Chemistry Practice Problems Orbital Overlap Practice Problems Solution: The double bonds are stronger and shorter than sin...

Solution: The double bonds are stronger and shorter than single bonds. For example, a C-C single bond has an average bond energy of 347 kJ/mole while a C=C double bond has an average bond energy of 611 kJ/mole. Use valence bond theory to explain why a double bond is not simply twice as strong as a single bond.

Problem

The double bonds are stronger and shorter than single bonds. For example, a C-C single bond has an average bond energy of 347 kJ/mole while a C=C double bond has an average bond energy of 611 kJ/mole. Use valence bond theory to explain why a double bond is not simply twice as strong as a single bond.

Solution

We have to explain why a double bond is not simply twice as strong as a single bond.


A chemical bond is a force of attraction that holds the atoms together to form a compound.


We will use the valence bond theory to explain the strengths of covalent bonds.

The valence electrons of atoms are contained in valence atomic orbitals.

The atomic orbitals overlap with other atomic orbitals to either form sigma bonds or pi bonds.

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