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Which atomic orbitals of which subshells have a dumbbell shape?

Answer
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Hint: 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 valuesl = 0, 1, 2,..., n  1and specifies the form of the orbital. This means that an orbital with n = 1may only have one l value, l = 0, but an orbital with n = 2can have l = 0andl = 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 thel value. A subshell is formed by orbitals with the same lvalue. 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 sorbital 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.
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Fig: dumbbell-shaped orbitals make up p subshells (x,y and z axis)

Note:
Note that s orbitals are orbitals withl = 0.The p orbitals are represented by the value l = 1.p orbitals form a p subshell for a given n (e.g., 3pforn = 3). The dorbitals are those withl = 2, followed by the f, g,and horbitals with l = 3, 4, 5,and higher values.
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