(A) The shape of an orbital is determined by the azimuthal quantum number $(l)$. For both $2p$ and $3p$ orbitals,the value of $l$ is $1$,which corresp

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(A) The shape of an orbital is determined by the azimuthal quantum number $(l)$. For both $2p$ and $3p$ orbitals,the value of $l$ is $1$,which corresponds to a dumb-bell shape. Therefore,they have the same shape. They differ in size,energy,and the value of the principal quantum number $(n)$.

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

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There is no difference between a $2p$ and a $3p$ orbital regarding

A
Shape
B
Size
C
Energy
D
Value of $n$

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Structure of Atom

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Quantum number, Electronic configuration and Shape of orbitals

Which quantum number determines the shape of the subshell?

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Which of the following electronic configurations is not possible according to Hund's rule?

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Show the distribution of electrons in an oxygen atom (atomic number $8$) using an orbital diagram.

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$(a)$ How many sub-shells are associated with $n=4?$
$(b)$ How many electrons will be present in the sub-shells having $m_{s}$ value of $-1/2$ for $n=4?$

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For $s-$orbitals,since $\psi$ (orbital) is independent of angles,the probability $(\psi^2)$ is

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There is no difference between a $2p$ and a $3p$ orbital regarding

Similar Questions

Which quantum number determines the shape of the subshell?

Which of the following electronic configurations is not possible according to Hund's rule?

Show the distribution of electrons in an oxygen atom (atomic number $8$) using an orbital diagram.

$(a)$ How many sub-shells are associated with $n=4?$$(b)$ How many electrons will be present in the sub-shells having $m_{s}$ value of $-1/2$ for $n=4?$

For $s-$orbitals,since $\psi$ (orbital) is independent of angles,the probability $(\psi^2)$ is

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$(a)$ How many sub-shells are associated with $n=4?$
$(b)$ How many electrons will be present in the sub-shells having $m_{s}$ value of $-1/2$ for $n=4?$