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(NONE) For a given principal quantum number $n = 2$,the possible values of the azimuthal quantum number $l$ are $0$ and $1$.For $l = 0$ ($s$-orbital),

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$3$

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(NONE) For a given principal quantum number $n = 2$,the possible values of the azimuthal quantum number $l$ are $0$ and $1$.For $l = 0$ ($s$-orbital),the magnetic quantum number $m_l$ can only be $0$.For $l = 1$ ($p$-orbital),the magnetic quantum number $m_l$ can be $-1, 0, +1$.Thus,for $n = 2$,the possible values for the magnetic quantum number are $0, -1, 0, +1$,which gives a total of $4$ values.

The magnetic quantum number for an electron when the value of principal quantum number is $2$ can have ............ values.

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