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Question

(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.

List-$I$ (Quantum number)	List-$II$ (Orbital)
$a. n=2, \ell=1$	$i. 2s$
$b. n=3, \ell=2$	$ii. 3s$
$c. n=3, \ell=0$	$iii. 2p$
$d. n=2, \ell=0$	$iv. 3d$

$A$ $3p$ orbital has

Similar Questions

Match List-$I$ with List-$II$ :
List-$I$ (Quantum number) List-$II$ (Orbital)
$a. n=2, \ell=1$ $i. 2s$
$b. n=3, \ell=2$ $ii. 3s$
$c. n=3, \ell=0$ $iii. 2p$
$d. n=2, \ell=0$ $iv. 3d$

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