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How is bonding molecular orbital of hydr...

How is bonding molecular orbital of hydrogen different from the antibonding molecular orbital ?

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To explain how the bonding molecular orbital (BMO) of hydrogen differs from the antibonding molecular orbital (ABMO), we can break down the explanation into several key points: ### Step-by-Step Solution: 1. **Understanding Molecular Orbitals**: - In a diatomic hydrogen molecule (H₂), two hydrogen atoms combine their atomic orbitals to form molecular orbitals. The atomic orbitals involved are the 1s orbitals from each hydrogen atom. 2. **Formation of Molecular Orbitals**: - When the two 1s atomic orbitals combine, they form two types of molecular orbitals: a bonding molecular orbital (σ1s) and an antibonding molecular orbital (σ*1s). - The bonding molecular orbital (σ1s) is formed when the wave functions of the two atomic orbitals constructively interfere, leading to a region of increased electron density between the two nuclei. 3. **Electron Configuration**: - In the case of H₂, there are a total of two electrons. These electrons will occupy the lower energy bonding molecular orbital (σ1s). - The electron configuration for H₂ can be written as: σ1s², indicating that both electrons are in the bonding orbital. 4. **Energy Levels**: - The bonding molecular orbital (σ1s) has lower energy compared to the antibonding molecular orbital (σ*1s). This is because the bonding orbital stabilizes the molecule by increasing electron density between the nuclei. - Conversely, the antibonding molecular orbital (σ*1s) has higher energy due to the destructive interference of the wave functions, which results in a node between the nuclei where electron density is low. 5. **Electron Presence**: - The bonding molecular orbital (σ1s) contains two electrons, which contribute to the bond formation between the hydrogen atoms. - The antibonding molecular orbital (σ*1s) is unoccupied in the case of H₂, meaning it has zero electrons. ### Summary of Differences: - **Energy**: The bonding molecular orbital (σ1s) has lower energy, while the antibonding molecular orbital (σ*1s) has higher energy. - **Electron Occupancy**: The bonding molecular orbital contains two electrons (σ1s²), whereas the antibonding molecular orbital has zero electrons (σ*1s⁰).
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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:

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. In the homonuclear molecule which of the following sets of M.O. orbitals are degenerate ?

L.C.A.O. Principle is involved in the formationof the molecular orbitals according ot molecular orbital theory. The energy of the bonding molecular orbital is less than that of thecombining 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 dossociation 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 prbitals at the time of overlap must have the same symmetry as well. Bond arder is :

Explain bonding and antibonding molecular orbitals.

A bonding molecular orbital has lesser energy than the corresponding antibonding molecular orbital. Justify

According to molecular orbital theory,

How will your differentiate between atomic and molecular orbitals ?

Describe molecular orbital. How is it different from an atomic orbital?

According to MOT, two atomic orbitals overlap relsulting in the formation of molecular orbital. Number of atomic orbitals overlapping together is equal to the molecular orbital formed. The two atomic orbital formed by LCAO (linear combination of atomic orbital) in the same phase or in the different phase are known as bonding and antibonding molecular orbitals respectively. theenergy of bonding molecular orbital is less than that of the pure atomic orbital by an amount Delta . this is known as the stabilization energy. the energy of antibonding molecular orbital is increased by 'Delta' (destabilisation energy) The bond order of N_(2)^(-) is equal to that of

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