Question

How many nodes are in a $2p$ orbital?

Answer 1

Hint: A node is a site where the probability of an electron is zero. There are two sorts of nodes for each orbital. Radial node and Angular node. The wave nature of electrons (or electron pairs) in an atom is described by atomic orbitals, which are mathematical functions.

Complete answer:
The total number of nodes in $2p$ orbital is $0$.
The total number of nodes is determined by $n - l - 1$ . Here , $n$ is the principal quantum number and
$l$ is the azimuthal quantum number.
$n = 2$ , $l = 1$
$2 - 1 - 1 = 0$
The $p$ orbitals are formed like dumbbells. The $p$ orbital node is located at the centre of the nucleus. Due to the presence of three orbitals, the $p$ orbital may hold a maximum of six electrons. The three $p$ orbitals are perpendicular to one another. The size of the $p$ orbitals is determined by the primary quantum number $n$ , with $4p > 3p > 2p$ being the most common.
On either side of the plane that goes through the nucleus, each $p$ orbital comprises parts known as lobes. At the point where the two lobes intersect, the chances of discovering an electron are zero.

Additional information: In an atom, a shell is a collection of subshells belonging to the same quantum number theory, $n$ . Orbitals each have two electrons, and electrons in the same orbital have the same size, angular momentum size, and magnetic quantum number values.

Note:
Sharp, primary, diffuse, and fundamental are represented by the letters $s,p,d,f$ respectively. The letters and words refer to the fine structure of the spectral lines that results from the first fundamental corrections, particularly the spin-orbital interaction.