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Half-filled and fully-filled orbital orb...

Half-filled and fully-filled orbital orbitals are more stable

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To determine whether half-filled and fully-filled orbitals are more stable, we can analyze the concept step by step. ### Step 1: Understanding Orbital Filling - Orbitals can be filled with electrons according to the Aufbau principle, Hund's rule, and the Pauli exclusion principle. - Half-filled orbitals have one electron in each orbital of a subshell (e.g., p, d, f), while fully-filled orbitals have the maximum number of electrons allowed. ### Step 2: Example of Half-Filled and Fully-Filled Orbitals - Consider the p subshell, which can hold a maximum of 6 electrons (3 orbitals). ...
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STATEMENT-1: Half-filled and fully-filled degenerate orbitals are more stable. STATEMEHNT-2: Extra stabillity is due to the symmetrical distribution of electrons and exchange energy.

We know that fully filled and half filled orbitals are more stable. Can you write the electronic configuration of Cr(Z=24)?

Cu_((aq.))^+ has less stable nature than Cu_((aq.))^(2+) but Fe_((aq.))^(3+) is more stable than Fe_((aq.))^(2+) . Half-filled and completely filled, sub-shell are more stable.

Assertion: Cu^(2+) (aq) is less than Cu^(3+) (aq) but Fe^(3+) is more stable than Fe^(2+) (aq) Reason : Half filled and completely filled subshells are more stable

s orbital is more penetrating because

Assertion : The covalency of carbon is four in excited state. Reason : The four half-filled pure orbitals of carbon form same kind of bonds with an atom as those are with hybridised orbitals.

Assertion : The covalency of carbon is four in excited state. Reason : The four half-filled pure orbitals of carbon form same kind of bonds with an atom as those are with hybridised orbitals.

Assertion-The free gaseous Cr atom has six unpaired electrons. Reason-Half-filled s-orbital has greater stability.

L.C.A.O. Principle is involved in the formation of the molecular orbitals according to molecular orbital theory. The energy of the bonding molecular orbital is less than that of the combining atomic orbitals while that of the antibonding molecular orbitals while that of the order (B.O.)=1/2(N_(b)-N_(a)) helps in predicting formation of molecules/molecular ions, bond dissociation energy, stability and bond length. Only the molecules or ions with positive B.O. can be formed. These will be diamagnetic if all molecular orbitals are dilled and paramagnetic if one of more are half filled. The atomic orbitals at the time of overlap must have the same symmetry as well. In the formation of N_(2)^(+) from N_(2), the electron is removed from a

L.C.A.O. Principle is involved in the formation of the molecular orbitals according to molecular orbital theory. The energy of the bonding molecular orbital is less than that of the combining atomic orbitals while that of the antibonding molecular orbitals while that of the order (B.O.)=1/2(N_(b)-N_(a)) helps in predicting (i) formation of molecules/molecular ions, bond dissociation energy, stability and bond length. Only the molecules or ions with positive B.O. can be formed. These will be diamagnetic if all molecular orbitals are dilled and paramagnetic if one of more are half filled. The atomic orbitals at the time of overlap must have the same symmetry as well. The bond order (B.O.) in B_(2) molecule is:

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