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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.