The state of an electron in a 3d_{z^2} orbita | vedclass

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(D) The state of an electron in an atom is fully described by four quantum numbers: principal quantum number $(n)$,azimuthal quantum number $(l)$,magn

Vedclass · Accepted Answer

$n, l, m$

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(D) The state of an electron in an atom is fully described by four quantum numbers: principal quantum number $(n)$,azimuthal quantum number $(l)$,magnetic quantum number $(m_l)$,and spin quantum number ($s$ or $m_s$).For a $3d_{z^2}$ orbital,the values are $n=3$ and $l=2$.The magnetic quantum number $(m_l)$ for $d$-orbitals ranges from $-2$ to $+2$.However,when specifying the state of an electron in a specific orbital,we define the orbital using $n, l,$ and $m_l$. The spin quantum number $(s)$ is also required to completely define the state of the electron.Since the question asks for the quantum numbers that describe the state of an electron in a specific orbital,$n, l,$ and $m$ are the spatial quantum numbers defining the orbital itself. Given the options,$n, l,$ and $m$ are the primary set defining the orbital state.

The state of an electron in a $3d_{z^2}$ orbital is described by which quantum numbers?

Similar Questions

Which of the following statements are correct for an electron that has $n = 4$ and $m = -2$?

Which of the following sequences is correct according to the Aufbau principle?

The number of electrons that can be accommodated in $d_{z^2}$ orbital is

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Statement $A$: In a potassium atom,the $19^{th}$ electron enters the $4s$-orbital instead of the $3d$-orbital.
Reason $R$: The $(n + l)$ rule is followed to determine the minimum energy of an orbital.

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