Anonymous
Apr 1
Explain VB THEORY, with it's suitable examples at least 5?
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Apr 1
VB theory, or Valence Bond theory, is a model used in chemistry to explain the bonding in molecules. It describes chemical bonding as the overlap of atomic orbitals to form covalent bonds. In this theory, electrons are localized between two atoms and are shared in the region of overlap of the atomic orbitals.
Here are five examples of VB theory in action:
1. Hydrogen molecule (H2): In the hydrogen molecule, two hydrogen atoms each contribute one electron to form a covalent bond. The two 1s atomic orbitals overlap to form a sigma bond.
2. Water molecule (H2O): In the water molecule, oxygen forms two sigma bonds with hydrogen atoms. The oxygen 2s and 2p orbitals overlap with the hydrogen 1s orbitals to form the covalent bonds.
3. Ethylene molecule (C2H4): In the ethylene molecule, the carbon atoms form a double bond. The carbon 2s and 2p orbitals overlap to form a sigma bond and a pi bond.
4. Ammonia molecule (NH3): In the ammonia molecule, nitrogen forms three sigma bonds with hydrogen atoms. The nitrogen 2s and 2p orbitals overlap with the hydrogen 1s orbitals to form the covalent bonds.
5. Methane molecule (CH4): In the methane molecule, carbon forms four sigma bonds with hydrogen atoms. The carbon 2s and 2p orbitals overlap with the hydrogen 1s orbitals to form the covalent bonds.
Overall, VB theory provides a simple and intuitive way to understand the formation of covalent bonds in molecules by considering the overlap of atomic orbitals.
Here are five examples of VB theory in action:
1. Hydrogen molecule (H2): In the hydrogen molecule, two hydrogen atoms each contribute one electron to form a covalent bond. The two 1s atomic orbitals overlap to form a sigma bond.
2. Water molecule (H2O): In the water molecule, oxygen forms two sigma bonds with hydrogen atoms. The oxygen 2s and 2p orbitals overlap with the hydrogen 1s orbitals to form the covalent bonds.
3. Ethylene molecule (C2H4): In the ethylene molecule, the carbon atoms form a double bond. The carbon 2s and 2p orbitals overlap to form a sigma bond and a pi bond.
4. Ammonia molecule (NH3): In the ammonia molecule, nitrogen forms three sigma bonds with hydrogen atoms. The nitrogen 2s and 2p orbitals overlap with the hydrogen 1s orbitals to form the covalent bonds.
5. Methane molecule (CH4): In the methane molecule, carbon forms four sigma bonds with hydrogen atoms. The carbon 2s and 2p orbitals overlap with the hydrogen 1s orbitals to form the covalent bonds.
Overall, VB theory provides a simple and intuitive way to understand the formation of covalent bonds in molecules by considering the overlap of atomic orbitals.
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