Write about $p$-orbitals.

(N/A) Presence of $p$-orbital: $p$-orbitals are possible for $n = 2, 3, 4, \ldots$ (i.e.,$2p, 3p, 4p, \ldots$),but $1p$ is not possible. For a $p$-orbital,the azimuthal quantum number $l = 1$. Since $l$ can range from $0$ to $n-1$,for $n=1$,$l$ can only be $0$ ($s$-orbital). Thus,$p$-orbitals are not possible in the first shell.
Boundary surface for $p$-orbital: $p$-orbitals have a dumbbell shape. Each $p$-orbital consists of two lobes.
These two lobes are located on opposite sides of the nucleus. The region where the two lobes meet is a nodal plane where the probability of finding an electron is zero.
Number of $p$-orbitals: For $l = 1$,the number of $p$-orbitals is given by $(2l + 1) = 2(1) + 1 = 3$. These are designated as $p_x, p_y,$ and $p_z$. For any $n > 1$,there are three $p$-orbitals.
Energy of $p$-orbitals: In a given subshell,all three $p$-orbitals $(p_x, p_y, p_z)$ are degenerate,meaning they have the same shape,size,and energy. The number of radial nodes is given by $(n - l - 1)$. For $3p$,radial nodes $= 3 - 1 - 1 = 1$. For $4p$,radial nodes $= 4 - 1 - 1 = 2$.
Energy order: As the principal quantum number $n$ increases,the energy of the $p$-orbitals increases. Thus,the energy order is $2p < 3p < 4p < 5p < \ldots$.