Which of the following orbitals will have 2 n | vedclass

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(A) For an orbital with principal quantum number $n$ and azimuthal quantum number $l$:$1.$ Number of angular nodes (nodal planes) $= l$$2.$ Number of

Vedclass · Accepted Answer

$5d$

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(A) For an orbital with principal quantum number $n$ and azimuthal quantum number $l$:$1.$ Number of angular nodes (nodal planes) $= l$$2.$ Number of radial nodes $= n - l - 1$$3.$ Total number of nodes $= (n - l - 1) + l = n - 1$Given: Number of nodal planes $= 2$,so $l = 2$ (which corresponds to a $d$-orbital).Given: Total nodes $= 4$,so $n - 1 = 4$,which implies $n = 5$.Therefore,the orbital is $5d$.

Which of the following orbitals will have $2$ nodal planes and $4$ total nodes?

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