Question

Assertion: p-orbital is dumb-bell shaped.
Reason: electrons present in p-orbital can have any one of the three values of magnetic quantum numbers, i.e., $0,{\text{ }} - 1{\text{ or }} + 1$.
A.Both Assertion and Reason are correct and the Reason is the correct explanation for Assertion.
B.Both Assertion and Reason are correct but the Reason is the not the correct explanation for Assertion.
C.Assertion is correct but the Reason is incorrect.
D.Assertion is incorrect but the Reason is correct.

Answer 1

Hint: There are different types of orbitals in a particular orbitals having different shapes. The number of the orbitals in a particular orbit is dependent upon the principal quantum number of the orbit.

Complete step by step answer:
The four commonly known subshells are the s, p, d, and f subshells. The number of subshells in an orbit is equal to 0 to \[\left( {n - 1} \right)\]where n is the principal quantum number. Each subshell has a certain number of orbitals which is dependent upon the azimuthal and the magnetic quantum numbers which is equal to \[\left( {{\text{2l + 1}}} \right)\]where l is the azimuthal quantum number.
For the second orbit, n = 2, hence the number of sub-shells are two with azimuthal quantum numbers 0 and 1 which are for the “s” and the “p” subshell respectively. Hence the magnetic quantum number is equal to 3 which are $\left( { - 1,0{\text{ or }} + 1} \right)$. For the p-orbitals as there is a response to the magnetic field in the $ - Z,0{\text{ and }} + Z$ axes so the p-orbitals get their dumbbell shape.
Hence, both the Both Assertion and Reason are correct and the Reason is the correct explanation for Assertion.

So, option A Is correct.

Note:
For the s-orbitals, the azimuthal quantum number is zero and hence the magnetic quantum number is also zero. So there is no response to the magnetic field along any of the axes, hence the shape of the orbital is spherical and hence there is an equal probability of finding the electrons in all the directions.