(C) According to the $(n+l)$ rule,the energy of an orbital is determined by the sum of its principal quantum number $(n)$ and azimuthal quantum number

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(C) According to the $(n+l)$ rule,the energy of an orbital is determined by the sum of its principal quantum number $(n)$ and azimuthal quantum number $(l)$.For $4s$ orbital: $n = 4, l = 0$,so $(n+l) = 4 + 0 = 4$.For $3d$ orbital: $n = 3, l = 2$,so $(n+l) = 3 + 2 = 5$.Since the $(n+l)$ value for $4s$ is less than that of $3d$,the $4s$ orbital has lower energy than the $3d$ orbital. Thus,$4s < 3d$.

Class 11 Chemistry Structure of Atom Quantum number, Electronic configuration and Shape of orbitals

Medium

In a potassium atom,the electronic energy levels are in the following order:

A
$4s > 3d$
B
$4s < 2p$
C
$4s < 3d$
D
$4s > 4p$

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Structure of Atom

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Quantum number, Electronic configuration and Shape of orbitals

Which of the following elements has the outer electronic configuration $3s^2 3p^5$?

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According to the Aufbau principle,what is the correct order of energy for $3d$,$4s$,and $4p$ orbitals?

Medium

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The angular momentum of an electron in a $d$ orbital is equal to:

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For a one-electron atom,the set of allowed quantum numbers is

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Match the $LIST$-$I$ with $LIST$-$II$:
List-$I$ (Orbital) List-$II$ (Radial nodes and nodal plane)
$A$. $2s$ $I$. $1$ Radial node + two nodal planes
$B$. $3s$ $II$. $1$ Radial node + one nodal plane
$C$. $3p$ $III$. $2$ Radial nodes + No nodal plane
$D$. $4d$ $IV$. $1$ Radial node + No nodal plane

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List-$I$ (Orbital)	List-$II$ (Radial nodes and nodal plane)
$A$. $2s$	$I$. $1$ Radial node + two nodal planes
$B$. $3s$	$II$. $1$ Radial node + one nodal plane
$C$. $3p$	$III$. $2$ Radial nodes + No nodal plane
$D$. $4d$	$IV$. $1$ Radial node + No nodal plane

In a potassium atom,the electronic energy levels are in the following order:

Similar Questions

Which of the following elements has the outer electronic configuration $3s^2 3p^5$?

According to the Aufbau principle,what is the correct order of energy for $3d$,$4s$,and $4p$ orbitals?

The angular momentum of an electron in a $d$ orbital is equal to:

For a one-electron atom,the set of allowed quantum numbers is

Match the $LIST$-$I$ with $LIST$-$II$:List-$I$ (Orbital)List-$II$ (Radial nodes and nodal plane)$A$. $2s$$I$. $1$ Radial node + two nodal planes$B$. $3s$$II$. $1$ Radial node + one nodal plane$C$. $3p$$III$. $2$ Radial nodes + No nodal plane$D$. $4d$$IV$. $1$ Radial node + No nodal plane

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Match the $LIST$-$I$ with $LIST$-$II$:
List-$I$ (Orbital) List-$II$ (Radial nodes and nodal plane)
$A$. $2s$ $I$. $1$ Radial node + two nodal planes
$B$. $3s$ $II$. $1$ Radial node + one nodal plane
$C$. $3p$ $III$. $2$ Radial nodes + No nodal plane
$D$. $4d$ $IV$. $1$ Radial node + No nodal plane