Question

Write the names of the orbital of the following quantum numbers. \[n = 2,l = 0\]

Answer 1

Hint: Orbital is the place where electrons are occupied in an atom. Quantum numbers help to locate an electron in an atom to its respective orbitals. Orbitals can be represented as s-.p-,d- and f- orbitals. Each orbital has different orientations in space. Orbital can occupy a maximum of two electrons. Generally, the s-subshell has one orbital, the p-subshell has 3 orbitals, the d-subshell has 5 orbitals and the f-subshell has 7 orbitals.

Complete step by step answer:
Quantum number helps to locate an electron in an atom to its respective orbitals. Principal quantum number (n) defines that each shell is characterized by this quantum number. It has the values from 1,2,3,.....etc. Azimuthal quantum number (l) represents the difference in energy levels and different shapes of orbitals. It has values from \[0 \to (n - 1)\] where n-Principal quantum number.
If \[l = 0\], then it symbolizes that it is s- orbital.
If \[l = 1\], then it symbolizes that it is p- orbital.
If \[l = 2\], then it symbolizes that it is d- orbital.
If \[l = 3\], then it symbolizes that it is f- orbital.
Thus, If \[n = 2,l = 0\], then it symbolises that the given orbital is 2s orbital.

Note: Generally, the quantum number is of four types. They are principal quantum number (n), Azimuthal quantum number (l), magnetic quantum number (m), and spin quantum number (s).
Magnetic quantum number (m) helps to define the orientations of orbitals in space. It has the values from \[ - l \to + l\] where l-Azimuthal quantum number. Spin quantum number (s) defines the rotation of electrons in an atom. It has two values namely \[ - \dfrac{l}{2}\] and \[ + \dfrac{l}{2}\].