Question

Which atomic orbitals of which subshells have a dumbbell shape?

Answer 1

We need to study atomic orbitals and their shapes in regards to subshells. For a better understanding of the geometry of electron orbitals, quantum theory and other characteristics of electron orbitals are used.

Complete answer:
One of three quantum numbers used to characterise an orbital, the main quantum number is one of the three quantum numbers. Unlike a regular orbit, atomic orbitals are broad regions in an atom where electrons are most likely to reside. When an electron is found in three-dimensional space surrounding a nucleus, a quantum mechanical model determines its probability. The angular momentum quantum number, $l$, is another quantum number. It is an integer that takes the values$l{\text{ }} = {\text{ }}0,{\text{ }}1,{\text{ }}2$,..., $n{\text{ }}-{\text{ }}1$and specifies the form of the orbital. This means that an orbital with $n{\text{ }} = {\text{ }}1$may only have one $l$ value, $l{\text{ }} = {\text{ }}0$, but an orbital with $n{\text{ }} = {\text{ }}2$can have $l{\text{ }} = {\text{ }}0$and$l{\text{ }} = {\text{ }}1$, and so on. The orbital's overall size and energy are defined by the main quantum number. The orbital's form is determined by the$l$ value. A subshell is formed by orbitals with the same $l$value. Furthermore, the angular momentum of an electron in this orbital is proportional to the angular momentum quantum number.
The $s$ subshells have a sphere-like form. The $s$orbital is present in both the $1n$ and $2n$ main shells, although the sphere in the $2n$ orbital is bigger. Each of the spheres represents a single orbital. Three dumbbell-shaped orbitals make up $p$ subshells. Shell $1$ does not have a $p$ subshell, but principal shell $2n$ does.

Fig: dumbbell-shaped orbitals make up $p$ subshells (x,y and z axis)

Note:
Note that $s$ orbitals are orbitals with$l{\text{ }} = {\text{ }}0$.The $p$ orbitals are represented by the value l{\text{ }} = {\text{ }}1.$$$p$ orbitals form a $p$ subshell for a given $n$ (e.g., 3p$for$n{\text{ }} = {\text{ }}3$). The$d$orbitals are those with$l{\text{ }} = {\text{ }}2$, followed by the$f - ,{\text{ }}g - ,$and$h - $orbitals with$l{\text{ }} = {\text{ }}3,{\text{ }}4,{\text{ }}5,$$and higher values.