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The statement are valid for :
  (I)    in filling a group of orbitals of equal  energy it is energetically preferable to assign electron to empty orbitals rather than pair them into a particular orbital.
 (II)    when two electrons are placed in two different orbitals, energy is lower if the spins are parallel.
  • a)
    Aufbau principle    
  • b)
    Hund’s rule
  • c)
    Pauli’s exclusion principle    
  • d)
    Uncertainty principle
Correct answer is option 'B'. Can you explain this answer?
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The statement are valid for :(I) in filling a group of orbitals of equ...
Only Hund’s rule discuss filling of electrons in degenerate orbitals.
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The statement are valid for :(I) in filling a group of orbitals of equ...
Explanation:

Hund's Rule:
- Hund's Rule states that when filling orbitals of equal energy (degenerate orbitals), electrons will fill empty orbitals first before pairing up.
- This is because electrons repel each other due to their negative charge, and by occupying separate orbitals, they can minimize repulsion and thus lower the overall energy of the system.

Parallel Spins:
- When two electrons are placed in two different orbitals, it is energetically more favorable for their spins to be parallel rather than paired with opposite spins.
- This is due to the Pauli Exclusion Principle, which states that no two electrons in an atom can have the same set of quantum numbers. By having parallel spins, the electrons can avoid being in the same quantum state and minimize their energy.
Therefore, the statement given in option (II) aligns with Hund's Rule, which explains the behavior of electrons in filling orbitals of equal energy and the significance of parallel spins in lowering the energy of the system.
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Read the following text and answer the following questions on the basis of the same:Band theory of solid:Consider that the Si or Ge crystal contains N atoms. Electrons of each atom will have discrete energies in different orbits. The electron energy will be same if all the atoms are isolated, i.e., separated from each other by a large distance. However, in a crystal, the atoms are close to each other (2 Å to 3 Å) and therefore the electrons interact with each other and also with the neighbouring atomic cores. The overlap (or interaction) will be more felt by the electrons in the outermost orbit while the inner orbit or core electron energies may remain unaffected. Therefore, for understanding electron energies in Si or Ge crystal, we need to consider the changes in the energies of the electrons in the outermost orbit only. For Si, the outermost orbit is the third orbit (n = 3), while for Ge it is the fourth orbit (n = 4). The number of electrons in the outermost orbit is 4 (2s and 2p electrons). Hence, the total number of outer electrons in the crystal is 4N. The maximum possible number of outer electrons in the orbit is 8 (2s + 6p electrons). So, out of the 4N electrons, 2N electrons are in the 2N s-states (orbital quantum number l = 0) and 2N electrons are in the available 6N p-states. Obviously, some p-electron states are empty. This is the case of well separated or isolated atoms.Q. The maximum possible electrons in an orbit is

The statement are valid for :(I) in filling a group of orbitals of equal energy it is energetically preferable to assign electron to empty orbitals rather than pair them into a particular orbital.(II) when two electrons are placed in two different orbitals, energy is lower if the spins are parallel.a)Aufbau principle b)Hund’s rulec)Pauli’s exclusion principle d)Uncertainty principleCorrect answer is option 'B'. Can you explain this answer?
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