How does a $2 p_{x}$ orbital differ from $2 p_{y}$ orbital?

Answer

Verified

469.8k+ views

1 likes

Hint: Orbital is the space around an atom where the probability of finding the electron is very high. Both orbitals have the same value of the quantum number. They differ in the orientation in space.

Complete step by step answer:
We know that an atomic orbital is a mathematical entity which explains the wave-like behaviour of an electron or a pair of electrons present in an atom. It is known to calculate the probability of finding an electron in a region around the nucleus. The entity corresponds to the physical space where the electron can be ought to be present, as known by the mathematical form of the orbital. The orbitals have the same size and energy and shape but are oriented differently in space (different magnetic quantum numbers).

Let’s understand the differences between

2 p_{x}

and

2 p_{y}

orbitals are as follows:

$2 p_{x}$	$2 p_{y}$
1) The $2 p_{x}$ orbital is on the x-axis	1) $2 p_{y}$ orbital has its lobes along the y-axis
2) $2 p_{x}$ has its electron density along the x-axis a	2) $2 p_{y}$ has its electron density along the y-axis.

Additional information:
These orbitals (

2 p_{x}

2 p_{y}

) are of the same energy and degenerate orbitals. They have the same energy and the same shape. They are just three-fold degenerate orbitals and differ in the orientation of the orbitals in shape. Every orbital in an atom is known by a unique set of values of the three quantum numbers n, l, and m, which corresponds to the electron's energy, angular momentum, and an angular momentum vector component.

Note: All the three p orbitals have the same energy since they are identical and reside in the same energy level. The shapes are also the same since the principal quantum number is also the same. All have an identical energy level.