer.

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

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