Question

Explain the following


1. Hund's Rule

2. Paule's principle


3. Aufbaus principle


4. Heisenberg principle

Answer 1

1) in the same subshell electrons cannot pair until all orbitals are singly occupied.
2) not any 2 electrons cannot hv same 4 quantum no.s . only 2 elctrons can be filled in same subshell with different spins
3)In ground state atoms are arranged in the increasig energy order.
4)at same time we cannot determine the exact position n momentum of electron.
hope it helps ot is nt tb lang. sorry abt that

Answer 2

Hey!
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(i)→ Hund's Rule states that in an atom , no electron pairing takes place until each orbital has at least one electron with the same spin.


For Example , Configuration of Oxygen ( O ) = 1s² 2s² 2 px² py¹ pz¹ according to this rule.


(ii)→ Paule's Principle states that an orbital can have a maximum of only 2 electrons . Because if they've more than 2 electrons , then they will have the same spin as well . This isn't possible . Hence , 2 electrons are only possible in an orbital.



(iii)→ Aufbau's Rule states that electrons are distributed in orbital according to their increasing energies.


For example , the configuration of Carbon ( C ) is = 1s² 2s² 2p² according to this rule.



(iv) Heisenberg's uncertainty principle states that it's impossible to measure simultaneously both the position as well as momentum of a macroscopic particle.


Expression : ∆X. ∆P ≥ h/4π


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