Question

Explain bonding and antibonding molecular orbitals.
(explain in 150 words)

Answer 1

Hey!
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★Molecular Orbital ★
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=> Molecular Orbital are formed by the combination of atomic orbital of definite energies . Based on type of bonding , Molecular Orbital are classified as -

• Bonding Molecular Orbital

• Anti Bonding Molecular Orbital


◼Bonding Molecular Orbital -

→ These are formed by the combination of atomic orbital with less energy and greater stability .

→ These are formed by the addition overlapping of orbital .

→The electron contribute to attraction in the orbital.

→They are more stable due to release of less energy.



◼Anti Bonding Molecular Orbital -

→ These are formed by the combination of atomic orbital with more energy and less stability .

→ They are formed by subtraction overlapping of orbital.

→ The electrons contribute to repulsion in the orbital.

→ They are less stable because of greater energy released .


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Answer 2

Hi
Here is the answer


Hybridization is a simple model that deals with mixing orbitals to from new, hybridized, orbitals. This is part of the valence bond theory and helps explain bonds formed, the length of bonds, and bond energies; however, this does not explain molecular geometry very well.

sp An example of this is acetylene (C2H2). This combines one s orbital with one p orbital. This means that the s and p characteristics are equal.
sp2 An example of this is ethylene (C2H4). This is the combination of one s orbital and two p orbitals.
sp3 An example of this is methane (CH4). This is the combination of one s orbital and three p orbitals.

If you add the exponents of the hybridized orbitals, you get the amount of sigma bonds associated with that bond. The sp2 hybridized orbital has one p orbitals that is not hybridized and so it can form a pi bond. This means that sp2 orbitals allow for the formation of a double bond. Also, sp hybridized orbitals form a triple bond.
Antibonding vs. Bonding Orbitals

Electrons that spend most of their time between the nuclei of two atoms are placed into the bonding orbitals, and electrons that spend most of their time outside the nuclei of two atoms are placed into antibonding orbitals. This is because there is an increasing in electron density between the nuclei in bonding orbitals, and a decreasing in electron density in antibonding orbitals (Chang 459). Placing an electron in the bonding orbital stabilizes the molecule because it is in between the two nuclei. Conversely, placing electrons into the antibonding orbitals will decrease the stability of the molecule. Electrons will fill according to the energy levels of the orbitals. They will first fill the lower energy orbitals, and then they will fill the higher energy orbitals. If a bond order of zero is obtained, that means that the molecule is too unstable and so it will not exist.

Hope it helps