Which of the following is violating Hund's ru | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(D) Hund's rule of maximum multiplicity states that for a given electron configuration,the lowest energy term is the one with the greatest value of sp

Vedclass · Accepted Answer

All of the above

Vedclass · Answer

(D) Hund's rule of maximum multiplicity states that for a given electron configuration,the lowest energy term is the one with the greatest value of spin multiplicity. This means that electrons must occupy all available degenerate orbitals singly with parallel spins before pairing begins.In option $A$,the $2p^4$ configuration is shown as $(\uparrow)(\uparrow\downarrow)(\uparrow)$. This is a valid configuration as it follows the rule of filling orbitals singly before pairing.In option $B$,the $2p^2$ configuration is shown as $(\uparrow\downarrow)(	ext{empty})(	ext{empty})$. This violates Hund's rule because the electrons should have occupied separate orbitals with parallel spins $(\uparrow)(\uparrow)(	ext{empty})$ instead of pairing in the first orbital.In option $C$,the $2p^3$ configuration is shown as $(\uparrow)(\downarrow)(\uparrow)$. This violates Hund's rule because the electrons should have parallel spins $(\uparrow)(\uparrow)(\uparrow)$ when occupying degenerate orbitals singly.Since both $B$ and $C$ violate Hund's rule,the correct answer is $D$.

Which of the following is violating Hund's rule?

Similar Questions

Assertion :- In $H$-atom,the energy of $3d$-level is smaller than $4s$-level.
Reason :- In multi-electron species,an orbital with lower value of $(n+\ell)$ has energy smaller than the orbital with larger value of $(n+\ell)$.

The total number of atomic orbitals in the fourth energy level of an atom is

The number of orbitals in the $d$ sub-shell is

Which orbital is dumb-bell shaped?

Define the principal quantum number $(n)$.

Vedclass Test Series

Exam Paper Generator

Online Exam Module