Question

How does an $2s$ orbital differ from $2p$ orbital?

Answer 1

Hint : We know that the atom is the smallest unit of matter in nature. The atom comprises electrons in the orbitals; neutrons and protons in the nucleus. The orbitals present in an atom are s, p, d and f according to the energy differences they have amongst them.

Complete Step By Step Answer:
Let us see the two orbitals i.e. $2s$ and $2p$ in detail;
$2s$ orbital: This orbital will have higher energy than that of $1s$ whereas; will be less energetic than other orbitals. It would be the next closest orbital from the nucleus after $1s$ orbital. The radius of $2s$ orbital will be larger than that of $1s$ orbital. After $1s$ the electrons will fill us $2s$ orbital. - Here, ‘n’ in the term ‘ns’ determines the principal quantum number and’ represents the subshell; the shape of the orbital. The s orbitals are spherically symmetrical amongst the nucleus of an atom
The most important difference between these two orbitals is that the probability of finding the electron decreases as we move away from the nucleus. Thus, the probability will be more in $1s$ orbital but will decrease in $2s$ orbital.
$2p$ orbital: This orbital has the lowest energy among all the corresponding orbitals and is located closest to the nucleus. The radius of $2p$ will be smaller than that of other orbitals i.e. it would be a smallest sphere. Electrons will be firstly filled into the $2p$ orbital as compared to other orbitals.

Note :
Note that the energy of the orbitals can be calculated by $n\text{ }+\text{ }l$ rule which will prove the fact of energy differences between the $1s$ and $2s$ orbitals. Also, do note that the radial node will be present in $2s$ orbital.