Question

Write the electronic configuration of chromium and copper?

Answer 1

Hint: Before writing the electronic configuration you should know that the electronic configuration of chromium and copper is called an exceptional electronic configuration. Now you can use these to answer your question.

Complete step by step answer:

First of all, you should know that some elements do not follow the Aufbau principle, there are some alternate ways that electrons can arrange themselves that give these elements better stability.
Using the Aufbau principle, you would write the following electron configurations
Cr = $[Ar]4s^{ 2 }3d^{ 4 }$
Cu = $[Ar]4s^{ 2 }3d^{ 9 }$
The actual electron configurations are:
Cr = $[Ar]4s^{ 1 }3d^{ 5 }$
Cu = $[Ar]4s^{ 1 }3d^{ 5 }$
To understand why this occurs, it is important to realize that
Completely filled sublevels are more stable than partially filled sublevels.
A sublevel which is exactly half filled is more stable than a partially filled sublevel which is not half full.
Electrons are lazy and will do whatever places them in the lowest energy state = which is the most stable state
In both examples, an electron moves from the 4s sublevel to produce a half-filled 3d(Cr) or completely filled 3d(Cu). This gives the atom greater stability so the change is favorable.

Therefore, we have written the electronic configuration of chromium and copper.

Note: It is important to note that this explanation is just looking at the examples of Cr and Cu. There are other elements which will have exceptions to the rules we have come up with to predict electron configurations. For example, W will follow the Aufbau principle and not display behavior like that of Cr. This is due to the fact that the atoms and electrons know nothing of the rules we (humans) come up with to try to explain and predict their behavior.