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Q: What is hybridization?
A: The mixing of atomic orbitals to form hybrid orbitals for bonding.
Q: What determines molecular polarity?
A: Electronegativity differences & molecular shape
Q: What shapes are typically nonpolar if all outer atoms are the same?
A: Linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral
Q: What are the three types of intermolecular forces?
A: London Dispersion, Dipole-Dipole, Hydrogen Bonding
a. London Dispersion Forces (LDFs)
Q: What are London Dispersion Forces?
A: Weak forces caused by temporary electron shifts. Present in all molecules, but strongest in large nonpolar molecules.
Q: What is an example of a molecule with only London Dispersion Forces?
A: COâ‚‚ (nonpolar molecule)
b. Dipole-Dipole Forces
Q: What are Dipole-Dipole Forces?
A: Attractions between permanent dipoles in polar molecules.
Q: What is an example of a molecule with Dipole-Dipole Forces?
A: HCl (polar molecule)
c. Hydrogen Bonding
Q: What is Hydrogen Bonding?
A: A strong dipole-dipole attraction between H and N, O, or F.
Q: What is an example of a molecule with Hydrogen Bonding?
A: Hâ‚‚O (water)
Q: Which intermolecular force is the weakest?
A: London Dispersion Forces
Q: Which intermolecular force is the strongest?
A: Hydrogen Bonding
A: Valence Shell Electron Pair Repulsion (VSEPR) Theory states that electron pairs around a central atom arrange themselves to minimize repulsion, determining the molecular shape.
Q: What is the main principle of VSEPR Theory?
A: Electron pairs (bonding and lone pairs) repel each other and adopt a geometry that maximizes distance between them.
Q: How does VSEPR Theory help predict molecular shape?
A: By counting the number of bonding and lone electron pairs, you can determine the molecular geometry of a molecule.