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(C) The total number of nodes is given by $n-1$.The number of spherical (radial) nodes is given by $n-l-1$.The number of non-spherical (angular) nodes

Vedclass · Accepted Answer

One spherical and one non-spherical node

Vedclass · Answer

(C) The total number of nodes is given by $n-1$.The number of spherical (radial) nodes is given by $n-l-1$.The number of non-spherical (angular) nodes is given by $l$.For a $3p$ orbital,the principal quantum number $n = 3$ and the azimuthal quantum number $l = 1$.Therefore,the number of spherical nodes $= n-l-1 = 3-1-1 = 1$.The number of non-spherical nodes $= l = 1$.Thus,a $3p$ orbital has one spherical and one non-spherical node.

$A$ $3p$ orbital has

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