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Questions and Answers
How does constructive interference of orbitals affect electron probability?
How does constructive interference of orbitals affect electron probability?
- Increases electron probability (correct)
- Does not affect electron probability
- Decreases electron probability
- Locks electrons in place
What is the main difference between sigma and pi bonds?
What is the main difference between sigma and pi bonds?
- Sigma bonds are linear while pi bonds are not (correct)
- Sigma bonds are weaker than pi bonds
- Pi bonds are stronger than sigma bonds
- Pi bonds involve only s-orbitals
How is bond order calculated in molecular orbital theory?
How is bond order calculated in molecular orbital theory?
- Dividing total electrons by the number of atoms
- Subtracting electrons in bonding orbitals
- Dividing by two after subtracting anti-bonding electrons (correct)
- Adding electrons in anti-bonding orbitals
In what situation do atomic orbitals not overlap to form molecular orbitals?
In what situation do atomic orbitals not overlap to form molecular orbitals?
What is the bond order for a molecule with 10 bonding electrons and 8 anti-bonding electrons?
What is the bond order for a molecule with 10 bonding electrons and 8 anti-bonding electrons?
What is the primary difference between valence bond theory and molecular orbital theory?
What is the primary difference between valence bond theory and molecular orbital theory?
How does molecular orbital theory differ from valence bond theory in terms of electron interactions?
How does molecular orbital theory differ from valence bond theory in terms of electron interactions?
What is the primary basis of molecular orbital theory?
What is the primary basis of molecular orbital theory?
How are molecular orbitals different from atomic orbitals?
How are molecular orbitals different from atomic orbitals?
Why does molecular orbital theory provide a more comprehensive view than valence bond theory?
Why does molecular orbital theory provide a more comprehensive view than valence bond theory?
What does the energy gap between bonding and anti-bonding orbitals determine?
What does the energy gap between bonding and anti-bonding orbitals determine?
In molecular orbital theory, why does a bond appear weaker when bonding and anti-bonding orbitals are close in energy?
In molecular orbital theory, why does a bond appear weaker when bonding and anti-bonding orbitals are close in energy?
How are bonds between atoms with different electronegativities represented in MO diagrams?
How are bonds between atoms with different electronegativities represented in MO diagrams?
What characteristic of molecular orbitals allows for easy determination of bond order?
What characteristic of molecular orbitals allows for easy determination of bond order?
How does a polar bond differ from a covalent bond in terms of electron density?
How does a polar bond differ from a covalent bond in terms of electron density?
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Study Notes
Molecular Orbital Theory vs Valence Bond Theory
- Molecular orbital theory provides a more comprehensive view than valence bond theory
- The primary difference between the two theories is how they describe electron interactions
- Valence bond theory focuses on electron pairing between atoms, whereas molecular orbital theory considers the entire molecule as a whole
Bond Order and Molecular Orbitals
- Bond order is calculated by subtracting the number of anti-bonding electrons from the number of bonding electrons and dividing by 2
- For a molecule with 10 bonding electrons and 8 anti-bonding electrons, the bond order is 1
- Molecular orbitals are different from atomic orbitals as they are delocalized over the entire molecule
Sigma and Pi Bonds
- The main difference between sigma and pi bonds is the orientation of the overlap of atomic orbitals
- Sigma bonds have end-to-end overlap, while pi bonds have side-by-side overlap
Electron Probability and Interference
- Constructive interference of orbitals increases electron probability between the nuclei of bonded atoms
- Destructive interference decreases electron probability
MO Diagrams and Electronegativity
- Bonds between atoms with different electronegativities are represented in MO diagrams as polar bonds
- Polar bonds have unequal electron density between atoms
Energy Gap and Bond Strength
- The energy gap between bonding and anti-bonding orbitals determines the strength of a bond
- When bonding and anti-bonding orbitals are close in energy, the bond appears weaker
- A larger energy gap results in a stronger bond
Characteristics of Molecular Orbitals
- Molecular orbitals allow for easy determination of bond order
- Molecular orbitals are delocalized over the entire molecule, unlike atomic orbitals which are localized between atoms
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