The relative stabilities of F 2 and F 2 + is to be compared using molecular orbital theory. Concept introduction: The combination of two atomic orbitals results in the formation of a bonding and an antibonding molecular orbital. Orbitals that lie on internuclear axis combine to form sigma σ molecular orbital, and orbitals parallel to each other combine to form π molecular orbitals. The molecular orbital formed by the combination of 1s orbital forms bonding molecular orbital designated as σ 1 s , and anti-bonding molecular orbital as σ ∗ 1 s . The 2s orbital forms corresponding molecular orbitals. Bond order is determined by subtracting the total number of antibonding electrons and the total number of bonding electrons and dividing the obtained number by two. Stability of molecules increases with increase in bond order.
The relative stabilities of F 2 and F 2 + is to be compared using molecular orbital theory. Concept introduction: The combination of two atomic orbitals results in the formation of a bonding and an antibonding molecular orbital. Orbitals that lie on internuclear axis combine to form sigma σ molecular orbital, and orbitals parallel to each other combine to form π molecular orbitals. The molecular orbital formed by the combination of 1s orbital forms bonding molecular orbital designated as σ 1 s , and anti-bonding molecular orbital as σ ∗ 1 s . The 2s orbital forms corresponding molecular orbitals. Bond order is determined by subtracting the total number of antibonding electrons and the total number of bonding electrons and dividing the obtained number by two. Stability of molecules increases with increase in bond order.
Solution Summary: The author explains that the relative stabilities of F_ 2 and > are to be compared using molecular orbital theory.
The relative stabilities of F2 and F2+ is to be compared using molecular orbital theory.
Concept introduction:
The combination of two atomic orbitals results in the formation of a bonding and an antibonding molecular orbital. Orbitals that lie on internuclear axis combine to form sigma σ
molecular orbital, and orbitals parallel to each other combine to form π
molecular orbitals.
The molecular orbital formed by the combination of 1s orbital forms bonding molecular orbital designated as σ1s, and anti-bonding molecular orbital as σ∗1s. The 2s orbital forms corresponding molecular orbitals.
Bond order is determined by subtracting the total number of antibonding electrons and the total number of bonding electrons and dividing the obtained number by two.
Stability of molecules increases with increase in bond order.
For the titration of a divalent metal ion (M2+) with EDTA, the stoichiometry of the reaction is typically:
1:1 (one mole of EDTA per mole of metal ion)
2:1 (two moles of EDTA per mole of metal ion)
1:2 (one mole of EDTA per two moles of metal ion)
None of the above
Please help me solve this reaction.
Indicate the products obtained by mixing 2,2-dimethylpropanal with acetaldehyde and sodium ethoxide in ethanol.
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Quantum Molecular Orbital Theory (PChem Lecture: LCAO and gerade ungerade orbitals); Author: Prof Melko;https://www.youtube.com/watch?v=l59CGEstSGU;License: Standard YouTube License, CC-BY