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.
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.
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Orbital Overlap concept. If you need more Orbital Overlap practice, you can also practice Orbital Overlap practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Jurisch's class at UIC.