Which electron configuration violates hunds rule

Q: Which electron configuration follows Hunds rule?

Example of Hunds rule The electron configuration can be written as 1s 22s 22p 4. The orbital diagram is drawn as follows: the first 2 electrons will pair up in the 1s orbital; the next 2 electrons will pair up in the 2s orbital.

Video Transcript

Hello. So in this question were given now some electronic configuration and we have to say that which is which is not obeying the home's rule. Right? So here, first of all, let us see what happens. Rule states. Okay, so who wants law states that states So in the orbit tells in the good vitals of the same sub cell or vitals after same sub cell 18 tough sell. Right? So electrons are first electrons ours build singly first. Well simply first before pairing right before baring skirts before theory starts. Right. Disease the rules stated by ones. Right. So we were given some electronic configurations of the first days helium 18 to S two, two P X two then two P Y two and 23. And that one. Right, Well this is the first one. So here if you see here, first of all it is the U S is occupying two electrons then to pay excess of buying two electrons. Right then her to be wise of buying two electrons and two P chat. It's occupying one electron. Right? So as you can see here it is obeying right there it is open Now let us see for the 2nd 1. It is mobile nasty number three. So here give it is given hee to S two to be X two and two py one and two pieces. So if you see her first it is for the s orbital there two electrons are there for two PX there two electrons for to be why there is one electron but for two pigeons there is two electrons Right, first we have to pair this up. Then you have to filter second one. Right? So this is not correct. Right? This is not obeying the rules. Okay, in the C option C it is hee us too two PX 1 To be Y two and 2 pieces too. Similarly, we see here here before pairing up To be why it's filled, right? Which is not correct. So first of all to be X should be paired up then to be Y2 then to be checked to right? So this is also not obeying the rules. Okay then it is see number 30. So here again again you can write to S two to be exact to and to be vital. So this is opening right then again very given 80 to S two two PX 1 2 3 Y one and to feel that. Right? So here it is not opening. Right? There are two electrons are there. Then again one electron is occupying in the first or vital. Right? In the two PX orbital again to be one before very you know, to be satisfied. Right? So this is also not a window construed. So these particular cases are not obeying that is B C and E. Okay, so this is our answer. Thank you

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Video Transcript
What type of configuration violates Hund's rule?
How do you know if an electron configuration violates Hund's rule?
Which elements do not follow Hund's rule?
Which electron configuration follows Hund's rule?

Answer

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Hint: We know that the distribution of electrons in different orbitals is termed as electronic configuration. Three rules to be followed while deciding electronic configuration of an atom, they are, Hund’s rule, Pauli’s exclusion principle and Aufbau’s principle.

Complete step by step answer:
Let’s discuss Hund’s rule in detail. Hund’s rule states that each subshell in an orbital must be filled with one electron each before anyone is doubly occupied and the spin of all electrons in singly occupied shells is the same.

Let’s identify the correct answer from the options.

Option A is,

Here, in p orbital one subshell is vacant but one subshell is doubly filled or full filled. This type of electronic configuration violated the Hund’s rule.
Option B is,

Here, Hund’s rule is followed as all subshells are singly filled before getting doubly filled.
Option C is,

Here also Hund’s rule is followed as all subshells are singly filled.
Option D is,

Here also, Hund’s rule is followed as all subshells are singly filled first before getting doubly filled.
Therefore, in option A Hund’s rule is violated. Hence, the correct answer is option A.

Additional Information
According to Pauli’s exclusion principle, all subshells in an orbital can accommodate a maximum of two electrons and spin of both the electrons is opposite to each other.

Note:
Aufbau principle also must be followed while deciding electronic configuration of an atom. According to this principle, electrons should be filled in lower energy orbitals first and then should be filled in higher energy orbitals.

Question 1

Both electrons in the #"3s"# orbital have the same spin.

This violates the Pauli Exclusion Principle: No two electrons in the same orbital can have the same spin.

Question 2

You have no electrons in the #"2s"# orbital, which is between the #"1s"# and #"2p"# levels.

This violates the Aufbau Principle: When adding electrons to an atom, you put them in the lowest-energy orbitals available.

Question 3

You have two electrons in one #"2p"# orbital, but none in the other #"2p"# orbitals.

This violates Hund's Rule: There must be one electron with the same spin in each orbital of the same energy before you can put two in the same orbital.

Question 4

The electrons in the half-filled #"4d"# orbitals don't all have the same spin.

This violates Hund's Rule: There must be one electron with the same spin in each orbital of the same energy before you can put two in the same orbital.

Question 5

You filled the #"4d"# orbitals before you filled the #"4p"# orbitals, which are lower in energy.

This violates the Aufbau Principle.

What type of configuration violates Hund's rule?

Here, in p orbital one subshell is vacant but one subshell is doubly filled or full filled. This type of electronic configuration violated the Hund's rule.

How do you know if an electron configuration violates Hund's rule?

You have two electrons in one 2p orbital, but none in the other 2p orbitals. This violates Hund's Rule: There must be one electron with the same spin in each orbital of the same energy before you can put two in the same orbital. The electrons in the half-filled 4d orbitals don't all have the same spin.

Which elements do not follow Hund's rule?

In singly occupied orbitals, the electrons show the same spin. Electrons first fill the degenerate orbitals of similar energy. The first electron filled can be either spin up or spin down. Chromium and copper elements violate Hund's rule.

Which electron configuration follows Hund's rule?

Example of Hund's rule The electron configuration can be written as 1s ²2s ²2p ⁴. The orbital diagram is drawn as follows: the first 2 electrons will pair up in the 1s orbital; the next 2 electrons will pair up in the 2s orbital.

electron configuration violates hunds rule