Question

write about short note on fallowing?
a) Pauli exelusion principle
b) Hund Rule of manimum Miltiplicity
c) Auf bau Rule
d) n+l Rule​

Answer 1

Answer:

here is your answer!!

Hunds Rule of Maximum Multiplicity rule states that for a given electron configuration, the term with maximum multiplicity falls lowest in energy. According to this rule electron pairing in p, d and f orbitals cannot occur until each orbital of a given subshell contains one electron each or is singly occupied.

State Hund’s Rule

It states that:

1. In a sublevel, each orbital is singly occupied before it is doubly occupied.

2. The electrons present in singly occupied orbitals possess identical spin.

Explanation of Hund’s Rule

The electrons enter an empty orbital before pairing up. The electrons repel each other as they are negatively charged. The electrons do not share orbitals to reduce repulsion.

When we consider the second rule, the spins of unpaired electrons in singly occupied orbitals are the same. The initial electrons spin in the sub-level decides what the spin of the other electrons would be

Explanation:

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Answer 2

Answer:

a) Pauli exclusion principle- No electron in an atom can have same values of all four quantum numbers i.e., an orbital can accommodate maximum 2 electrons with opposite spin.

b) Hund's rule - Pairing in degenerative orbital doesn't takes place until each orbital is signly filled.

Ex- In p orbital, first px, py, pz will be first singly filled then px will be full filled.

c) Afbau principle- The subshell with minimum energy is filled up first when this subshell obtained maximum quota of electrons then the next subshell of higher energy starts filling.

The sequence is 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6, 5s2..

d) n+l rule - The subshell with lowest n+l value is filled up first. When two or more subshell have same n+l value then the subshell with lowest value of n filled up first.

where, n - principal quantum number

p - azimuthal quantum number

Ex- Between 3d and 4p, 3d filled first

hope this will help you.